Process for producing alkali hydroxide or alkaline earth oxide employing a weak acid intermediate

Abstract

The present application pertains to processes producing oxides using a weak acid intermediate. In one embodiment a material comprising calcium carbonate is reacted, with a solution comprising aqueous carboxylic acid to form a gas comprising carbon dioxide and a solution comprising aqueous calcium carboxylate. The solution comprising aqueous calcium carboxylate is reacted with sodium sulfate to form a solution comprising aqueous sodium carboxylate and a solid comprising calcium sulfate. The solution, comprising aqueous sodium carboxylate is reacted with sulfur dioxide to form sodium sulfite and an aqueous carboxylic acid. The sodium sulfite is separated from said aqueous carboxylic acid and reacted to form a solid comprising calcium sulfite which is decomposed to form calcium oxide and sulfur dioxide.

Description

PROCESS FOR PRODUCING ALKALI HYDROXIDE OR ALKALINE EARTH OXIDE EMPLOYING A WEAK ACID INTERMEDIATECROSS-REFERENCE TO RELATED APPLICATIONS

[0001] For PCT purposes this application claims priority to U.S. Provisional Application 63 / 342,870 filed .May 17, 2022 which application is incorporated herein by reference.

[0002] For U.S. purposes this application claims priority to U.S. Provisional Application 63 / 342,870 tiled May 17, 2022 which application is Incorporated herein by reference.

[0003] For U.S. purposes the present application also claims priority to pending U.S. Ser. No. 18 / 087,432 which is a continuation of U.S: Ser. No. 17 / 744,161 filed on May 13, 2022 issuing as U.S. Pat. No. 1 1,542,219 on Jan. 3, 2023. U.S. Ser. No. 17 / 744, 161 was a continuation-in-part of U.S. application Ser. No. 17 / 732,808 filed Apr 29, 2022 which application is a continuation-in-part of U.S. application Ser. No. 17 / 590,483 filed Feb. I, 2022 which application is a continuation of U.S. application Ser. No. 17 / 243,714 filed Apr. 29, 2021 issued as U.S . Pat. No. 11,236,033 which application is a continuation-in-part of U.S. application Ser. No. 16 / 944,850 filed Jul. 31, 2020 issued as U.S. Pat. No. 1 1 ,034,619 which application claims priority from U.S. Provisional Application No. 62 / 895,557 filed Sep. 4, 2019 and U.S. Provisional Application No. 63 / 042,397 filed Jun. 22, 2020 and U.S. Provisional Application No. 62 / 890,254 filed Aug. 22, 2019. The present application also claims priority to U.S. Provisional Application No. 63 / 188,275 filed May 13, 2021.

[0004] The above described continuation which is U.S. application Ser. No. 17 / 590,483 filed Feb. 1 , 2022 also claims priority to U.S. Provisional Application No. 63 / 147,286 filed Feb. 9, 2021; U.S. Provisional Application No. 63 / 153,461 filed Feb. 25, 2021; U.S. Provisional Application No. 63 / 157,847 filed Mar. 8, 2021; U.S.. Provisional Application No. 63 / 163, 993 filed Mar. 22, 2021 ; and U.S. Provisional Application No. 63 / 179,822 filed Apr. 26, 2021. All of the above applications are incorporated herein by reference.BACKGROUND AND SUMMARY

[0005] Sodium hydroxide is generally produced using the chlor-alkali process, which is energy intensive, requires rare metal anodes and cathodes, and produces hydrochloric acid, which has a limited market and cannot be discharged into the environment. Production of sodium hydroxide in prior art is energy intensive, CO2emissions intensive; and expensive. Additionally, prior art production of sodium hydroxide may not be employed in CO2removal, or may not be added to a sea for deacidification or CO2removal, because they areenergy intensive, CO2emissions intensive, expensive, and environmentally damaging. Commercial applications of hydrochloric acid often involve employing hydrochloric acid in a reaction with, a carbonate salt, which may result in the release of CO2and may counter any CO2emissions reduction benefi t Additionally, if hydrochloric acid is released into the environment, it will react with carbonate or bicarbonate salts present in the environment, emiting carbon dioxide and acidifying water bodies, such as the ocean. Sodium hydroxide is an essential chemical employed in a wide range of applications, which include, tor example, pulp & paper production, lithium processing, soap production, rayon production, aluminum refining, io name a few. Production of sodium hydroxide in prior art is energy intensive, CO2emissions intensive, and expensive. Reducing the energy, cost, and emissions associated with the production of sodium hydroxide would greatly benefit the economy and environment There .is a significant need for a low energy consumption, low CO2emissions, environmentally friendly process for producing sodium hydroxide.

[0006] Production of calcium oxide, or calcium hydroxide, or cement klinker in prior art produces CO2emissions, which may be difficult or expensive to capture. It may be highly desirable to develop a calcium oxide, or calcium hydroxide, or cement klinker production process which does not produce CO2emissions and / or inherently produces high purity, captured CO2.

[0007] Some embodimen t s of the present invention may pertain to low carbon emissions, or low energy consumption, or carbon negative production of sodium hydroxide, or sodium carbonate, or sodi um bicarbonate, or sodium sulfite, or sodium bisulfite, or gypsum, or alkaline-earth sulfate, or alkali hydroxide, or alkali carbonate, or alkali bicarbonate, or alkali sulfite. Some embodiments of the present invention may enable ultra-low CO2emissions prod uction of sodium hydroxide with calcium sulfate as the side product. Calcium sulfate comprises a solid, is minimally soluble in water, is non-toxic, is not dangerous for the environment, and has a multi-billion metric ton per year market in gypsum wallboard, concrete aggregates, fireproofing, plaster, building materials, and other applications. Some embodiments of the present invention may be capable of scaling to greater than 1 billion ton per year COt emissions reduction, or carbon removal, or a combination thereof. Some embodiments of the present invention may enable highly scalable, environmentally beneficial systems and methods for ocean deacidification, which are capable of sealing to meaningfully increase ocean pH, rejuvenate marine ecosystems, and permanently sequester carbon dioxide. Additionally some embodiments may lower the required cost and energy consumption ofalkali hydroxides, alkali carbonates, and alkali bicarbonales. Some embodiments may be employ equipment comprising abundant and recyclable materials.

[0008] Some embodiments of the present invention may pertain to low carbon emissions, or low energy consumption, or carbon negative production of calcium oxide, or calcium hydroxide, or calcium carbonate, or magnesium oxide, or magnesium hydroxide, or cement, or cement klinker, or Portland cement, or magnesium carbonate, or alkaline earth oxide, or alkaline earth hydroxide, or alkaline earth carbonate or any combination thereof. Some embodiments of the present invention may enable ultra- low CO2, emissions production of calcium oxide, or magnesium oxide, or cement. Some embodiments may comprise a CO2capture process, or a CO2air capture process, or CO2removal process, or a CO2conversion process, or a CO2separation process, or a process for recovering or separating CO2, from solutions comprising carbonate, or bicarbonate, or any combination thereof. Some embodiments of the present invention may enable calcium oxide or cement production with inherent production of high purity, high pressure carbon dioxide in the nature of the process, which may reduce the cost and energy required to produce low emissions or zero emissions calcium oxide or cement. Some embodiments may be employ equipment comprising abundant and recyclable materials.

[0009] Advantages of some embodiments include lower energy consumption, lower cost, or lower CO2emissions, CO2emissions negative outputs, or application in carbon dioxide removal, or no strong acid products, or abundant materials, or global scalability.BRIEF FIGURE DESCRIPTIONS

[0010] Figure 1 : Process for producing calcium oxide and captured carbon dioxide with carboxylic acid and sulfur dioxide intermediates.

[0011] Figure 2A: Process for producing calcium oxide and weak acid derivative employing carboxylic acid and sulfur dioxide intermediates.

[0012] Figure 2B: Process for producing calcium oxide and weak acid derivative employing carboxylic acid and sulfur dioxide intermediates.

[0013] Figure 3A: Process for producing magnesium oxide and weak acid derivati ve employing carboxylic acid and sulfur dioxide intermediates.

[0014] Figure 3B: Process for producing magnesium oxide and weak acid derivative employing carboxylic acid and sulfur dioxide intermediates.

[0015] Figure 4A: Process for producing alkaline earth oxide and captured carbon dioxide employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0016] Figure 4B: Process for producing alkaline earth oxide and captured carbon dioxide employing carboxylic acid, alkali, and sulfur dioxide Intermediates.

[0017] Figure 4C: Process for producing alkaline earth oxide and captured carbon dioxide employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0018] Figure 5A: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0019] Figure 5B: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates

[0020] Figure 5C; Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0021] Figure 5D: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0022] Figure 5E: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0023] Figure 5F: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0024] Figure 6A: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0025] Figure 6B: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates.

[0026] Figure 7A: Process for producing alkaline earth oxide and weak acid deri vative employing carboxylic acid, alkali, and sulfur dioxide intermediates with membrane separation of at least a portion of alkali sulfite.

[0027] Figure 7B: Process for producing alkaline earth oxide and weak acid deri vative employing carboxylic acid, alkali, and sulfur dioxide intermediates with membrane separation of at least a portion of alkali sulfite.

[0028] Figure 8; Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali, and sulfur dioxide intermediates with membrane separation of at least a portion of alkali sulfite.

[0029] Figure 9A: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0030] Figure 9B; Precess for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0031] Figure 9C: Process for producing alkali hydroxide from alkali sulfate using carboxylic- acid and sulfur dioxide intermediates.

[0032] Figure 9D: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0033] Figure 10A; Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0934] Figure 10B: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0035] Figure 10C; Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0036] Figure 10D: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0037] Figure 10E; Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0038] Figure 10F: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0039] Figure 11 A: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0040] Figure 11B; Process for producing alkali hydroxide from alkali sulfate using carboxylie acid and sulfur dioxide intermediates.

[0041] Figure 11C: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0042] Figure 12A: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0043] Figure .12B: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0044] Figure 12C: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0045] Figure 13 A: Process for producing alkali carbonate and removing or capturing or convening CO2from alkali sulfete employing acid, such as carboxylic acid, and sulfur dioxide intermediates.

[0046] Figure 138: Process for producing alkali carbonate and removing or capturing or converting CO2, from alkali sulfate employing acid, such as carboxylic acid, and sulfur dioxide intermediates,

[0047] Figure BC: Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfete employing acid, such as carboxylic acid, and sulfur dioxide intermediates.

[0048] Figure 13D; Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfate employing acid, such as carboxylic acid, and sulfur diox ide intermediates.

[0049] Figure 13E: Process for producing alkali carbonate and -removing or capturing or converting CO2from alkali sulfate employing acid, such as carboxylic acid, and sulfur dioxide intermediates.

[0050] Figure 13 F: Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfate employing acid, such as carboxylic acid, and sulfur dioxide intermediates.

[0051] Figure 14A: Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfate employing carboxylic acid and sulfur dioxide Intermediates.

[0052] Figure 14B; Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfate employing carboxylic acid and sulfur dioxide intermediates.

[0053] Figure 14C: Process for producing alkali carbonate and removing or capturing or converting CO2from alkali sulfate employing carboxylic acid and sulfur dioxide intermediates.

[0054] Figure 15 A: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0055] Figure 15B: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0056] Figure 15C: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia, or ammonium), and sulfur dioxide intermediates,

[0057] Figure 16A: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0058] Figure 16B: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0059] Figure 16C: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0060] Figure 17A; Process for producing alkaline earth oxide and weak acid deri vative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates,

[0061] Figure 17B: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic aeid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0062] Figure 17C: Process for producing alkaline earth oxide and weak acid derivative employing carboxy lie acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0063] Figure 18; Process for producing alkaline earth oxide and weak acid derivative employing catboxylic acid, alkali (such as ammonia or aranionium), and sulfur dioxide intermediates.

[0064] Figure 19: Process for producing alkaline earth oxide and weak acid derivative employing carboxylic acid, alkali (such as ammonia or ammonium), and sulfur dioxide intermediates.

[0065] Figure 20A; Process for producing or recovering ammonia from ammonium sulfate

[0066] Figure 20B; Process for producing or recovering ammonia from ammonium sulfate

[0067] Figure 20C: Process for producing or recovering ammonia from ammonium sulfate

[0068] Figure 21 A; Process for producing or recovering ammonia from ammonium sulfate

[0069] Figure 21 B: Process for producing or recovering ammonia from ammonium sulfate

[0070] Figure 21 C: Process for producing or recovering ammonia from ammonium sulfate

[0071] Figure 22 A: Process for producing or recovering ammonia from ammonium sulfate

[0072] Figure 22B: Process for producing or recovering ammonia from ammonium sulfate

[0073] Figure 22C: Process for producing or recovering ammonia from ammonium sulfate

[0074] Figure 23A: Process for producing or recovering ammonia from ammonium sulfate

[0075] Figure 23B: Process for producing or recovering ammonia from ammonium sulfate

[0076] Figure 23C : Process for producing or recovering ammonia from ammonium sulfate

[0077] Figure 24: Process for thremally decomposing or calcining alkaline earth sulfite to form alkaline earth oxide and sulfur dioxide and / or absorbing sulfur dioxide employing a recirculating carrier gas to, for example, enable use of zero emissions heat and / or enable low diatomic oxygen concentrations

[0078] Figure 25: Process for thermally decomposing or calcining alkaline earth sulfite to form alkaline earth oxide and sulfur dioxide and / or absorbing sulfur dioxide employing a recirculating carrier gas

[0079] Figure 26 A: Process for producing alkali hydroxide using carboxylic acid and sulfur dioxide intermediates from alkali chloride.

[0080] Figure 26B: Process for producing alkali hydroxide using carboxylic acid and sulfur dioxide intermediates from alkali chloride.

[0081] Figure 26C: Process for producing alkali hydroxide using carboxylic acid and sulfur dioxide intermediates from alkali chloride.

[0082] Figure 26D: Process for producing alkali hydroxide using carboxylic acid and sulfur dioxide intermediates from alkali chloride.

[0083] Figure 27: Process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide intermediates

[0084] Figure 28A: Process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide intermediates

[0085] Figure 288: Process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide intermediates

[0086] Figure 28C: Process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide intermediates

[0087] Figure 29: Process for producing alkali sulfate and capturing CO2employing alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide intermediates

[0088] Figure 30: Process for producing alkali sulfate, capturing CO2, and / or producing urea employing alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide

[0089] Figure 31 A; Process for producing alkali hydroxide from alkali sulfite employing acid and sulfur dioxide intermediates

[0090] Figure 3 IB: Process for producing alkali hydroxide from alkali sulfite employing acid and sulfur dioxide intermediates

[0091] Figure 31C: Process for producing alkali hydroxide from alkali sulfite employing acid and sulfur dioxide intermediates

[0092] Figure 32A: Process for absorbing or reacting sulfrir dioxide within alkali acid- anion, such as alkali carboxylate, in a manner which may minimize or reduce potential residual vapor in remaining gases.

[0093] Figure 32B: Process for absorbing or reacting sulfur dioxide within alkali acid- anion, such as alkali carboxylate, in a manner which may minimize or reduce potential residual vapor in remaining gases.

[0094] Figure 33: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide intermediates.

[0095] Figure 34: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid, sulfur dioxide, and carbon dioxide intermediates.

[0096] Figure 35: Process for producing alkali hydroxide from alkali sulfate usingcarboxylic acid, sulfur dioxide, and carbon dioxide intermediates.

[0097] Figure 36A: Process for producing alkali bicarbonate or carbonate from alkali sulfate using carboxylic acid and sulfur dioxide intermediates and carbon dioxide input and intermediate.

[0098] Figure 37: Process for producing alkali hydroxide from alkali sulfate using carboxylie acid, magnesium, sulfur dioxide, and carbon dioxide intermediates.

[0099] Figure 38: Process for producing alkali hydroxide from alkali sulfate using carboxylic acid, magnesium, sulfur dioxide, and carbon dioxide intermediates.

[0100] Figure 39A: Process for producing alkali bicarbonate or carbonate from alkali sulfate using carboxylic acid and sulfur dioxide intermediates and carbon dioxide input and intermediate.

[0101] Figure 39B: Process for producing alkali bicarbonate or carbonate from alkali sulfate using carboxylic acid and sulfur dioxide intermediates and carbon dioxide input and intermediate.DETAILED DESCRIPTIONEXAMPLE CHEMISTRY

[0102] Example 1: Proces for Producing Calcium Oxideor Cement or Clink

[0103] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid, which may comprise, inchiding, but not limited fo, one or more or any combination of the following:• CaCO3(s or aq) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + CO3(g)• Calcium Silicate(s) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + Silicon Dioxide(s)• CaS(s) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + H2S(g)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq)

[0104] Note: Residual solids or undissolved solids, such as silicon dioxide or other iindissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0105] Note: CO2(g) may comprise captured CO2.

[0106] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesi um.

[0107] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[0108] (2) Ca(CH3COO)2(aq) + SO2(g (1 or aq) H2O(1 or aq) -> CaSO2(s) + 2CH3COOH(aq)

[0109] Note: CaSO3(s) may be separated using a solid-liquid separation.

[0110] Note: In some embodiments, SO2(g) may comprise other gases in addition toSO2(g). In some embodiments, the remaining gases after the absorption or reaction of at least a portion of SO2(g) may comprise a portion of acetic acid vapor. In some embodiments, the remaining gases after the absorption or reaction of at least a portion of SO2(g) may comprise at least a portion of acetic acid vapor, which may comprise acetic acid evaporated from theproducts of reaction step '(2)'. In some embodiments, remaining gases comprising at least aportion of acetic acid vapor may be contacted with Ca(CH3COO)2(aq) before the reaction wi th SO2(g), which may enable at least a portion of acetic acid vapor to be absorbed in the Ca(CH3COO)2(aq) and / or removed from the remaining gases. In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth hydroxide, or alkaline earth hydroxide ~ water slurry, or alkaline earth hydroxide - water suspension, or alkaline earth hydroxide - water solution, or water, of alkali carbonate, or alkali bicarbonate, or alkali hydroxide.Note: In some embodiments, residual aqueous magnesium sulfite may be present in the ‘2 CH3COOH(aq)'. In some embodiments, the residual aqueous magnesium sulfite may remain in the ‘2 CH3COOH(aq)’ transferred to reaction '(I)’ from, for example, reaction ‘(2)’, In some embodiments, at least a portion of the aqueous magnesium sulfite may remain in the ‘2 CH3COOH(aq)’ solution transferred to reaction ‘(I )’ from reaction ‘(2)7. Additional magnesium sulfite above the solubility limits of magnesium sulfite in the solution may precipitate or co-precipitate during the reaction of Ca(CH3COO)2(aq) or Mg(CH3COO)2(aq) with SO2(g or aq), or sulfite, or bisulfite, or any combination thereof.

[0112] Note: In some embodiments, residual aqueous magnesium sulfite may be present in the ‘2 CH3COOH(aq)’. In some embodiments, a portion of the residual aqueous magnesium sulfite may be concaitated and / or separated. using, including, but not limited to, one or more, or any combination of the following: heating, or cool ing, or reverse osmos is, or membrane based process, or precipitation, or electrodialysis, or forward osmosis, or any combination thereof. For example, the residual aqueous magnesium sulfite may be separated by concentrating the magnesium sulfite using reverse osmosis or nanofiltration, wherein the pore si ze or properties of the membrane may enable the permeation of at least a portion of the acetic acid and the rejection of at least a portion of magnesium sulfite, and / or cooling the resulting concentrated magnesium sulfite solution to produce at least a portion of a magnesium sulfite precipitate,

[0113] (3) CaSO3(s) -> CaO(s) + SO2(g)

[0114] Note: “(3)’ may comprise calcining CaSOfrs), which may employ a kiln,

[0115] Note: CaSO3(s) may be dried, or dehydrated, or both before or during '(3)'.

[0116] Example 2 : Process for Producing Magnesium Oxide or Cement or Clinker

[0117] (l) .React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• MgCO3(s or aq) + 2CH3COOH(aq) -> Mg(CH3COO)2(aq) + CO2(g)• Magnesium Silicate(s) + 2 CH3COOH(aq) -> Mg(CH3COO2(aq) + Silicon Dioxide(s)• MgS(s) + 2 CH3COOH(aq) 4- MgCH3COO)3(aq) + H2S(g)• Magnesium(Weak Acid Anion) + 2 CH3COOH(aq) -> Mg(CH,COO)’(aq) + Weak AcicKs, or g, or 1, or aq)

[0118] Note: Residual solids or undtssolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0119] Note: In some embodiments, 2 CH3COOH(aq) may comprise at least a portion of MgSO3(aq), which may be referred to as residual MgSO3(aq).

[0120] (2) Mg(CTliCOO) ;(aq) + SO2(g (1 or aq +) H2O(1 (1 or aq -♦) MgSO3( s) + 2CH3COOH(aq)

[0121] Note: MgSO3(s) may be separated using a solid-liquid separation.

[0122] Nate: Residual MgSO3(aq) may be present in the 2 CH3COOH(aq) solution.

[0123] (3) MgSO3(s) MgO(s) + SO2(g)

[0124] Note: ‘(3) ' may comprise calcining MgSO3(s), which may employ a kiln.

[0125] Note: MgSO3(s) may be dried, or dehydrated, or both before or during" (3)'.

[0126] Example 3: Process for Producing Caleiam Oxide or Cement or Clinker withAlkali Intermediate

[0127] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCO3(s or aq) 2 CH3COOH(aq) Ca(CH3COO)2(aq)+ CO2(g)• Calcium Siiicate(s) + 2 CH3COOH(aq) Ca(CH3COO)2(q)( + Silicon Dioxide(s)• CaS(s) + 2 CH3COOH(aq) Ca(CH3COO')2(aq) + H2S(g)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq)

[0128] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated .ftom the liquid solution using a solid-liquid separation.

[0129] Note: If CO2(g) is produced, it may be desirable for said CO2(g) to be produced at a high partial pressure CO2(g), or purity CO2l'g), or to comprise captured COft'g).

[0130] (2) Ca(CH3COO)2(aq) + Na2SO3(s (1 or aq) -> 2 NaCH3COO(aq) + CaSO3(s)

[0131] Note: CaSO3(s) may be separated using a solid-liquid separation.

[0132] Note: In some embodiments, Na2SO3(s or aq) may comprise a solid comprising sodium sulfite, which may be added to or dissolved in a solution comprising calcium acetate.

[0133] Note: In some embodiments, Na2SO3(s or aq) may comprising an aqueous solution comprising sodium sulfite and acetic acid.

[0134] (3) 2 NaCH3COO(aq) + SO2( g or aq) + H3O(l (1 or aq) Na2SO3(aq) + 2CH3COO(aq)

[0135] Note: In some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[0136] (4) Na2SO3(aq) + 2 CH3COOH(aq) -> 2 CH3COOH(aq or 1) + Na2SO3(s)

[0137] Note; CH3COOH may be more soluble in water than Na2SO3, In some embodiments, Na2SO3may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation. or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0138] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments, CH3COOH may evaporate with, water vapor and / or condense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[0139] Note: In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step ‘(4)' . In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof.s

[0140] Note: Na2SO3(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0141] Note: In some embodiments, a feed solution comprising sodium sulfite and acetic acid may be evaporated, wherein a portion of acetic acid and water vapor evaporate and / or are condensed to form an a separated acetic acid solution, and / or the remaining solution comprises aqueous acetic acid and a higher concentration of sodium sulfite than in the concentration of sodium sulfite in the feed solution.

[0142] (5) CaSO3(s) → CaO(s) + SO2(g)

[0143] Note: (5)’ may comprise calcining CaSO3(s), which may employ a kiln.

[0144] Note: CaSOa(s) may be dried, or dehydrated, or both before, or during ‘(5)’.

[0145] Note: In some embodiments, it may be preferred or desired to react SO2(g) withNa CH3COO(aq) to form Na2SOfoaq), and then react Na2SOa with Ca(CH3COO)2(aq) to form CaSO3(s) because, for example, including, but not limited to, one or more or any combination of the following potential benefits:• In some embodiments, i t may be desirable to absorb SO2(g) in an absorption column. Precipitate formation can be problematic in an absorption column due to, for example, including, but not limited to, precipitate clogging packing material, or plates, or interfering with gas flows, or interfering with liquid flows, or formingscaling, or any combination thereof The reaction of Ca(CH3COO)2(ac|) with SO3(g) may form a precipitate comprising CaSO3(s), which may be challenging in some absorption columns or a gas absorption processes. The reaction of NaCH3COO(aq) with SO2(g) may, if desired, the salt may mostly remain at an aqueous or liquid phase throughout the reaction, because, for example, Na2.SO3may be soluble in water, which may be desirable in an absorption column,• In some embodiments, if the SO2f g) comprises gases in addition to SO2(g), acetic acid vapor may be present in the remaining gases during or after the reaction of SO2(g) with an acetate salt. If SO2(g) is contacted with NaCH3COO(aq), which may form aqueous phase Na2SO2(aq) and / or acetic acid, the reactor or absorption column may be configured such that NaCH3COO (aq) entering the reactor or absorption column absorbs or recovers at least a portion of acetic acid vapor from the remaining gases. If SO2(g) is contacted with NaCH3COO(aq), which may form aqueous phase Na2SO2(aq) and / or acetic acid, the reactor or absorption column may be configured such that NaCH3COO(aq) entering the reactor or absorption column absorbs or recovers at least a portion of acetic acid vapor from the remaining gases before or while NaCH3COO(aq) is substantially reacted with SO2(g). The employing NaCH3COO(aq) may react with residual SO2(g) potentially present in the remaining gases, which may avoid solid formation or solid handing issues which may occur if Ca(CH3COO)2(aq) is reacted with residual SOrtg).• For example, in some embodiments in some embodiments, the ability for the reaction products to comprise aqueous or pumpable phases may enable absorption column, or absorber, or reac tor, or any combination thereof designs or configurations which may facilitate the recovery of acetic acid vapor and / or may reduce the potential amount or concentration of acetic acid vapor in the remaining gases.• For example, it may be desirable to absorb SO2(g) in an absorption column because the SO2(g) may be at a dilute concentration, or a low partial pressure, or may comprise a gas mixture, or to improve absorption efficiency, or to facilitate the recovery or removal of any acid vapor from remaining gases, or to facilitate the recovery or removal of acetic acid vapor from remaining gases, or prevent or minimize or reduce the concentration or partial pressure of acetic acid vapor in the remaining gases, or any combination thereof. For example, in some embodiments,the process employed to decompose calcium sulfite to calcium oxide and sulfur dioxide may form a gas mixture comprising sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in said gas mixture may be lower than 1 atm, or 0.9 atm, or 0.8 atm, or 0.7 atm, or 0.6 atm, or 0.5 atm, or 0.4 atm, or 0.3 atm, or 0.2 atm, or 0.1 atm, or 0.05 atm, or any combination thereof and / or wherein the volume percent concentration of sulfur diox ide in said gas mixture may be lower than 100%, or 90%, or 80%, or 70%, or 60%, or 50%, or 40%, or 30%, or 20%, or 1.0%, or 5%, or any combination thereof.• Greater absorption rate or absorption efficiency.• Solid-liquid separations may be easier or simpler or higher yielding. For example, in some embodiments, if the rate of precipitation is dependent on the mixing of two liquids, rathe r a precipitation reaction from a gas and a liquid, the formation of and / or separation of precipitates may be more controllable.

[0146] Example 4: Process for Producing Magnesium Oxide or Cement or Clinker with Alkali Intermediate

[0147] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• MgCO3(s or aq) + 2 CH3COOH(aq) -> Mg(CH3COO)2(aq) + CO2(g)• Magnesium Silicate(s) + 2 CH3COOH(aq) .MgfCH3COO)2(aq) + SiliconDioxide(s)• MgS(s) + 2 CH3COOH(aq) -> Mg(CH3COO)2(aq) + H2S(g)• Magnesium (Weak Acid Anion) + 2 CH3COOH(aq) Mg(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq)

[0148] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0149] Note: If CO2(g) is produced, it may be desirable for said CO3(g) to be produced at a high partial pressure CO2(g), or purity CO2(g), or to comprise captured CO2(g).

[0150] (2) Mg(CH3COO(aq) + Na2SO3(s or aq)-> 2 NaCH3COO(aq) + MgSO3(s)

[0151] Note: MgSO3(s) may be separated using a solid-liquid separation.

[0152] (3) 2 NaCH3COO(aq) + SO2(g (1 or aq +) H2O(l or aq) -> Na2SO3(aq) + 2CH3COOH(aq)

[0153] (4) Na2SO3(aq)+ 2 CH3COOHCaq) -> 2 H3C OOH(aq or 1) + Na2SO3(s)

[0154] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, wafer may be removed and / or Na2SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0155] Note: in some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may precipitate or erystalize before Na2SO2. In some embodiments, if present, magnesium sulfite may precipitate or crysialize before Na2SO3, which may enable the separation of at least a portion of magnesium sulfite from Na2SO3.

[0156] Note: Na2SO3(s) may be separated from CH3COOH(aq or 1) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof,

[0157] Note: In some embodiments, CTfeCOOH may evaporate with wafer vapor and / or condense with water vapor to form a distillate or condensate comprising CH3COOH(aq).

[0158] (5) MgSO3(s) MgO(s) + SO2(g)

[0159] Note: ‘(5)’ may comprise calcining CaSO3(s), which may employ a kiln.

[0160] Note: CaSOj(s) may be dried, or dehydrated, or both before, or during ‘(5)’.

[0161] Note: In some embodiments, it may be preferred to react SO2(g) with NaCH3COO(aq) to form Na:?SO3(aq), and then react Na2.SO3with Mg(CH3COO)2((a4) to form MgSO3(s) because, for example, including, but not limited to, one or more or any combination of the following potential benefits:• In some embodiments, it may be desirable to absorb SO in2(g an) absorption column. Precipitate formation can be problematic in an absorption columns due to, for example, including, but not limited to, precipitate clogging packing material, or plates, or interfering with gas flows, or interfering with liquid flows, or forming scaling, or any combination thereof. The reaction of Mg(CH3C)2(aq) with SO2(g) may form a precipitate comprising MgSO3(s), which may be problematic in some absorption columns or a gas absorption processes. The reaction of NaCH3COO(aq)with SO2(g) may, if desired, remain an aqueous solution or liquid solution throughout the reaction, because, for example, Na2SO3is soluble in water, which may be desirable in an. absorption column.• For example, it may be desirable to absorb SO2(g)in, absorption column because the SO2(g) may be at a dilute concentration, or a low partial pressure, or may comprise a gas mixture, or to improve absorption efficiency, or to facilitate the recovery or removal of any acid vapor from remaining gases, or any combination thereof. For example, in some embodiments, the process employed to decompose calcium sulfite to calcium oxide and sulfur dioxide may form a gas mixture comprising sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in said gas mixture may be lower than 1 atm, or 0.9 atm, or 0.8 atm, or 0.7 atm, or 9.6 atn, or 0.5 atm, or 0.4 atm, or 0.3 aim, or 0.2 atm, or 0.1 atm, or 0.05 atm, or any combination thereof and / or wherein the volume percent coiicentration of sulfur dioxide in said gas mixture may be lower than 100%, or 90%, or 80%, or 70%, or 60%, or 50%, or 40%, or 30%, or 20%, or 10%, or 5%, or any combination thereof.• In some embodiments, if the SO2(g) comprises gases in addition to SO2(g), acetic acid vapor may be present in the remaining gases during or after the reaction of SOd.g) with an acetate salt. If SO2(g) is contacted with NaCH3COO(aq), which may form aqueous phase NarSO3(aq) and / or acetic acid, the reactor or absorption column may be configured such that NaCH3COO(aq) entering the reactor or absorption column absorbs or recovers at least a portion of acetic acid vapor from the remaining gases. If SO2(g) is contacted with NaCH3COO(aq), which may form aqueous phase Na2SO3(aq) and / or acetic acid, the reactor or absorption, column may be configured such that NaCH3COO(aq) entering the reactor or absorption column absorbs or recovers at least a portion of acetic acid vapor from the remaining gases before or while NaCH3COO(aq) is substantially reacted with SO2(g). The employing NaCH3COO(aq) may react with residual SO2(g) potentially present in the remaining gases, which may avoid solid formation or solid handing issues which may occur if Ca(CH3COO)2(aq) is reacted with residual SO2(g) .• Greater absorption rate or absorption efficiency.• Solid-liquid separations may be easier or simpler or higher yielding. For example, if the rate of precipitation is dependent on the mixing of two liquids, rather than a gasand a liquid, the formation of and / or separation of precipitates may be more controlled.

[1162] Example 5: Process for Producing Calcium Oxide or Cement or Clinker withAlkali Intermediate with Recirculating Separation Process

[0163] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCO3(s (1 or aq+) 2 CH3COOH(aq)-> Ca(CH3COO)2(aq+) CO2(g)• Calcium Silicate(s) -t 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + Silicon Dioxide) s)• CaS(s) + 2 CH3COOHtaq) -> Ca(CH3COO)3Caq) + H2S(g)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + WeakAcid(s, or g, or 1, or aq)

[0164] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0165] (2) Ca(CH3COO)2(aq) + Na2.SO3(s (1 or aq +) CH3COOH(aq) -> 2 NaH3COO (aq)+ CH3COOH (aq) + CaSO2(s)

[0166] Note: CaSO3(s) may be separated using a solid-liquid separation,

[0167] Note: CH3C OOH(aq) may be present due to CH3COOHtaq) being present in the retaliate solution comprising Na2SO3(aq) from a membrane based separation of CH3COOH(aq) and Na2SO3faq).

[0168] (3) 2 NaCH3COO(aq) + SOrig or aq) + H2O(l (1 or aq) Na2SO3(aq+) 2 CH3COOH(aq)

[0169] (4) Na2SO3(aq)+ 2 CH3COOH(aq) 2 CH3COOH(aq) separately fromNa2SO3(aq)+ 2 CH3COOH(aq)

[0170] Note: A portion of CH3COOH(aq) may be separated from NaxSOriaq) using a separation process, such as a membrane based process, such as reverse osmosis. In some embodiments, CH3COOH(aq) may have a hydration radius or molar mass sufficiently small to permeate through a membrane, while said membrane may reject NmSO3(aq). In some embodiments, Na2SOriaq) + 2 CH3COOH(aq) may be separated into a permeate solution comprising 2 CH3COOH(aq) and a retentate solution comprising Na2SO3(aq) •> 2 CH3COOH(aq).

[0171] (5) CaSCh(s) CaO(s) + SO2tg)

[0172] Note: ‘(5)!may comprise calcining CaSOris), which may employ a kiln,

[0173] Note: CaSOj(s) may be dried, or dehydrated, or both before or during ‘(5) ’ .

[0174] Example 6: Process for Producing Magnesium Oxide or Cement or Clinker with Alkali Intermediate with Recirculating Separation Process

[0175] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• MgCO3(s or aq) + 2 CH3COOH(aq) -> MglCH3COO)2(aq) fr CO2(g)• Magnesium Silicate(s) + 2 CH3COOH(aq) ->Mg (CH3COO)2(aq) + Silicon Dioxide(s)• MgS(s) + 2 CH3COOH(aq) ->Mg (CH3COO(2)aq) + HjS(g)• hiagnesium(Wcak Acid Anion) + 2 CH3COOH(aq) M.g(CH3COO)Aaq) fr Weak Acid(s, or g, or 1, or aq)

[0176] Note: Residual solids or undtssolved solids, such as silicon dioxide of other undissolved solids, may be separated from the liquid solution using a solid- liquid separation,

[0177] (2) Mg(CH3COO)2(aq) + Na2SO^s or aq) + CH3COOH(aq) -> 2 NaCH3COO(aq)+ CH3COOH(aq) + MgSOt(s)

[0178] Note: MgSO3(s) may be separated using a solid-liquid separation.

[0179] Note: CH3COOH(aq) may be present due io CH3COOH(aq) being present in the retaliate solution comprising Na2SO3(aq) from a membrane based separation of CH3COOH(aq) and Na;SO3(aq).

[0180] (3) 2 NaCH3COO(aq) + SO2(g (1 or aq +) H2O(l (1 or aq) NaiSO3(aq) + 2CHCOOH(aq)

[0181] (4) Na2SO3(aq) 2 CH3COOH(aq) 2 CH3COOH(aq) separately from Na2SO3(aq) + 2 CH3COOH(aq)

[0182] Note: A portion of CH3COOH(aq) may be separated from Na2SO3(aq) using a separation process, such as a membrane based process, such as reverse osmosis. In some embodiments, CH3COOH(aq) may have a hydration radius or molar mass sufficiently small to permeate through a membrane, while said membrane may reject Na aSO3faq). In some embodiments, NarSOfraq) + 2 CH3COOH(aq) may be separated into a permeate solutioncomprising 2 CH3COOH (aq) and a retentale solution comprising Na3SO3(aq) + 2 CH3COOH(aq).

[0183] (5) MgSO3(s) MgO(s)+ SO2(g)

[0184] Note: '(5)’ may comprise calcining MgSO3(s), which may employ a kiln.

[0185] Note: MgSO3(s) may be dried, or dehydrated, or both before or during ‘(5)’.

[0186] Example 7: Sodium Hydroxide Production from Sodium Sulfate usingCalcium Precipitation and Acid Intermediate

[0187] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth ~Weak Acid Amon with Acetic Acid• CaCO3(s or aq.) + 2 CH3COOH(aq) -> Ca(CH3COO(2)aq) + CO2(g) + H2O (1 or aq)• Calcium Silicate(s) + 2 CH3COOH(aq) -> Ca(CH3COO)?(aq) + Silicon Dioxide(s) + H2O(1 or aq.)• CaS(s) + 2 CH3COOH(aq) -> Ca CH3COOH(aq) + H2S(g) + H2O (1 or aq)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq) + H2O (1 or aq)

[0188] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation,

[0189] Note: CO»(g) may comprise captured CO2.

[0190] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium, In some embodiments, for example. Input chemicals or input material may comprise amixture of calcium and magnesium.

[0191] Note: Tn some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO3(g).

[0192] (2) Ca(CH3COO)2(aq) + Na2SO4(s or aq) -> 2 NaCH3COO(aq) + CaSO4(s)

[0183] Note: In some embodiments, Na2StM's) may be added directly to or dissolved in Ca(CH3COO)2(aq).

[0194] Note: In some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form Na2SO4(aq) before mixing with Ca(CH3COO)2(aq).

[0195] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an. output, or any combination thereof In some embodiments, water may be added to the process by NarSCfr being in the form of Na2SO2(aq) or an aqueous solution comprising sodium sulfate, wherein at least a portion of the water in Na2SO4(aq) may comprise water added to the process. In some embodiments, Na2SO4(aq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SO4(aq) may be provided to the process in the form of Na2SO4(aq). In some embodiments, Na2SO4(aq) may be provided or sourced as a solid or Na2SO4(s), then dissolved in water to form Na2SO^aq).

[6196] (3) 2 NaCH3COO(aq) + SO2(g (1 or aq ) H +2O(1 or aq) -> Na2SO3(aq) + 2 CH3COOH(aq)

[0197] Note: In some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some enfoodiments, th reeaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in t rheemaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[0198] (4) N Na2SO3(aq) 2 CH3COOH(aq) 2 CH3COOH(aq) + Na2SO3(s)

[0199] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, Na2SO2may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0200] Nbte: In some embodiments, CH3COOH and or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments, CH3COOH may evaporate with water vapor and / orcondense with water vapor, which may resul t in a distillate or condensate comprisingCH3COOH(aq),

[0201] Note; In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2 CHCOOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate orcrystalize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step ‘(4)’. In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof. s

[0202] Note; NarSO3(s) may be separated .from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods desen bed in the art, or any combination thereof,

[0203] (5) Na2SO3(s or aq) + Ca(OH)Xs or aq) 2 NaOHtaq or s) + CaSOXs)

[0204] Note: Ca(OH)2(s (1 or aq m) ay comprise a solid-liquid suspension, such as milk of lime.

[0205] Note: CaSO3('s) may be separated using a solid-liquid separation,

[0206] (6) CaSO3(s) -> CaO(s) + SO2(g)

[0207] Note: ‘(6)' may comprise calcining CaSO3(s), which may employ a kiln.

[0208] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘(6)2

[0209] (7) CaO(s) + Water(g or 1 (1 or aq ) -> Ca(OH)2(s or aq)

[0210] Note: In some embodiments, CaO(s) may be employed to remove water vapor or facilitated drying of CaSO3(s) before or during decomposition of CaSO3(s) to CaO(s).

[0211] Note: In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide. In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide, which may comprise combining step '(5)’ and step ‘(7)'

[0212] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-liquid suspension, or milk of lime, or solid, or any combination thereof comprising calcium hydroxide.

[0213] (8) 2 NaOH(aq or s) 2 NaOH(aq or s) + Water

[0214] Note: in some embodiments, NaOH(aq) may be concentrated into an aqueous solution comprising a greater mass percent concentration of NaOH.

[0215] Note: In some embodiments, water may be removed and / or NaOH may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0210] Note: In some embodiments, it may be desirable for NaOH to comprise a concentrated aqueous solution.

[0217] Example 8: Sodium Hydroxide Production from Sodium Su 1 fat e usingAlkaline-Earth Precipitation and Acid Intermediate

[0218] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• MgCO3(s or aq) + 2 CH3COOH(aq) -> Mg(CH3COO(aq) + CO3(g)• Magnesium Silicatcts) + 2. CH3COOH(aq) Mg(CH3COO)2(aq+) Silicon Dioxide(s)• MgS(s) + 2 CH3COOH(aq) Mg(CH3COO)2(aq) + H2S(g)• Magnesium} Weak Acid Anion) + 2 CH3COOH(aq) -> Mg(CH3COO2(aq) + WeakAcidfs, or g, or 1, or aq)

[0219] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0220] (2) Mg(CH3COO)2(aq) + Na2SCfrtaq) 2 Na CH3COO(aq) + MgSO-if s (1 or aq)

[0221] (3) 2 Na CH3COO(aq) + SO2(g or aq) + ftO(l (1 or aq) Na2SO3(aq) + 2 CH3COOH(aq)

[0222] (4) Na2SO3(aq) + 2 CH3COOH(aq) -> 2 CH3COOHfaq) + Na2SO3(s)

[0223] Note: CH3COOH may be more soluble in waler than Na2SO3. In some embodiments, water may be removed and / or Na2SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crj / stallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0224] Note: Na2SO3(s) may be separated from CH3COOH(aq o r 1) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0225] (5) NarSO3(s or aq) + Mg(OH)2(s or aq -> 2 NaOH(aq or s) + MgO3(s)

[0226] Note: Mg(OH)(s (1 or aq m) ay comprise a solid-liquid suspension, such as milk of lime.

[0227] Note: MgSO3(s) may be separated using a solid-liquid separation.

[0228] (6) MgSOj(s) MgO(s) + SO2(g)

[0229] Note: (6)' may comprise calcining MgSO3(s) which may employ a kiln.

[0230] Note: MgSO3(s) may be dried, or dehydrated, or both before or during ‘(6)’ -

[0231] (7) MgO(s) + Watering or 1 (1 or aq) Mg(OH)2(s or aq)

[0232] Note: MgO(s) may be employed to remove water vapor or facilitated drying of MgSO3(s) before or during decomposition of MgSO3(s) to IMgO(s).

[0233] (8) 2 NaOH(aq or s) 2 'NaOH(s) + Water

[0234] Note: In some embodiments, water may be removed and / or NaOH may beseparated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0235] Note: In some embodiments* it may be desirable for NaOH to comprise a concentrated aqueous solution.

[0236] .Example 9; Sodium Hydroxide Production from Sodium Sulfate usingCalcium Precipitation and Acid Intermediate

[0237] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCO3( s or aq A) 2 CH3COOH(aq) Ca(CH3COO.h(aq) + CO2.(g)• Calcium Sihcate(s) 2 CH3COOH(aq) -> Ca(CH3COO)2(aq) Silicon Dioxide(s)• CaS(s) + 2 CH3COOH(aq) Ca(CHhCOO)2( aq) - H2S(g). Calcium( Weak Acid Anion) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + Weak Acid(s, or g, or I. or aq)

[0238] Note; Residual solids or undissoked solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0239] (2) Ca(CH3COO)2(aq) + Na2SO)4(aq) → 2NaCH3COO(aq) + CaSO4(s)

[0240] (3) 2 NaCH3COO(aq) + SO2(g or aq) + H2O(1 or aq) → Na2SO3(aq) + 2 CH3COOH(aq)

[0241] (4) Na2SO3(aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq) + Na2SO3(s)

[0242] Note: CH3COOH may be more soluble in water than Na2.SO2. In some embodiments, water may be removed and / or Na2SO3may be separated or precipitated by, for example, including, but not limited to* evaporation* or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0243] Note: Na2SO3(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge* or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0244] (5) Na2SO3(s (1 or aq ) + Mg(OH)2(s or aq) → 2 NaOH(aq or s) + MgSO3(s or aq)

[0245] Note: Mg(OH)2(s or aq) may comprise a solid-liquid suspension, such as milk of lime.

[0246] Note: MgSO3(s) may be separated using a solid-liquid separation.

[0247] (6) MgSO3(s) → MgO(s) + SO2(g)

[0248] Note: ‘(6)’ may comprise calcining MgSO3(s), which may employ a kiln,

[0249] Note: MgSO3(s) may be dried, or dehydrated, or both before or during ‘(6)’.

[0250] (7) MgO(s) + Watcr(g or I or aq) → Mg(OH)2(s or aq)

[0251] Note: MgO(s) may be employed to remove water vapor or facilitated drying of MgSO3(s) before or during decomposition of MgSO3(s) to MgO(s).

[0252] (8) 2 NaOH(aq or s) → 2 NaOH(s) + Water Or2 NaOH(aq) → 2 NaOH(aq - more concentrated) + Water

[0253] Note: In some embodiments, water may be removed and / or NaOH may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0254] Note: in some embodiments, it may be desirable for NaOH io comprise a concentrated aqueous solution.

[0255] Note: Residual MgSO2.(aq) may be present or dissolved in the solution comprising NaOH(aq). lb some embodiments, during the concentrating of NaOH(aq) or removal of at least a portion of water from the NaOH(aq), at least a portion of the residual MgSO3may precipitate or may be separated or recovered. For example, in some embodiments, MgSO3(aq) may be less soluble in water than NaOH(aq), Separated or recovered MgSO3may be transferred, for example, to step ‘(6)’.

[0256] Example 10: Sodium Carbonate Production from Sodium Sulfate usingAlkaline-Earth Precipitation and Acid Intermediate

[0257] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCO3(s or aq) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g)• Calcium Silicate( s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + Silicon Dioxide(s)• CaS(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + HsS(g)• CafciumfWeak Acid Anion) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + WeakAcid(s, or g, or I, or aq)

[0258] Note: Residual sol ids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0259] (2) Ca(CH3COO)2(aq) + Na2SO4(aq) → 2 NaCH3COO(aq) + CaSO3(s)

[0200] (3) 2 NaCH3COO(aq) + SO2(g or aq) + H2O (1 or aq ) → Na2SO3(aq) + 2CH3COOH(aq)

[0261] (4) Na2SO3(aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq) + NarSO3(s)

[0262] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, water may be removed and / or N'asSO3may be separated or precipitated by.for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0263] Note: Na2SO3(s) may be separated from CH3COOH(aq or I) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0264] (5) Na2SO3(s or aq) + Ca(OH)2(s or aq) 2 NaOH(aq or s) CaSO3ts)

[0265] Note: Ca(OH)2(s or aq)may comprise a solid-liquid suspension, such as milk of lime.

[0266] Note: CaSO3(s) .may be separated using a solid-liquid separation.

[0267] Note: in some embodiments, Na2SO3(s) may be dissolved in water to form Na2SCh(aq) before step '(5)’. In some embodiments, water may provided from internally within the process, or water may be provided from an external source, or any combination thereof. For example, if net water is consumed, or water is in the sodium hydroxide or sodium carbonate product, or water is in the product, or any combination thereof, it may be desirable for a portion of the water to come from an external source.

[0268] (6) CaSOfrs) CaO(s) + SO2(g)

[0269] Note: '(6)' may comprise calcining CaSOfrs), which may employ a kiln.

[0270] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘(6)’.

[0271] (7) CaO(s) + Watert g or 1 (1 or aq) Ca(OH)2(s or aq)

[0272] Note: CaO(s) may be employed to remove water vapor or facilitated drying of CaSO3(s) before or during decomposition of CaSOfrs) to Ca()(s).

[0273] Note: In some embodiments, CaO may be reacted directly with NatSChfs or aq) or an aqueous solution comprising sodium sulfite. For example, in some embodiments, step "(5)’ may be combined with step ‘(7)’

[0274] Note: In some embodiments, water may provided from internally within the process, or water may be provided from an external source, or any combination thereof. For example, if net water is consumed, or water is in the sodium hydroxide or sodium carbonateproduct, or water is in the product, or any combination thereof it may be desirable tor aportion of the water to come from an external source.

[0275] (8) 2 NaOH(aq or s) + CO2(g) → Na2CO2(s (1 or aq ) + H2O(l or aq or g)

[0276] Note: In some embodiments, CO2may comprise a gas with a dilute concentration of carbon dioxide, which may include, but is not limited to, CO2sources described herein or CO2sources. In some embodiments, NaOH(aq) may be capable of reacting with a wide range of CO2(g) concentrations, including, potentially, for example, very low CO2(g) concentrations, such as CO2(g) in air.

[0277] Note: In some embodiments, NaOHfaq or s) may be added to the ocean or sea, where it may react with CO2or CO2derivative ions or chemical species in the ocean or air and. or increase ocean pH.

[0278] Note: Na2CO3( s or aq)may be further reacted with carbon dioxide and / or water to form sodium bicarbonate.

[0279] Note: Na2CO3( s) may precipitate and / or be separated from the remaining solution. After precipitation, NaOH(s) may be added and / or dissolved in the remaining solution, to, tor example, make up for sodium lost during the precipitation and separation of Na2CO3(s).

[0280] Note: in some embodiments, Na2CO3(aq), which may comprise a ‘feed' solution into a concentrating process, may be concentrated using an energy efficient concentrating method, such as reverse osmosis or electrodialysis or heat recovery distillation, at an elevated temperature and / or the resulting concentrate or retentate may be cooled to precipitate a portion of Na2CO3(s). In some embodiments, the remaining solution after precipitation and separation of Na?.CO2(s) may be mixed with Na2CO3(aq) feed solution before heating the combined solution and / or concentrating the combined solution using an energy efficient concentrating method. In some embodiments, water recovered during the concentrating, such as water permeate, or diluate, or condensate, may be, including, but not limited to, one or more or any combination of the following: employed dissolve sodium sulfite and form aqueous sodium suffite, or transferred to a reaction of calcium oxide with water to produce calcium hydroxide, or transferred to dissolve sodium sulfate.

[0281] Note: SOc(g) from calcining CaSOs may be further concentrated, or pressurized, or purified.

[0282] Note: SO2(g) from calcining CaSO3may be absorbed into water or an aqueous solution to form sulfurous acid or aqueous sulfur dioxide.

[0283] Note; Weak acid or weak acid anion may comprise an acid or acid anion with an acid strength lower than the acid strength of formic acid, or acetic acid, or propionic acid, or butyric acid, or citric acid, or lactic acid, or valeric acid, or caproic acid, or enanthic acid, or caprylic acid, or pelargonic acid, or capric acid, or carboxylic acid, or sulfurous acid.

[0284] Note: Weak acid or weak acid anion may comprise an acid or acid anion with a higher pK.a than acetic acid, or carboxylic acid, or sulfurous acid.

[0285] Note: Acetic acid may be provided as an example acid with an acid strength greater than" Weak Acid’, and an acid strength lower than sulfurous acid or aqueous sulfur dioxide.

[0286] Note: Acetic acid may be provided as an example acid with an pKa lower than “Weak Acid’, and an pK.a great©' than sulfurous acid or aqueous sulfur dioxide.

[0287] Note: Calcium may be provided as an example alkaline earth. Other alkaline earths, which may include beryllium (Be), or magnesium (Mg), or calcium (Ca), or strontium (Sr), or barium (Ba), or radium (Ra), or any combination thereof, may be employed instead or in addition io calcium.

[0288] Example 11: Process for 'Producing Calcium Oxide or Cement or Clinker with Ammonia Inter mediate

[0289] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCO3(s or aq )+ 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g)• Calcium Silicate(s) + 2 CH3COOH(aq) → Ca(CH3COO )2(aq) + Silicon Dioxide(s)• CaS(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + H2(g )• Calcium(Weak. Acid Anion) + 2 CH3COOH(aq) → Ca(CH3COO)3(aq) + Weak Acid(s, or g, or 1, or aq)

[0290] Note: Residual solids or undissolvcd solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0291] Note: If CO2(g) is produced, it may be desirable for said CO2(g) to be produced at a high partial pressure CO2(g'), or purity CO2(g), or to comprise captured CO2(g).

[0292] (2) Ca(CH3COO)2(aq) + (NH4)2SO3(s or aq) → 2 NH4CH3COO(aq) + CaSO3( s)

[0293] Note: CaSO3( s) may be separated using a sol id-liquid separation.

[0294] (3) 2 NH4CH3COO(aq) + SO2(g or aq +) H2O (1 or aq) → (NH4SO3(aq) + 2 CH3COOH(aq)

[0295] (4) (NH4)2SO3(aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq) + (NH4)2SO3(S)

[0296] Note: CH3COOH may be more soluble in water than (NHyhSOj. In some embodiments, water may be removed and / or (NH4)2SO3may be separated or precipitated by, for example, including, but not limited io, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or zero-liquid discharge methods described in the art, or separation systems or methods described in the art, or any combination thereof.

[0297] Note: In some embodiments, magnesium sulfite(aq) may be present in the (NH4)2SO3(aq) + 2 CH3COOH(aq). In some em bodiments, if present, at least a portion of magnesium sulfite may begin to precipitate or erystalize before (NH3)2SO3. In some embodiments, it may be desi rable to separate at least a portion of the magnesium sulfite from (NH^SO3.

[0298] Note: (NH4)2SO3(s) may be separated from CH3COOH(aq or I) by a solid-liquid separation, which may include, but is not l imited io, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0299] (5) Ca SO3(s) → CaO(s) + SO2(g)

[0300] Note: ‘(5)' may comprise calcining CaSO3(s), which may employ a kiln,

[0301] Note: CaSO2(s) may be dried, or dehydrated, or both before, or during ‘(5)’.

[0302] Note: In some embodiments, it may be preferred to react SO2(g) with NH4CH3COO(aq) to form (NH4)2SO3(aq), then react (NH4)2SO3with Ca(CH3COO)2(aq) to form CaSO3(s) because, for example, including, but not limited to, one or more or atty combination of the foltowing potential benefits;* In some embodiments, it may be desirable to absorb SO2(g) in an absorption column. Precipitate formation can be problematic in an absorption columns due to, for example, including, but not limited to, precipitate clogging packing material, orplates, or interfering with gas flows, or interfering with liquid flows, or forming scaling, or any combination thereof The reaction of Ca(CH3COO)2(aq) with SO2(g) may form a precipitate comprising CaSO3(s), which may be problematic in some absorption columns or a gas absorption processes. The reaction ofNH4CH3COO(aq) with SO2(g) may, if desired, remain an aqueous sol ution or liquid solution throughout the reaction, because, tor example, (NH4)2SO3is soluble in water, which may be desirable in an absorption column* For example, it may be desirable to absorb SO2tg) in an absorption column because the SO2(g) may be at a dilute concentration, or a low partial pressure, or may comprise a gas mixture, or to improve absorption efficiency, or any combination thereof For example, in some embodiments, the process employed to decompose calcium sulfite to calcium oxide and sulfur dioxide may form a gas mixture comprising sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in said gas mixture may be lower than 1 atm, or 0.9 arm, or 0.8 atm, or 0.7 atm, or 0,6 aim, or 0.5 atm, or 0.4 atm, or 0-3 atm, or 0.2 atm, or 0. 1 atm, or 0.05 atm, or any combination thereof and / or wherein the volume percent concentration of sulfur dioxide in said gas mixture may be lower than 100%, or 9(1%, or 80%, or 70%, or 60%, or 50%, or 40%, or 30%, or 20%, or 10%, or 5%, or any combination thereof + Greater absorption rate or absorption efficiency.* Solid-liquid separations may be easier or simpler or higher yielding. For example, if the rate of precipitation is dependent on the mixing of two liquids, rather than a gas and a liquid, the formation of and 7 or separation of precipitates may be more controlled.

[0303] Example 12; Process for Producmg Alkaline- Earth Oxide nr Cement orClinker with Ammonia Intermediate

[0304] (1 ) React .Material comprising Calcium, or Magnesium, or Other Alkaline Earth —Weak Acid Anion with Acetic Acid• MgCO3(s (s or aq) + 2 CH3COOH(aq) → Mg(CH3COO)2(aq) + CO2(g)• Magnesium Silicates) + 2 CH3COOH(aq) → Mg(CH3COO)2(aq) E Silicon Dioxide(s)• MgSl's) + 2 CH3COOH(aq) Mg(CH3COO ) 2 H2S(g)+ Magnesium (Weak Acid Anion) + 2 CH3COOH(aq) Mg(CH3COO)2(aq) + Weak Acid(s, or g, or I, or aq)

[0305] Note: Residual solids or undissofoed solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation,

[0306] Note: If CO3(g) is produced, it may be desirable for said CO2(g) to be produced at a high partial pressure CO3(g), or purity CO2(g), or to comprise captured CO2(g).

[0307] (2) Mg(CH3COO)2(aq) + (NH4)2SO3(s or aq) → 2 NH4CH3COO(aq) + MgSO3(s)

[0308] Note: MgSOa(s) may be separated using a solid-liquid separation,

[0309] (3) 2 NH4CH3COO(aq) + SO2(g or aq) + H2O(I or aq) (NH4)2SO3(aq) + 2 CH3COOH(aq)

[0310] (4) (NH4)2SO3(aq) + 2 CH3COOH(aq) -> 2 CH4COOH(aq) + (NH4)2SO3(s)

[0311] Note: CH3COOH may be more soluble in water than (NH4)2SO3. In some embodiments, water may be removed and / or (NHO3SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0312] Note: In some embodiments, magnesium sulfite(aq) may be present in the (NH4)2SO3(aq)+ 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before (NH4)2SO3.

[0313] Note: (NbUbSOAs) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0314] (5) MgSO3(s) → MgO(s) + SO2(g)

[0315] Note: ‘(S) may comprise calcining CaSO3(s), which may employ a kiln.

[0316] Note: CaSO3(s) may be dried, or dehydrated, or both before, or during "(5)"

[0317] Note: In some embodiments, it may be preferred to react SO2(g) with NH4CH3COO(aq) to form (NH4)2SO3( aq), then react (NH4)2SO3with Mg(CH3COO)2(aq) toform MgSO2(s) because, for example, including, but not limited to, one or more or any combination of the following potential benefits;• In some embodiments, it may be desirable to absorb SO2(g) in an absorption column. Precipitate formation can be problematic in an absorption columns due tosfor example, including, but not limited to, precipitate clogging packing material, or plates, or interfering with gas flows, or interfering with liquid flows, or forming scaling, or any combination thereof. The reaction of Mg(CH3COO)2(aq) with S0?(g) may form a precipitate comprising MgSO,t(s), which may be problematic in some absorption columns or a gas absorption processes. The reaction of NHiCHjCOO(aq) with SO2(g) may, if desired, remain an aqueous solution or liquid solution throughout, the reaction, because, for example, NarSOa is soluble in water, which may be desirable in an absorption column.• For example, it may be desirable to absorb SO2(g) in an absorption column because the SCht'g) ma_v be at a dilute concentration, or a low partial pressure, or may comprise a gas mixture, or to improve absorption efficiency, or any combination, thereof For example, in some embodiments, the process employed to decompose calcium sulfite to calcium oxide and sulfur dioxide may tai a gas mixture comprising sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in said gas mixture may be lower than 1 atm, or 0.9 atm, or 0.8 atm, or 0.7 atm, or 0,6 atm, or 0,3 atm, or 0.4 atm, or 0.3 aim, or 0.2 atm, or 0.1 atm, or 0,05 atm, or any combination thereof and / or wherein the volume percent concentration of sulfur dioxide in said gas mixture may be lower than 100%, or 90%, or 80%, or 70%, or 60%. or 50%, or 40%, or 30%, or 20%, or 10%, or 5%, or any combination thereof.• Greater absorption rate or absoiption efficiency.• Solid-liquid separations may be easier or simpler or higher yielding. For example, if the rate of precipitation is dependent on the mixing of two liquids, rather than a gas and a liquid, the formation of and / or separation of precipi tates may be more controlled.

[0318] Example 13: Process for Producing Calciu Oxide or Cement or Clinker with Ammonia Intermediate with Recirculating Separation

[0319] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid•••.

[0320] Note; Residual solids or undissotved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0321]

[0322] Note; be separated using a solid-liquid separation.

[0323] Note:( q) may be present due tobeing present in the reientate solution comprisingfrom a membrane based separation of

[0324]

[0325]

[0326] Note: A portion ofmay be separated fromq using a separation, process, such, as a membrane based process, such as reverse osmosis. In some embodiments,may have a hydration radius or molar mass sufficiently small to permeate through a membrane, while said membrane may reject (NH^SO3(aq), In some embodiments,may be separated into a permeate solution comprising 2 CH3COOH(aq) and a retentete solution eotnprising

[0327]

[0328] Note: (5)’ may comprise calcining which may employ a kiln.

[0329] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘(5)’.

[0330] Example 14; Process for Producing Alkaline-Earth Oxide or Cement or Clinker with Ammonia Intermediate with Recirculating Separation

[0331] (1) React Material comprising Calcium, or Magnesium, or Other .Alkaline Earth -Weak Acid Anion with Acetic Acid»•••

[0332] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid- liquid separation.

[0334] Note: MgSO3(s) may be separated using a solid-liquid separation.being present in the retaliate solution comprisingfrom a membrane based separation of

[0338] Note: A portion ofmay be separated from using aseparation process, such as a membrane based process, such as reverse osmosis. In some embodiments, q) may have a hydration radius or molar mass sufficiently smallto permeate through a membrane, while said membrane may reject In someembodiments,may be separated into a permeate solution comprising and a retentate solution comprising

[0339] (5) MgSO3(s) MgO(s+) SO2(g)

[0340] Note: ‘ (6) ' may comprise calcining MgSO3(s), which may employ a kiln,

[0341] Note: MgSO3(s) may be dried, or dehydrated, or both before or during 26)’ -

[0342] Example.15; Ammonia Production from Ammoninm Sulfate using CalciumPrecipitation and Acid Intermediate

[0343] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth —Weak Acid Anion with Acetic Acid••••

[0344] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0345]

[0346]

[0347] Water

[0348] Note: CH3COOH may be more soluble in water than (NH4)2SO3In some embodiments, water may be removed and / or (NH4)2SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0349] Note: (NH4)SO3(s) may be separated from CH3COOH(aq or 1) by a solid-liquid separation, which may include, but is not limited to, fil ter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0350]

[0351] Note: may comprise a solid-liquid suspension, such as milk oflime.

[0352] Note may be separated using a solid-liquid separation.

[0353] Note; may be separated into ammonia gas and water if desired,

[0354]

[0355] Note: ‘(6)’ may comprise calciningwhich may employ a kiln,

[0356] Note:may be dried, or dehydrated, or both before or during ‘ (6)2

[0357]

[0358] Note; CaO(s) may be employed to remove water vapor or facilitated drying ofbefore or during decomposition of

[0359]

[0360] Note: In some embodiments, it may be desirable to produce ammonia gas or liquid ammonia. In some embodiments, it may be desirable to produce a high concentration or greater concentration aqueous ammonia or ammonium hydroxide solution.

[0361] Note: In some embodiments, it may be desirable for 2 NH«OH(aq) or 2 NH3fhq) to comprise an aqueous solution. If example, in some embodiments, it may be desirable for to

[0362] Earth Precipitation and Add Intermediate

[0363] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid•••»

[0364] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, .may be separated from the liquid solution using a solid-liquid separation.

[0365]

[0366]

[0367]

[0368] Note:may be more soluble in water than In someembodiments, water may be removed and / ormay be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0369] Note: may be separated from by a solid-liquidseparation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof|037O<

[0371] Note: q m) ay comprise a solid-liquid suspension, such as milk oflime.

[0372] Note: may be separated using a solid-liquid separation.

[0373] Note: may be separated into ammonia gas and water if desired.

[0374]

[0375] Note: ‘(6)’ may comprise calcining which may employ a kiln.

[0376] Note:may be dried, or dehydrated, or both before or during "(6)".

[0377]

[0378] Note: MgO(s) may be employed to remove water vapor or facilitated drying ofbefore or during decomposition of

[0379]

[0389] Note: In some embodiments, it may be desirable to produce ammonia gas or liquid ammonia. In some embodiments, it may be desirable to produce a high concentration or greater concentration aqueous ammonia or ammonium hydroxide solution,

[0381] Note: In some embodiments, it may be desirable for 2 NHtOH(aq) or 2 NH3(aq) to comprise an aqueous solution. If example, in some embodiments, it may be desirable for to keep aqueous ammonia or ammonium hydroxide at an aqueous phase.

[0382] Example 17: Ammonia Production from Ammonium Sulfate using Alkaline- Earth Precipitation and Acid Intermediate

[0383] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid +• +•

[0384] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0385]

[0386]

[0387]

[0388] Note: CH3COOH may be more soluble in water than (NH4)SO3. In some embodiments, water may be removed and / or (NH4)SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0389] Note:may be separated from CH3COOH(aq or 1) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0390]

[0391] Note; may comprise a solid-liquid Suspension, such as milk oflime.

[0392] Note:may be separated using a solid-liquid separation,

[0393] Note:may be separated into ammonia gas and water if desired.

[0394]

[0395] Note: '(6)’ may comprise calciningwhich may employ a kiln.

[0396] Note: may be dried, or dehydrated, or both before or during ‘(b)’.

[0397]

[0398] Note:may be employed to remove water vapor or facilitated drying ofbefore or during decomposition of

[0399]

[0400] Note: In some embodiments, it may be desirable to produce ammonia gas or liquid ammonia. In some embodiments, it may be desirable to produce a high coneentration or greater concentration aqueous ammonia or ammonium hydroxide solution.

[0401] Note: In some embodiments, it may be desirable forto comprise an aqueous so l ution. If example , in some embodiments, it may be desirable for to keep aqueous ammonia or ammonium hydroxide at an aqueous phase.

[0402] Example 18: Ammonium Carbonate or Ammonium Bicarbonate orAmmonium Carbamate or Urea Production using Add Intermediate

[0403] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid

[0404] Note: Residual solids or -undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a sol id-liquid separation.

[0405]

[0406]

[0407]

[0408] Note: CH3COOH may be more soluble in waler than Na2SOa. In some embodiments, water may be removed and / or Na2SO2may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0409] Note: may be separated fromby a solid-liquidseparation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art or any combination thereof.

[0410]

[0411] Note: q m) ay comprise a solid-liquid suspension, such as milk oflime.

[0412] Note:may be separated using a solid-liquid separation.

[0413]

[0414] Note: '(6)’ may comprise calciningwhich may employ a kiln.

[0415] Note:may be dried, or dehydrated, or both before or during ‘(6)'.

[0416]

[0417] Note: may be employed to remove water vapor or facilitated drying ofbefore or during decomposition of

[0418]

[0419] Note: In some embodiments, may be further reacted withcarbon dioxide and Z or water to form sodium bicarbonate.

[0420] Note: In some embodiments, the aqueous solution may comprise a mixture of ammonium carbonate, or ammonium bicarbonate, or ammonium carbamate, or ammonium sesquicarbonate, or fee ammonia, or aqueous ammonia, or ammonium hydroxide, or any combination thereof

[0421] Example 19: Direct Air Capture, or Capture of CO2fro Air, or CO2Capture using Alkaline-Earth , Sulfa r Dioxide, a nd Acid

[0422] (1) Reaction of alkaline-earth oxide, or alkaline-earth hydroxide, or any combination thereof with carbon, dioxide.

[0423]

[0424]

[0425]

[0426] Note: In some embodiments, SO2( g) may comprise a gas comprising a dilute concentration of SO2( g )

[0427]

[0428]

[0429] Example 20: Direct Air Capture, or Capture of CO2from Air, or CO2Capture using Alkaline-Earth, Sulfur Dioxide, and Acid

[0430] ( I) Reaction of alkaline-earth oxide, or alkaline-earth hydroxide, or any combination thereof with carbon dioxide.

[0431]

[0432] Note: CO2(g) in ‘(2) ’ may comprise captured CO2(g).

[0433]

[0434] Note: in some embodiments, SOAg) may comprise a gas comprising a dilate concentration of CO2(g).

[0435] (4) MgSO2(s) MgO(s) + SO2(g)

[0436] (5) MgO(s) + H2O(1 or g) →Mg(OH)3(s or aq)

[0437] Example 21: Direct Air Captnre, or Capture of CO2from Air, or CO2Capture using Alkali, Alkaline-Earth, and Sulfur Dioxide

[0438] (1) 2 NaOH(aq) ± CO2(g) Na2CO3(aq or s) + H2O(g or 1)

[0439] (2) Na2CO3(aq or s) + SO2(1 or aq)→ Na2SO3(aq or s) + CO2(g)

[0440] Note: CO2(g) in S'2)’ may comprise captured CO2(g).

[0441] (3) Na2SO3(aq or s) + Ca(OH)2(s or aq) 2 NaOH(aq) + CaSO3(s)

[0442] (4) CaSO3(s) CaO(s) + SO2(g)

[0443] (5) CaO(s) + H2O (1 or g) Ca(OH)2(s or aq)

[0444] Example 22: Direct Air Capture, or Capture of CO2from Air, or CO2Capture using Alkali, Alkaline-Earth, and Sulfur Dioxide

[0445] (I) 2 NaOH(aq) A CO2(g) Na2CO3(aq or s) + H2O(g or 1)

[0446] (2) NazCO3(aq or s) + SO2(1 or aq)→ Na2SO3(aq or s) + CO2(g)

[0447] Note: CO2(g) in ‘(2)’ may comprise captured CO2(g).

[0448] (3) Na2SO3(aq or s) + Mg(OH)2(1 or aq) 2 NaOH(aq) + MgSO3(s)

[0449] (4) MgSO3(s) MgO(s) + SO2(g)

[0450] (5) MgO(s) + H2O(1 or g) Mg(OH)2(s or aq)

[0451] Example 23: Direct Air Capture, or Capture of CO2from Air, or CO2Capture using Alkali, Alkaline-Earth, and Sulfur Dioxide

[0452] (1) 2 NaOH(aq) + CO2(g) NazCO3(aq or s) + H2O(g or 1)

[0453] (2) Na2CO3(aq or s) + 2 CH3COOH (1 or aq)→ 2 NaCH3COO(aq) + CO2(g)

[0454] Note: CO2(g) in ‘(2)’ may comprise captured CO2(g),

[0455] (3) 2 NaCH3COO(aq) + SO2(g) Na2SO3(aq or s) + 2 CH3COOH (aq)

[0456] Note: in some embodiments, SOrig) may comprise a gas comprising a dilute concentration of SO2(g).

[0457] (4) Separate Na2SOa from 2 CH3COOH

[0458] (5) Na2SO3(aq or s) + Ca(OH)2(s or aq) → 2 NaOH(aq) + CaSO3(s)

[0459] (6) CaSO3(s) CaO(s) + SO2(g)

[0460] (7) CaO(s)+ H2O(1 or g) →> Ca(OH)2(s or aq)

[0461] Example 24: Direct Air Capture, or Capture of CO2from Air, or CO2Capture using Alkali, Alkaline-Earth, and Sulfur Dioxide

[0462] (1) 2 NaOH(aq) t- CO2(g) Na2CO3(aq or s) + H2O (g or 1)

[0463] (2) Na2CO3iaq or s) + 2 CH3COOH (1 or aq)→ 2 Na CH3COOH (aq) + CO2(g)

[0464] Note: CO2(g) in ‘(2)’ may comprise captured CO2(g).

[0465] (3) 2 NaCH3COO(aq) A SO2(g) -> Na2SO3(aq or s )+ 2 CH3COOH (aq)

[0466] Note: In some embodiments, SO2(g m)ay comprise a gas comprising a dilute concentration of SOrig).(4) Separate Na2SO3from 2 CH3COOH

[0468] (5) Na2SO3(aq or s) + Mg(OH)2(s or aq) → 2 NaOH(aq) + MgSO3(s)

[0469] (6) MgSO3(s) → MgO(s) + SO2(g)

[0470] (7) MgO(s) + H2O(1 or g) → Mg(OH)2(s or aq)CO2 Desorption or Displacement, and Reagent Regeneration

[0472] (I) CO2Absorption: CO2may be absorbed or adsorbed in calcium oxide, or calcium hydroxide, or calcium hydroxide suspension, such as milk of lime, or any combination thereof to produce calcium carbonate solid or suspension.

[0473] Ca(OH)2(s (1 or aq -t) CO2(g) CaCO3(s) + H2O(1 or g)

[0474] Note: Calcium hydroxide suspension may be transported to the absorption location and / or stored at or near the absorption location.

[0475] Note: Calcium carbonate solid may be separated by settling, or solid-liquid separation, or any combination thereof.

[0476] Note: Calcium carbonate may be stored at or near the absorption or adsorption location. Calcium carbonate may be transported to an application using calcium carbonate. Calcium carbonate may be transferred to the CO2desorption or displacement location. In some embodiments, the CO2desorption or displacement location may be the same as the CO2absorption or adsorption location. In some embodiments, the CO2desorption or displacement location may be different than the CO2absorption or adsorption location. For example, in some embodiments, it may be desirable for the CO2absorption or adsorption to be located at multipie distributed sites, while the Regeneration may be conducted at a larger and / or more centralized facility or site.

[0477] (2 ) CO2Desorption or Displacement: Calcium carbonate may be reacted with acetie acid to produce calcium acetate and carbon dioxide.

[0478] CaCO2(s) + 2 CH3COOH Ca(CH3COO)2(aq) + CO2(g)• Note: Calcium carbonate may be stored at or near the CO2Desorption or Displacement location.• Note: Acetic acid may be stored at or near the CO2Desorption or Displacement location,• Note: CO2Desorption or Displacement may be located at an application requiring carbon dioxide, or high purity carbon dioxide, or high pressure carbon dioxide, or captured carbon dioxide, or any combination thereof. For example, CO2Desorption or Displacement may be located at a site requiring CO2enhanced oil recovery (EOR).• Note: Calcium acetate may comprise an aqueous calcium acetate solution,, or calcium acetate solid, or any combination thereof.• Note: Calcium acetate may be stored at or near the CO2Desorption or Displacement, Calcium acetate may be transported to an application using calcium acetate. Calcium acetate may be transferred to at or near the Regeneration location. In some embodiments, the CO2desorption or displacement location may be the same as Regeneration location. In some embodiments, the CO2desorption or displacement location may be different than the Regeneration location. For example, in some embodiments, it may be desirable for the CO2Desorption or Displacement to be located at multiple distributed sites, while the Regeneration may be conducted at a larger and / or more centralized facility or site.. Note: Acetic acid vapor may be present in the CO2(g), In some embodimeuts, acetic acid vapor may be at least partially removed from CO2(g) by, for example, including, but not limited to, one or more or any combination of the following: contacting CO2(g) comprising a portion of acetic acid vapor with CaCO2, or contacting CO2(g) comprising a portion of acetic acid vapor with sodium carbonate, or contacting CO2(g) comprising a portion of acetic acid vapor with an alkali carbonate, or compression, or cooling, or condensing, or cryo-separation, or freeze separation.

[0479] (3) Regeneration: Calcium acetate may be reacted with sulfur dioxide to produce calcium sulfite. Calcium sulfite may be converted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to form a calcium hydroxide suspension, such as milk of lime.

[0480] Ca(CH3COO)2(aq) + SO2(g or aq) CaSO3(s) + 2 CH3COOH(aq)

[0481] CaSOAs) → CaO(s )+ SO2(g)

[0482] CaO(s) + H2O(g or 1) Ca(OH)2(s or aq)

[0483] Note: Calcium oxide or calcium hydroxide may be transported to the CO2Absorption or Adsorption location.

[0484] Note: Acetic acid may be transported to the CO2Desorption or Displacement location.

[0485] Note: It may be desirable for the regeneration to comprise a centralized facility, or a facility which may benefit from economies of scale, or any combination thereof

[0486] Example. 26: CO2Capture with Decoupled CO2Absorption or Adsorption,CO3, Desorption or Displacement, and Reagent Regeneration

[0487] (I) CO2Absorption: CO2may be absorbed or adsorbed in calcium oxide, or calcium hydroxide, or calcium hydroxide suspension, such as milk of lime, or any combination thereof io produce calcium carbonate solid or suspension.

[0488] Ca(OH)2(s or aq) + CO2(g) CaCO3(s) + H2O (1 or g)

[0489] (2) CO2Desorption or Displacement: Calcium carbonate- may be reacted with aqueous sulferous acid to produce calcium sulfite and carbon dioxide.

[0490] CaCO3(s) + SO2(aq) -> CaSO3(s) + CO2(g). Note: SO3(g) vapor may be present in the CO2(g), In some embodiments, SO2(g) may be at least partially removed from CO2(g) by, for example, including, but not limited to, one or more or any combination of the following: con tacting CO2(g) comprising a portion of SO3(g) with CaCO3, or contacting CO2(g) comprising a portion of SOfog) with sodium carbonate, or contacting CO2(g) comprising a portion of SOi(g) with an alkali carbonate, or compression, or cooling, or condensing, or eryo-separatioik or freeze separation.

[0491] (3) Regeneration: Calcium sulfite is converted into calcium oxide arid sulfur dioxide. Calcium oxide is reacted with water to form a calcium hydroxide suspension, such as milk of lime.

[0492] CaSO3(s) CaO(s) SO2(g)(M93| CaO(s) H2O(g or 1) -> Ca(OH)2(s or aq)

[0494] Example 27 ; CO2Capture with Decoupled CO2Absorption or Adsorption, CO2Desorption or Displacement, and Reagent Regeneration

[0495] (I) C02 Adsorption: CO2adsorption or absorption in calcium oxide or calcium hydroxide to produce calcium carbonate solid

[0496] CaO(s) + CO2(g) -> CaCO;(s)

[0497] Ca(OH)2(s or aq) + CO2→(g) CaCO3(s) + H2O(1 or g)

[0498] (2) CO2Desorption or Displacement: Calcium carbonate may be reacted with acetic acid to produce calcium acetate and carbon dioxide.

[0499] CaCO3(s) + 2 CH3COOH → Ca( CH3COO)2(aq) + CO2(g)

[0499] (3) Regeneration: Calcium acetate may be reacted with sulfur dioxide to produce calcium sulfite. Calcium sulfite is converted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to form a calcium hydroxide. In some embodiments, calcium hydroxide may form due io reaction of calcium oxide with water vapor.

[0501] Ca( CH3COO)2(aq.) + SO2(g or aq)→ CaSO3(s) + 2 CH3COOH(aq)

[0502] CaSO3(s) → CaO(s) • + SO2(g))

[0503] CaO(s) t- H2O(g or 1) Ca(OH)2(s or aq)

[0504] Example 28: CO2. Capture with Decoupled CO2Absorption or Adsorption, CO2Desorption or Displacement, and Reagent Regeneration

[0505] (1) CO2Adsorption: CO2adsorption or absorption in calcium oxide or calcium hydroxide to produce calcium carbonate solid.

[0506] CaO(s) + CO2(g) CaCO3(s)

[0507] Ca(OH)2(s or aq) + CO2(g) → CaCO3(s) + H2O(1 or g)

[0508] (2) CO2Desorption or Displacement: Calcium carbonate may be reacted with sulfurous acid to produce calcium sul fite and carbon dioxide.

[0509] CaCO2(s) + 2 CH3COOH. → Ca(CH3COO)2(aq) CO2(g)

[0510] (3) Regeneration: Calcium sulfite may be converted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to form a calcium hydroxide. In some embodiments, calcium, hydroxide may form due to reaction of calcium oxide with water vapor.

[0511] Ca(CH3COO)3(aq) + SO2(g or aq) → CaCO3(s) + 2 C&COOH(aq)

[0512] CaSO3(s) → CaO(s)+ SO2(g)

[0513] CaO(s) + H2O(g or 1) Ca(OH)2(s or aq)

[0514] Example 29: CO2Capture with Decoupled CO2Absorption or Adsorption, CO2Desorption or Displacement, and Reagent Regeneration

[0515] (1) CO2Absorption: CO2absorption In sodium hydroxide solution to produce sodium carbonate solution or sodium carbonate precipitate. If sodium carbonate precipitate forms, sodium carbonate precipitate may be separated using, for example, a sotid-liquid separation method.

[0516] 2 NaOH(aq or s) + CO2(g) → Na2CO3.(aq or s) + H2O(1 or aq or g)

[0517] Notes Sodium hydroxide solid or solution may be transported to the absorption location and / ' or stored at or near the absorption location.

[0518] Note: Sodium carbonate may be stored at or near the absorption or adsorption location. Sodium carbonate may be transported to an application using calcium carbonate. Sodium carbonate may be transferred to the CO2desorption or displacement location. In some embodiments, the CO2desorption or displacement location may be the same as the CO2absorption or adsorption location. In some embodiments, the CO2desorption or displacement location may be different than the CO2absorption or adsorption location. For example, in some embodiments, it may be desirable for the CO2absorption or adsorption to be located at multiple distributed sites, while the Regeneration may be conducted at a larger and / or more centralized facility or site.

[0519] (2) CO2Desorption or Displacement: Sodium carbonate may be reacted with acetic acid to produce sodium acetate and carbon dioxide,

[0520] Na2CO3.(aq or s) + 2 CH3COOH 2 NaCH3COO + CO2(g)• Motet Sodium carbonate may be stored at or near the CO2Desorption or Displacement location,. Note: Acetic acid may be stored at or near the CO2Desorption or Displacement location,• Note: CO2Desorption or Displacement may be located at an. application requiring carbon dioxide, or high purity carbon dioxide, or high pressure carbon dioxide, or captured Carbon dioxide, or any combination thereof. For example, CO2Desorption or Displacement may be located at a site requiring CO2enhanced oil recovery (EOR).* Note: Sodium acetate may comprise an aqueous calcium acetate solution, or sodium acetate solid, or any combination thereof.• Note: Sodium acetate may be stored at or near the CO2Desorption or Displacement. Sodium acetate may be transported to an application using sodium acetate. Sodium acetate may be transferred to at or near the Regeneration location. In some embodiments, the CO2desorption or displacement location may be the same as Regeneration location. In some embodiments, the CO2desorption or displacement location may be different than the .Regeneration location. For example, in some embodiments, it may be desirable for the CO2Desorption or Displacement to be located at multiple distributed sites, while the Regeneration may be conducted at a larger and / or more centralized facility or site.. Note: Acetic acid vapor may be present in the CO2(g) . In some embodiments, acetic acid vapor may be at least partially removed from CO2(g) by, for example, including, but not limited to, one or more or any combination of the following; contacting CO2(g) comprising a portion of acetic acid vapor with CaCO2, orcontacting CO2(g ) comprising a portion of acetic acid vapor with sodium carbonate, or contacting CO2(g )comprising a portion of acetic acid vapor with an alkali carbonate, or compression, or cooling, or condensing, or cryo-separation or freeze separation.

[0521] (3) 'Regeneration : Sodium acetate may be reacted with sulfur dioxide to produce sodium sulfite and acetic acid. Sodium sulfite may be separated from acetic acid. Sodium sulfite may be reacted with calcium hydroxide, or calcium oxide, or calcium hydroxide suspension, or any combination thereof to produce sodium hydroxide and calcium sulfite. Calcium sulfite solid may be separated from sodium hydroxide solution. Calcium sulfite solid may be con verted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to produce calcium hydroxide or calcium hydroxide suspension.

[0522] 2 NaCH3COO + SO2(g or aq) Na2SO3(aq or s) + 2 CH3COOH(aq)

[0523] Separate NatSO3and 2 CH3COOH

[0524] Na2SO3(aq or s) + Ca(OH)2(s or aq) CaSO3(s) + 2 NaOH

[0525] CaSO3(s) → CaO(s) e SO2(g)

[0526] CaO(s) H2O(g or 1) Ca(OH)2(s or aq)• Note: Sodium hydroxide may be transported to the CO3Absorption or Adsorption location,• Note: Acetic acid may be transported to the CO2Desorption or Displacement location.• Note: It may be desirable for the regeneration to comprise a centralized facility, or a facility which may benefit from economies of scale, or any combination thereof

[0527] Example 30: CO2Capture with Decoupled CO2Absorption or Adsorption,CO2.Desorptiou or Displacement, and Reagent Regeneration

[0529] (I) CO2Absorption; CO2absorption in sodium hydroxide solution to produce sodium carbonate solution, or solid precipitate, or any combination thereof.

[0529] 2 NaOH(aq or s) + CO2(g) Na2CO3(aq or s) + H2O(1 or aq or g)

[0530] (2) CO2Desorption or Displacement: Sodium carbonate may be reacted with aqueous sulfurous acid or aqueous sulfur dioxide to produce sodium sulfite and carbon dioxide.

[0531] Na2CO3(aq or s) SO2(aq) → Na2SO3(aq or s) + CO2(g)• Note: SO2(g) vapor may be present in the CO2(g). In some embodiments, SO2(g) may be at least partially removed from CO2(g) by, for example, including, but not limited to, one or more or any combination of the following: contacting CO2(g) comprising a portion of SO2(g) with CaCOy or contacting CO2(g) comprising a portion of SO2(g) with sodium carbonate, or contacting CO2(g) comprising a portion of SO2(g) with an alkali carbonate, or compression, or cooling, or condensing, or cryo-separation, or freeze separation.

[0532] (3) Regeneration: Sodium sulfite may be reacted with calcium hydroxide, or calcium oxide, or calcium hydroxide suspension, or any combination thereof to produce sodium hydroxide and calcium sulfite. Calcium sulfite solid is separated from sodium hydroxide solution. Calcium sulfite solid is converted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to produce calcium hydroxide or calcium hydroxide suspension.

[0533] Na2SO3(aq or s)+ Ca(OH)2(s or aq) CaSO3(s) + 2 NaOH(aq or s)

[0534] CaSO3(s) → CaO(s+) SO2(g)

[0535] CaO(s+) H2O(g or 1) Ca(OH)2(s or aq)

[0536] Example 31 ; CO2Production and Production of Sodium Hydroxide

[0537] (I) CO2Desorption or Displacement: Sodium bicarbonate, which may compriseNahcolite, may be reacted with aqueous sulfurous acid or aqueous sulfur dioxide to produce sodium sulfite and carbon dioxide,

[0538] 2 NaHCO3(aq or s)+ SO2(aq) Na2SO3(aq or s) + H2O + 2 CO2(g) O22 NaHCO2(aq or s) + 2 SO2(aq) → NaHSO3(aq or s) + 2 CO2(g)

[0539] (2) Production of Sodium Hydroxide: Sodium sulfite may be reacted with calcium hydroxide, or calcium oxide, or calcium hydroxide suspension, or any combination thereof to produce sodium hydroxide and calcium sulfite. Calcium sulfite solid is separated from sodium hydroxide solution. Calcium sulfite solid is converted into calcium, oxide and sulfur dioxide. Calcium oxide may be reacted with water to produce calcium hydroxide or calcium hydroxide suspension.

[0540] Na2SO3(aq or s)+ Ca(OH)2(s or aq) → CaSO3(s) 2 NaOH(aq or s)

[0541] CaCO3(s) CaO(s) + SOrtg)

[0542] CaO(s) + H2O(g or 1) Ca(OH)2(s or aq)

[0543] Example 31 ; CO2Production and Production of Sodium Hydroxide

[0544] (2) CO3Desorption or Displacement: Sodium bicarbonate, which may compriseNahcolite, may be reacted with acetic acid to produce sodium acetate and carbon dioxide,

[0545] 2 NaHCO3.(aq or s) 4 2 CH3COOH → 2 NaCHCOO+ 2 CO2.(g)

[0546] (3) Regeneration: Sodium acetate may be reacted with sulfur dioxide to produce sodium sulfite and acetic acid. Sodium sulfite is separated from acetic acid. Sodium sulfite may be reacted with calcium hydroxide, or calcium oxide, or calcium hydroxide suspension, or any combination thereof to produce sodium hydroxide and calcium sulfite. Calc ium sulfite solid is separated from sodium hydroxide solution. Calcium sulfite solid is converted into calcium oxide and sulfur dioxide. Calcium oxide may be reacted with water to produce calcium hydroxide or calcium hydroxide suspension.

[0547] 2 NaCH3COO+ SO2(g or aq) Na2SO3.(aq or s) 42 CH3COOH(aq)

[0548] Separate Na2SO3and 2 CH3COOH

[0549] Na2SO3(aq or s) + Ca(OH) (1 or aq) CaSO3(s) + 2 NaOH

[0550] CaSO3(s) → CaO(s+) SOAg)

[0551] CaO(s+) H2O(g or 1) Ca(OH)2(s or aq)

[0552] Example 32: Lithium Hydroxide Production from Lithium Sulfate usingCalcium Precipitation and Acid Intermediate

[0553] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Add Anion with Acetic Acid* CaCO3(s or aq)+ 2 CH3COOH(aq) Ca( CH3COO)2(aq) CO2(g)• Calcium Silicate(s) + 2 CH3COOH(aq) Ca( CH3COO)2(aq) Silicon Dioxide(s)• CaS(s) + 2 CH3COOH (aq) Ca( CH3COO)2(aq) + H2S(g)* Calcium(Weak Acid Anion+) 2 CH3COOH(aq) Ca( CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq)0554] Note: Residual solids orundissolved ved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a sol id-liquid separation.

[0555] (2) Ca( CH3COO)2(aq) + Li2SO4( aq) → 2 LiCH3COO(aq) + CaSO3(s)

[0556] (3) 2 LiCH3COO(aq) + SO2(g or aq) + H2O(1 or aq) → Li2SO3( aq) + 2 CH3COOH(aq)

[0557] (4) Li2SO3( aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq or 1) + Li2SO3(s) + Water

[0558] Note: CH3COOH may be more soluble in water than Li2SO3, In some embodiments, water may be removed and / or Li2SO3may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0559] Note: Li2SO3(s) may be separated from CH3COOH(aq or 1) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0560] (5) Li2SO3( s or aq) + Ca(OH)2(s or aq) 2 LiOH(aq or s) + CaSO3(s)

[0561] Note: Ca(OH)2(1 or aq m) ay comprise a solid-liquid suspension, such as milk of lime.

[0562] Note: CaSO3(s) may be separated using a solid-liquid separation.

[0563] (6) CaSO3(s) CaO(s) + SO2(g)

[0564] Note: ‘(6) ' may comprise calcining CaSO3(s), which may employ a kiln.

[0565] Note: CaSO3(s) may be dried, or dehydrated, or both before or during '(6)’,

[0566] (7) CaO(s) + Water(g or 1 or aq) Ca(OH)2(s or aq)

[0567] Note: CaO(s) may be employed to remove water vapor or facilitated drying of Ca SO3(s) before or daring decomposition of CaSO3(s) to CaO(s).

[0568] (8) 2 LiOH(aq or s) 2 LiOH(s) + Water}0569( Note: In some embodiments, water may be removed and / or LiOH may be separated or precipitated by, for example, including, but not limited to, evaporation, or3istillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[9570] Note: In some embodiments, it may be desirable for LiOH to comprise a concentrated aqueous solution.

[0571] Example 33 : Sodium Hydroxide Production from Sodium Chloride usingCalcium Precipitation, Acid Intermediate, and Process for Producing Sodium Sulfate and Calcium Chloride from Calcium Sulfate and Sodium Chloride

[0572] (I) React Material comprising Calcium, or Maguesium, or Other Alkaline Earth --Weak Acid Anion with Acetic Acid + CaCO3(s or aq) 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g)• Calcium Silicate(s) + 2 CH3COOH(aq) → Ca( CH3COO)2(aq) + Silicon Dioxide(s) • CaS(s) + 2 CH3COOH (aq) → Ca(CH3COO)2(aq) + HzS(g)• CaIcium(Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH,COO)2(aq) +• Weak Aeid(s, or g, or 1, (1 or aq)[0573[ Note: Residual solids or undissol ved solids, such as silicon dioxide or otherundissolved solids, may be separated from the liquid solution using a solid- liquid separation.

[0574] (2) Ca(CH3COO)2(aq) + Na2SO3(s or aq) 2 NaCH3COO(aq) + CaSO3(s)

[0575] Note: In some embodiments, Na2SO3(s (1 or aq m) ay be transferred from step ‘(IO)’.

[0576] (3) 2 NaCH3COO(aq) + SO2(g or aq) + HzO(l (1 or aq) Na2SO3(aq) + 2 CH3COOH(aq)

[0577] (4) Na2SO3(aq) + 2 CH3COOH(aq) -> 2 CIHCOOH(aq or 1) + NaSO3(s) + Water

[0578] Note: CH3COOH may be more soluble in water than Na2SOa, In some embodiments, water may be removed and / or Na2SO3may be separated or precipitated by, for example, .including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described In the art, or any combination thereof.

[0579] Note: CaSO3(s) may be separated from CH3COOH(aq or 1) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation, systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0580] (5) Na2SO3(s or aq) + Ca(OH)2(s or aq) 2 NaOH(aq or s) + CaSO3(s)

[0581] Note: Ca(OH)2(s (1 or aq m) ay comprise a solid-liquid suspension, such as milk of lime.

[0582] Note: CaSO3(s) may be separated using a solid-liquid separation,

[0583] (6) CaSO3's) CaO(s) + SO2(g)]0584] Note: ‘(h)’ may comprise calcining CaSOfrs), winch may employ a kiln,

[0585] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘ (6)2

[0586] (7) CaO(s) -t Water(g or 1 or aq) Ca(OH)2(s or aq)

[0587] Note: CaO(s) may be employed to remove water vapor or facilitated drying of Ca SO2(s) before or during decomposition ofCaSO3(s) to CaO(s).

[0588] (8) 2 NaOH(aq or s) -> 2 NaOH(s) Water|0589|: Note: In some embodiments, water may be removed and / or NaOH may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, orseparation systems or methods described in the art, or any combination thereof.

[0590] Note: In some embodiments, it may be desirable for NaOH to comprise a concentrated aqueous solution,

[0591] (9) CaSO4s (1 or aq ) + (NH4)2CO3(aq) CaCO3(s (1 or aq ) +]0592] Note: CaSO4(s or aq) may be transferred from step ‘(2)2

[0593] Note: CaCO3(s) may be separated from a solution comprising CNH^SO3(aq) by a sol id-1 iquid separation ,

[0594] (10) + 2 NaCl(aq) →(1 or aq)

[0595] Note: In some embodiments, a portion of Na2SO4s) maybe precipitated by cooling precipitation: due to, for example, the increasingly lower solubili ty of NaeSO2in water compared to NH4Cl fee lower fee temperature below about 32 degrees Celsius or fee closer the temperature of the solution is to 0°C.]0596] Note: In some embodiments, Na2SO4may be separated from 2NHC1 by evaporation, or crystallization, or cooling precipi tation, or any combination thereof. In someembodiments, Na2SO4(s), or water, oror any combination thereof may be produced or may form.

[0597] (II) One, or more, or any combination of the following: +•»

[0598] Note: CaCO3(s) may be iransfeired from step ‘(9)'.

[0599] Note: One or more or any combination of the above reactions may require heat input.

[0600] Note: In some embodiments, heat may be recovered from one or more or any combination of reactions. For example, the calcium carbonate and hydrogen chloride may be exothermic.

[0601] Note: In some embodiments. 2 NH4Cl(s) may be precipitated or crystallized from an aqueous solution in the presence of calcium carbonate to, for example, create a distributed m ixture of calcium carbon ate and ammon ium chloride.

[0602] Note: Calcium chloride may comprise an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may comprise a waste product.

[0603]

[0604] Note may be transferred to step ‘(9)’.

[0605] Note or CO2(g), or any combination thereof may berecycled or recirculated. within the process. In some embodiments, losses may occur and / or make up 2 NH3, or H3O, or CO2, or any combina tion thereof may be added.

[0606] Example 34: Process for Producing Sodium Sulfate, Ammonia, and Calcium Chloride from Ammonium Sulfate, Sodium Chloride. and Calcium- Weak Acid

[0607]

[0608] Note: In some embodiments, a portion of Na2SO4(s) may be precipitated by cooling precipitation due to, for example, the increasingly lower solubili ty of Na2SQt inwater compared to NH4Cl the lower the temperature below about 32 degrees Celsius or the closer the temperature of the solution is to 0°C,

[0609] Note; In some embodiments, Na2SO4may be separated from 2Nl-riCl by evaporation, or crystallization, or cooling precipitation, or any combination thereof. In some embodiments, Na2SO4s), or water, or 2NH4Cl(aq), or 2NH4C1(S), or any combination thereof may be produced or may form.

[0610] (2) One, or more, or any combination of the following;• 2NH4C1(S) -> 2 NH3(g) + 2 HCl(g)» 2 NH3(g)+2 HCl(g) + CaCOds)’→ CaCl2(s) + H2O(g) + CO2(g) +- 2 NH3(g)• CaCO3(s) + 2 NHtCKs) → CaCh(s) + IfrCKg) + CO2(g) + 2 NH3(g)• 2 Nft(g) + 2 HCl(g) + Ca(WA)(s)→ CaCh(s) i- H2O(g) + WA(s or g or I) -4 2 Nffog)• Cat' WAXs) + 2 NH3Cl(s) CaCh(s) + IliO(g) + WA(s or g or 1) t- 2 N'H3(g)

[0611] Note: One or more or any combination of the above reactions may require heat input.

[6612] Note: In some embodiments, heat may be recovered from one or more or any combination of reactions. For example, the calcium carbonate and hydrogen chloride may be exothermic.

[0613] Note: In some embodiments, 2 NH3CKs) may be precipitated or crystallized from an aqueous solution in the presence of calcium - weak acid to, for example , create a distributed mixture of calcium - weak acid and ammonium chloride.

[0614] Note: Calcium chloride may comprise an output. In. some embodiments, calcium chloride may be sold or utilized, in some embodiments, calcium chloride may comprise a waste product.

[0615] Note: In some embodiments, carbon dioxide produced may comprise captured carbon dioxide. For example, ammonia and / or water may be separated from carbon dioxide using an aqueous solution and / or high pressures and / or elevated temperatures.

[0616] Example 35: Process for Producing Sodium Sulfate and Calcium Chloride from Sodium Chloride and Calcium Sulfate usmg an Ammonia and Carbon Dioxide Intermediate)0617] (1)

[0618] Note may comprise an input. For example, CaSO3('s) may be aproduct or byproduct from a process. For example, CaSCfr(s) may be mined. For example, CaSO4s) may comprise phosphogypsum.

[0619] Note: CaCO3(s) may be separated front a solution comprising (NH4)2SO4(aq) by a solid-liquid separation ,

[0620] (2) (NH4)2SO4(aq)+2 NaCl(aq) 2 NH4Cl(aq) + Na2SOafs or aq)

[0621] Note: In some embodiments, a portion of Na2SO4(s) may be precipitated by cooling precipitation due to, for example, the increasingly lower solubility ofNa2SO4in water compared to NH4Cl the lower the temperature below about 32 degrees Celsius or the closer the temperature of the solution is to 0°C.

[0622] Note: In some embodiments. Na2SO4may be separated from 2 NH4Cl by evaporation, or crystallization, or cooling precipitation, or separation method described herein, or any combination thereof, In some embodiments, Na2SO4(s) , or water, or SNH4Cl( aq), or 2NH4Cl(S), or any combination thereof may be produced or may form.

[0623] (3) One, or more, or any combination of the following.'•••|<I624| Note: CaCO3(s) may be traasferred: from step ‘( 1 )’.

[0625] Note: One or more or any combination of the above reactions may require heat input

[0626] Note: In some embodiments, heat may be recovered from one or more or any combination of reactions. For example, the calcium carbonate and hydrogen chloride may be exothermic.

[0627] Note: In some embodiments, 2 NH4Cl(s) may be precipitated or crystallized from an aqueous solution in the presence of calcium carbonate to, for example, create a distributed mix lure of calcium carbonate and ammonium chloride.

[0628] Note: Calcium chloride may comprise an output. in some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may comprise a waste product.

[0629]

[0630] Note;

[0631] Note: 2 NH3(g), or H2O(g), or CO2( g), or any combination thereof may be recycled or recirculated. within the process. In some embodiments, losses may occur and / or make up 2 NH3or IM), or CO3, or any combination thereof may be added.

[0632] Example 36; P roc ess for Product Sodium Sulfate and Calci um Ch Io ride from Sodium Chloride and Calcium Sulfate while Capturing Carbon Dioxide

[0633]

[0634] Note: CO2(g) may comprise a gas comprising CO2(g) In some embodiments, the CO2(g) may comprise a gas comprising a dilute coneentration of carbon dioxide, which may include, but is not limited to, flue gas, or emissions gas, or sour gas, or air, or other CO2sources described herein, or other CO2sources in the art, or any combination thereof.

[0635]

[0636] Note: CaSO3(s (1 or aq m) ay comprise an input. For example, may be aproduct or byproduct from a process. For example, may be mined. For example,CaSO4(s) may comprise phosphogypsum.

[0637] Note: CaCO3(s) may be separated from a solution comprising (NH4)2SO4(aq) by a solid-liquid separation.

[0638] (3)

[0639] Note: In some embodiments, a portion of (NH4)2SO m4(aaqy) be precipitated by cooling precipitation due to, for example, the increasingly lower solubility of Na2SO4in water compared to NH4Cl the lower the temperature below about 32 degrees Celsius or the closer the temperature of the solution is to IFC.

[0640] Note: In some embodiments, Na2SO4may be separated from 2NH4Cl by evaporation, or crystallization, or cooling precipitation, or separation method described herein, or any combination thereof. In some embodiments, Na2SO4(s), or water, or or any combination thereof 'may be produced or may form.

[0641] (4) One, or more, orany combination of the following;•••

[0642] Note: CaCO3(s) may be transferred from step '(1)'

[0643] Note: One or more or any combination of the above reactions may require heat mput.

[0644] Note: in some embodiments, heat may be recovered from one or more or any combination of reactions. For example, the calcium carbonate and hydrogen chloride may be exothermic.

[0645] Note: In some embodimentsmay be precipitated or crystallized from an aqueous solution in the presence of calcium carbonate to, for example, create a distributed mixture of calcium carbonate and ammonium chloride.

[6646] Note: Calcium chloride may comprise an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may emprise a waste product.

[0647] (5)

[0648] Note: 2 NHfraq) may be transferred to step ‘(1)2

[0649] Note: If conducted at a pressure greater than 0.9 atm, or I atm, or 1.2 atm, or I .4 atm, or 1 .6 atm, or 1.8 atm, or 2 atm, or 2.5 atm, or 3 atm, or 4 atm, or 5 atm, or any combination thereof and / or temperature greater than 50°C, 60°C, or 70°C, or 80°C or 90°C or 100°C, or 110°C , or 120°C, or 130°C or any combination thereof in the presence of liquid water, ammonia may mostly transfer to the aqueous phase, while carbon dioxide may mostly remain at a gas phase .

[6650] Note: In some embodiments, CO2may be further purified to remove residual ammonia. For example, CO2(g) comprising residual ammonia may be cooled, which may result in the removal of at least a portion of the residual ammonia by the formation of ammonia - carbon dioxide derivative salts, such as ammonium carbamate, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof. For example, CO2.(g) comprising residual ammonia may be cooled and / or contacted with water, which may resultin the removal of at least a portion of the residual ammonia by the formation of aqueous ammonia, or ammonia ••• carbon dioxide derivative salts, such as ammonium carbamate, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof.

[0651] Example 37: Process for Producing Sodium Sulfate, Calcium Chloride, and[0652[ (1)

[0653] Note: CO2(g) may comprise a gas comprising CO2tg). In some embodiments, the CO)2g) may comprise a gas comprising a dilute concentration of carbon dioxide, which may include, but is not limited to, flue gas, or emissions gas, or sour gas, or air, or other CO2sources described herein, or other CO2sources in the art, or any combination thereof.

[0654] (2)

[0655] Note: q m) ay comprise an input. For example may be aproduct or byproduct from a. process. For example,may be mined. For example, CaSO4(s) may comprise phosphogypsum.

[0656] Note: CaCORs) may be separated from a solution comprising (NH4)2SO4(aq) by a solid-Iiqu id separation .

[0657] (3) (NH4)2SO4(aq) + 2 NaCl(aq) 2 NH4Cl(aq) + Na2SO4s or aq)

[0658] Note: In some embodiments, a portion of Na2SO4(s) may be precipitated by cooling precipitation due to, for example, the increasingly lower solubility ofNa2SO* in water compared to NH4Cl the lower the temperature below about 32 degrees Celsius or the doser the temperature of the solution is to 0°C.

[0659] Note: In some embodiments, Na2SO4may be separated from 2NH4Cl by evaporation, or crystallization, or cooling precipitation, or separation .method described herein, or any combination thereof. In some embodiments, Na2SO Rs), or water, oror any combination thereof may be produced or may form.

[0660] (4) One. or more. Or any combination of the following:•••

[6661] Note: CaCO3(s) may be transferred from step ‘( 1 )’.

[0662] Note: One or more or any combination of the above reactions may require heat input

[0663] Note: In some embodiments, heat may be recovered from one or more or any combination of reactions. For example, the calcium carbonate and hydrogen chloride may be exothenme.

[0664] Note: In some embodiments,may be precipitated or crystallized ftom an aqueous solution in the presence of calcium carbonate to, for example, create a distributed mixture of calcium carbonate and ammonium chloride.

[0665] Note: Calcium chloride may comprise an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may comprise a waste product.

[0666] (5) 2

[0667] Note: if conducted at a pressure greater than 0.9 atm, or 1 atm, or 1 .2 atm, or 1 .4 atm, or 1.6 atm, or 1.8 atm, or 2 atm, or 2,5 atm, or 3 atm, or 4 atm, or 5 atm, or any combination thereof and / or temperature greater than 50°C, 60°C, or 70°C, or 80°C or 90°C or 100°C, or 110°C , or 120°C, or 130°C or any combination thereof in the presence of liquid water, ammonia may mostly transfer to the aqueous phase, while carbon dioxide may mostly remain at a gas phase.

[0668] (6)

[0669] (7)

[0670] Note: The process may produce urea and / or water.

[0671] Note: it may be desirable to further dry the ammonia, or carbon dioxide, or both before use in the production of urea.

[0672] Example 38: Sodium Hydroxide Production from Sodium Sulfate using Calcimn Precmitation and Acid I ntermediate

[0673] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid + +*+ CalciumfWeak Acid Anion)Acidfs, or g, or I, or aq)

[0674] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution usings solid* liquid separation,

[0675] (2)

[0676] (3)CH3COOH(aq)

[0677] (4)separate)

[0678] Note: Aft aqueous solution comprising sodium sulfite and acetic acid may be separated into a separate aqueous solution comprising acetic acid and a separate aqueous solution comprising sodium sulfite using, for example, electrodialysis, or electrodialysis reversal, or selective electrodialysis.

[0679] Note: For example, some embodiments may employ electrodialysis selective for monovalent or divalent or trivalent or tetravalent cations, or monovalent or divalent or trivalent or tetravalent anions, or any combination thereof.

[0680] Note: The aqueous solution compri sing acetic acid may be employed as the aqueous acetic acid in step ‘(1)2

[6681] (5)

[0682] Note: (1 or aq m) ay comprise a solid-liquid suspension, such as milk oflime.

[0683] Note: CaSO3(s) may be separated using a solid-liquid separation.

[0684] (6)

[0685] Note: “(6)' may comprise calcining CaSO3(s), which may employ a kiln.

[0686] Note: may be dried, or dehydrated, or both before or during ‘(6)2

[0687] (7)

[0688] Note: CaO(s) may be employed to remove water vapor or facilitated drying of CaSO3(s) before or during decomposition of

[0689] (8) 2 NaOH(aq) 2 NaQH(aq or s)4Water

[0690] Note: In some embodiments, it may be desirable for NaOH to comprise an aqueous solution or concentrated aqueous solution. In some embodiments, NaOH(aq) may be concentrated or further concentration using one or more or any combination of separation methods or water removal methods.

[0691] Note: In some embodiments, water may be removed and / or .NaOH may be separated or precipitated by, for example, including, but not limited io, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0692] Note: Water or distillate from concentrating or further concentrating may be employed within the process. For example, water or distillate from concentrating or further concentrating may be employed to, for example, including but not limited to, one or more or any combination of the following: to dissolve sodium sulfete, or to absorb ace tic acid vapor, or dilute or mix with the aqueous solation comprising sodium acetate, or dilute or mix with the aqueous solution comprising sodium sulfite and acetic acid, or any combination thereof.

[0693] Example 39: Sodium Hydroxide and Calcium Oxide Production fromSodium Sulfate and Calcium Carbonate using Calcium Precipitation and Acid Intermediate

[0694] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••Acid(s, or g, or 1, or aq)

[0695] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution, using a solid-liquid separation.

[0696] (2

[0697] (3[0698| (4)

[0699] (5)

[0700] Note: In some embodiments, may be conducted under high CO2partial pressures and / or elevated temperatures. For example, some embodiments may employ CO2partial pressures greater than I Bar, or 2 Bar, or 3 'Bar, or 4 Bar, or 5 Bar, or any combination thereof and for temperatures greater than

[0701] Note: CO2may be sourced from, including, but not limited to, one or more or any combination of the following: the decomposition of sodium bicarbonate, or captured carbon dioxide, or any combination thereof.

[0702] (0703 )

[0704]

[0705]

[0706]

[0707]

[0708]

[0709] Note: In some embodiments, calcium carbonate may be decomposed into calcium oxide in a manner which produces high purity or captured carbon dioxide. For example, in some embodiments, calcium carbonate may be calcined or decomposed by indirect calcination or indirect heating, which may -result in the production of high purity or captured carbon dioxide.

[0710] Note: Captured carbon dioxide may be sequestered or employed in one or more or any combination of applications.

[0711] (13)

[0712] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous sol ution, or solid-liquid suspension, or milk of lime, or solid, or any combination thereof comprising calcium hydroxide,

[0713] Note: In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium carbonate to produce calcium carbonate and sodiumhydroxide. For example, in some embodiments, step ‘(10)’ may be combined with step

[0714] Example 40: Sodium Carbonate or Sodium Bicarbonate Production from Sodium Sulfate using Calcium Predpitation and Acid Intermediate

[0715] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••Aeid(s, or g, or 1, or aq)

[0716] Note: Residual sol ids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0717] (2)(3)|0719( (4)

[0720] (5)

[0721] Note: In. some embodiments, may be conducted under high CO2, partial pressures and / or elevated temperatures. For example, some embodiments may employ CO2partial pressures greater than 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or any combination thereof and / or temperatures greater than or

[0722] Note: CO2may be sourced from, including, but not limited to, one or more or any combination of the following: the decompositioii of sodium bicarbonate, or captured carbon dioxide, or any combination thereof.

[0723] (6)

[0724] (7)

[0725] (8)

[0726] (9)

[0727] (10

[0728] Example 41 : Sodium Hydroxide Production from Sodium Sulfate using Calcium Precipitation, Arid Intermediate and Calcium Carbonate Intermediate

[0729] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth —Weak Acid Anion with Acetic Acid• • •*Acidfs, or g, or 1, or aq)

[0730] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0731] jft732|

[0733] (4)

[0734] (5)

[0735] Note: In some embodiments, may be conducted under high CO2partial pressures and / or elevated temperatures. For example, some embodiments may employ CO2partial pressures greater than 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, of 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or 11 Bar, or 12 Bar, or 13 Bar, or .14 Bar, or 15 Bar, or any combination thereof and / or temperatures greater than

[0736] Note: CO2may be sourced from, including, but not limited to, one or more or any combina tion of the following: the decomposition of sodium bicarbonate, or captured carbon dioxide, or any combination thereof

[0737] (6)

[0738] (7)

[0739] (8)

[0740] Note: CaO(s) may be transferred to step ‘(9)’ or step

[0741] Note: SO2(g) may be transferred to step ‘(3),’

[0742] (9

[0743] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-liquid suspension, or milk of lime, or solid, or any combination thereof comprising calcium hydroxide.

[0744] Note: In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium carbonate to produce calcium carbonate and sodium hydroxide. In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium carbonate to produce calcium carbonate and sodium hydroxide, which may comprise combining step '(9)’ and step *(1 1).’

[0745] (10)

[0746] Note: CO2may be transferred to step '(5)\

[0747] (11) N

[0748] Note: An aqueous solution comprising sodium hydroxide may be separated from calcium carbonate by a solid-liquid separation.

[0749] Note: Calcium carbonate may be transferred to ‘(5)".

[0750] (12) Water

[0751] Note: The solution comprising sodium hydroxide may be .further concentrated, or at least a portion of water may be removed from the solution comprising sodium hydroxide, or any combination thereof.

[0752] Note: In some embodiments, at least a portion of the water removed or recovered from the solution comprising aqueous sodium hydroxide may be transferred to step;(6)’-

[0753] Example 42: Sodium ilydroxide Production from Sodium Sulfate andCalcium Carbonate using Calcium Precipitation and Carbon Dioxide Intermediate

[0754] (1)

[0755] Note: In some embodiments, may be conducted under high CO2partial pressures and / or elevated temperatures. For example, some embodiments may employ CO2partialpressures greater than 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or 1 1 Bar, or 12 Bar, or 13 Bar, or 14 Bar, or 15 Bar, or any combination thereof and for temperatures greater than

[1756] Note: CO2may be sourced from, including, but not limited to, one or more or any combination of the following; the decomposition of sodium bicarbonate, or captured carbon dioxide, or any combination thereof

[0757] (2)|0758( (3)

[0759] Note: CO2may be transferred to step ' ( 1 )'

[0760] (4)

[0761] Note: An aqueous solution comprising sodium hydroxide may be separated from calcium carbonate by a solid-liquid separation.

[0762] Note: Calcium carbonate may be transferred to '(5)’ .

[0763] (5) Water

[0764] Note: The solution comprising sodium hydroxide may be further concentrated, or at least a portion of water may be removed from the sol ution comprising sodium hydroxide, or any combination thereof

[0765] Note: In some embodiments, at least a portion of the water removed or recovered from the solution comprising aqueous sodium hydroxide may be transferred to step ‘ (1 ) ’ or step ‘(2)’.

[0766] (6)

[0767] Note: In some embodiments, calcium carbonate may be decomposed into calcium oxide in a manner which produces high purity or captured carbon dioxide. For example, in some embodiments, calcium carbonate may be calcined or decomposed by indirect calcination or indirect heating, which may result in the production of high purity or captured carbon dioxide.

[0768] Note: Captured carbon dioxide may be sequestered or employed in one or more or any combination of applications.

[0709] (7)

[0770] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-liquid suspension, or milk of lime, or solid, or any combination thereof comprising calcium hydroxide.

[1771] Note: In some ejnbodiments, calcium oxide may be reacted directly with a» aqueous solution comprising sodium carbonate to produce calcium carbonate and sodium hydroxide. For example, in some embodiments, step ‘(4)’ maybe combined with step ‘(7)’.(0772}

[0773]

[0774] Note: In some embodiments, may be conducted under high CO3partial pressures and / or elevated temperatures. For example, some embodiments may employ CO2partial pressures greater than .1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or 1 1 Bar, or 12 Bar, or 13 Bar, or 14 Bar, or 15 Bar, or any combination thereof and for temperatures greater than 0°C, or

[0775] Note: CO2may be sourced from, induding, but not limited to, one or more or any combination of the following: the decomposition of sodium bicarbonate, or captured carbon dioxide, or any combination thereof

[0776] (2)

[0777] Note: In some embodiments, NaHCO3(aq) or NaHCO3(s) may comprise a product which may be sold or utilized.

[0778] Note: 2 NaHCO3(aq) may be separated from at least a portion of CaSO4(s) by solid-liquid separation .

[0779] (3)

[0780] Note: CO2may be transferred to step ‘(O2-

[0782] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••|<)783} Note: Residual solids or undissolvcd solids, such as silicon dioxide or other undissoivcd solids, may be separated from the liquid, solution using a solid-liquid separation.

[0784] Nate.: CO2(g) may comprise captured CO2.

[0785] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[0786]

[0787] Note: CaSO3(s) may be separated using a solid-liquid separation,

[0788] Note: In some embodiments, residual aqueous magnesium sulfite may be present in the. In some embodiments, the residual aqueous magnesium sulfite may remain in the transferred to reaction '( 1)' from reaction ‘ . In someembodiments, the aqueous magnesium sulfite may remain in thetransferred to reaction ‘(I )’ from reaction ‘(2)’ because, for example, magnesium sulfite additional or accumulated magnesium sulfite above the solubility' limits of magnesium sulfite in the solution may precipitate or co-precipitate during the reaction of or) with SQ?(g (1 or aq o)r sulfite or bisulfite,

[0789] Note: In some embodiments, residual aqueous magnesium sulfite may be present In the ‘2 CTfeClOOH(aq)’. hr some embodiments, a portion of the residual aqueous magnesium sulfite may be concentrated and / or separated using, including, but not limited to, one or more, or any combination of the following: heating, or cooling, or reverse osmosis, or membrane based process, or precipitation, or electrodialysis, or forward osmosis, or any combination thereof. For example, the residual aqueous magnesium sulfite may be separated by concentrating the magnesium sulfite using reverse osmosis or nanofiltration, wherein thepore size or properties of the membrane may enable the permeation of at least a portion of the acetic ac id and the rejection of at least a portion of magnesium sulfite, and Z or cooling the .resulting concentrated magnesium sulfite solution, to produce at least a portion of a magnesium sulfite precipitate.

[0790] (3)

[0791] (4)

[0792] Note: ‘(4) * may be conducted at an elevated temperature to reduce the solubility or dissolution ofor reduce potential formation of CaSO3(aq).

[0793] (5) One or more or any combination of the following:•••

[0794] (6)

[0795] (7)

[8796] (8)

[0797] (9)

[0798] Example 45: Sodium Hydroxide Production from Sodium Sulfate usingCalcium Precipitation and Acid Intermediates

[0799] (1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth ~Weak Acid Anion with Acetic Acid

[0800] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0801]

[0802] (3)

[0863] Note: In some embodiments, other carboxylic acids than citric acid may be employed, such as carboxylic acids which form soluble sodium salts and relatively low solubility calcium salts.

[0804] (4)

[0805] Note: ‘(4)' may comprise separating sodium citrate from acetic acid. For example, sodium citrate may be separated from an aqueous solution comprising acetic acid or from acetic acid by distillation,

[0886] (5)

[0807] Note: Aqueous solution comprising sodium hydroxide may be separated from a solid comprising calcium citrate by a solid-liquid separation.

[0808] (6)

[0809] Note: In some embodiments, an aqueous solution comprising sodium hydroxide may be further concentrated, or water may be removed from the solution comprising sodium hydroxide, or any combination thereof, in some embodiments, the aqueous solution comprising sodium hydroxide may undergo further treatment. In some embodiments, the aqueous solution comprising sodium hydroxide may comprise a product and / or may be ready to be sold or utilized.

[0810] (7)

[0811] (8)

[0812] (9)

[0813] (10

[0814] Note: In some embodiments, CaO(s) may be reacted with water. In some embodiments, CaO(s) may be reacted with Sodium Citrate to produce Calcium Citrate and Sodium Hydroxide. In some embodiments, for example, step ‘(5)’ and step "(10)' may be combined.

[0815] Example 46: Process for Producing Calcium Oxide or Cement or Clinker with Ascorbic Acid Intermediate

[0816] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Ascorbic Acid, which may comprise, including, but not limited to, one or more or any combination of the following:»•••Weak Acidfs, or g, or 1, (1 or aq)

[0817] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, .may be separated from the liquid solution using a solid-liquid separation.

[0818] Note: COdg) may comprise captured CO3.

[0819] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium, In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[0820] (2)

[0821] Notemay be separated using a solid-liquid separation.

[0822] Note: In some embodiments, residual, aqueous magnesium sulfite may be present in the. In some embodiments, the residual aqueous magnesium sulfite may remain in the transferred to reaction h l)’ from reaction \ In someembodiments, the aqueous magnesium sulfite may remain in thetransferred to reaction ‘(1)’ from reaction ‘(2)’ because, for example, magnesium sulfite additional or accumulated magnesium sulfite above the solubility limits of magnesium sulfite in the solution may precipitate or co-p.recipitate during the reaction of orwith q o)r sulfite or bisulfite.

[0823] Note: In some embodiments, residual aqueous magnesium sulfite may be present in th In some embodiments, a portion of the residual aqueousmagnesium sulfite may be concentrated and / or separated using, including, but not limited to, one or more, or any combination of the following: heating, or cooling, or reverse osmosis, or membrane based process, or precipitation, or electrodialysis, or forward osmosis, or any combination thereof. For example, the residual aqueous magnesium sulfite may be separated by concentrating the magnesium sulfite using reverse osmosis or nanofiltration, wherein the pore size or properties of the membrane may enable the permeation of at least a portion of the acetic acid and the rejection of at least a portion of magnesium sulfite, and / or cooling the resulting concentrated magnesium sulfite solution to produce at least a portion of a magnesium sulfite precipitate.

[0824] Note: In some embodiments, the use of ascorbic acid may be desirable because ascorbic acid may be non-volatile, or may comprise minimal or no vapor phase, or any combination thereof. which may mean ascorbic acid may substantially remain at an aqueous phase, or ascorbic acid may substantially not evaporate into remaining gases, or any combination thereof In some embodiments, other acids with stronger acid strength than a ‘WA’ or ‘Weak Acid’ and weaker acidity than sulfurous acid, or which form water soluble calcium or magnesium or alkaline earth salts, or which are non- volatile or have a lower vapor pressure or higher boiling point than water, or any combination thereof may be employed instead of, or in addition to, ascorbic acid.

[0825] (3)

[0826] Note: "(3)' may comprise calcining which may employ a kiln.

[6827] Note: CaSO3(s) may be dried, or dehydrated, or both before or during '(S)’.

[0828] Example 47: Sodium Hydroxide Production from Sodium Sulfate withCalcium Precipitation and Add Intermediate

[0829] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••

[0839] Note: Residual solids or undissolved solids, such as silicon dioxide or oilier undtssolved solids, may be separated .from the liquid solution rising a solid-liquid separation.

[0831] (2)

[0832] (3)CH3COOH(aq)

[0833] (4)

[0834] (5)

[0835] Note: In some embodiments, the present reaction may be conducted at an elevated temperature or temperature greater thanor any combination thereof.

[0836]

[9837] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••* •

[0838] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0839]

[0840]

[0841]

[0842] ) ( ) g) (g

[0843] Note: In some embodiments, the present reaction may he conducted at an elevated temperature or temperature greater than oror any combination thereof

[0844] Example 49; Process for Direct Air Capture with Alkali Intermediate

[0845] (I) One or more or any combination of the followin g:

[0846] Note: Ifis produced, it may be desirable for said CO2(g) to be produced at a high partial pressureor purity or to comprise captured

[0847] (2)

[0848] Note: It may be desirable for the ) to be produced at a high partial pressure or to comprise captured

[0849]

[0850] Note may be separated using a solid-liquid separation.

[0851] (4)

[0852] (5)

[0853] (6)

[0854] (7)

[0855] Example 50; Process for Producing Precipitated Calcium Carbonate

[0856] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Add, which may comprise, hicluding, but not limited to, one or more or any combination of the following' ..••

[0857]

[0858] (3)

[0859] (4) One or more or any combination of the following:•••

[0860] Example 51: Sodium Hydroxide Production and Precipitated CalciumCarbonate Production from Sodium Bicarbonate using Calcium Precipitation and Acid Intermediate

[0861] (I) .React Material comprising Calcium, or Magnesium, or Other Alkaline Earth —Weak Acid Anion wi th Acetic Acid

[0862] Note: Residual solids or undissolved solids, such as silicon dioxide or other nndissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0863] Note: CO2(g) may comprise captured CO2.

[0864] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[0865] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[0866] (2)

[0867] Note: l.n some embodiments, may be added directly to or dissolved in

[0866] Note: In some embodiments, NaHCO3(aq or s) may comprise a mineral, or may comprise nahcolite, or any combination thereof.

[0869] Note: In some embodiments, NaHCO3(s) may be dissolved in water or an aqueous solution to form NaHCO3(aq) before mixing with Ca(CH3COO)2(aq).

[0870] Note: The CO2(g) may comprise captured CO2(g).

[0871] Note: Some embodiments may form dissolved calcium bicarbonate. In some embodiments, dissolved calcium bicarbonate may be decomposed into calcium carbonate and carbon dioxide may heating solution, or depressurizing the solution, or any combination thereof.

[0872] Note: may comprise precipitated calcium carbonate.

[0873] Note:may be separated by solid-liquid separation.

[0874] (3)( q

[0875] Note: In some embodiments, SO2( mg)ay comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2) may result in at least a portion of acetic acid vapor in tire remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reactingwithIn some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[0876]

[0877] Notemay be more soluble in water than . In someembodimentsmay be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0878] Note: in some embodiments,and / or water may be separated from by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments,may evaporate with water vapor and / orcondense with water vapor, which may -result in a disci hate or condensate comprising CH3COOH(aq).

[0879] Note; In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize befor r In some embodiments magnesium sulfitesolid may be separated during step ‘(4)2 In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof. s

[9880] Notemay be separated from by a, solid-liquidseparation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof,

[0881] (5)

[0882] Note: q m) ay comprise a solid-liquid suspension, such as milk oflime.

[0883] Notemay be separated using a solid-liquid separation,

[0884] (6)

[0885] Note: ‘(6)' may comprise calcining , which may employ a kiln,

[0886] Note may be dried, or dehydrated, or both before or during ‘(6)2

[0887] (7)

[0888] Note: In some embodiment may be employed to remove water vapor or facilitated drying of before or during decomposition of to CaO(s).

[9889] Note: In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide. In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide, which may comprise combining step "(5)’ and step ‘(7)’.

[0890] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-liquid suspension, or milk of lime, or solid, or any combination thereof comprising calcium hydroxide.

[0891] (8)Water

[0892] Note: In some embodiments, may be concentrated into an aqueoussolution comprising a greater mass percent concentration of NaOH.

[0893] Note: In some embodiments, water may be removed and / or NaOH may be separated or precipitated by, for example, including,, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0894] Note: In some embodiments, it may be desirable for NaOH to comprise a concentrated aqueous solution

[0895] Example 52; Sodium Hydroxide Production and Precipitated Calcium Carbonate Production from Sodium Carbonate using Calcium Precipitation and Arid Intermediate

[0897] (I) React. Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••

[0897] Note: Residual solids or imdissol ved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a sol id- liquid separation.

[0898] Note: CO2(g) may comprise captured CO2.

[0899] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example., input chemicals or input material may comprise a mixture of calcium and magnesium.

[0900] Note: la some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[0901] (2)

[0902] Note: In some embodiments, Na2CO3laq or s) may be added directly to or dissolved in

[0903] Note: in some embodiments,may comprise a mineral, or may comprise decomposed nahcolite, or any combination thereof

[0904] Note: In some embodiments may be dissolved in water or anaqueous solution to form NaHCOftaq) before mixing with

[0905] Note: Some embodiments may form dissolved calcium bicarbonate. In some embodiments, dissolved calcium bicarbonate may be decomposed into calcium carbonate and carbon dioxide may heating solution, or depressurizing the solution, or any combination thereof,

[0906] Note:

[0907] Note:

[0908] (3)

[0909] Note: In some embodiments, SO2.(g) may comprise other gases in addition to SO2(g> In some embodiments, the reaction of 2 mSOay2( rge)sult in atleast a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, entering the present step may be pre-contacted with ormay absor b at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor inbefore or while reactingwitn some embodiments, acetic acid vapor may be removed from remaining gases using, for example, i ncl uding, but not l imited to, one or more or any combination of the follow ing: alkaline earth carbonate, or alkaline earth. ~ weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[9910] (4)

[0911] Note may be more soluble in waler than Na2SO3. In some embodiments may be separated or precipitated from solution by, for example,including, but not limited to, e vaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof'

[0912] Note: In some embodimenand / or water may be separated from by, for example, evaporation, or distillation, or crystallization, or any combinationthereof. In some embodiments, may evaporate with wafer vapor and / or condense with water vapor, which may result in a distillate or condensate comprising

[0913] Note: In some embodiments, magnesium sulfite(aq) may be present in the In some embodiments, if present, magnesium sulfite may begin to precipitate or crystafize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step '(4)’, In some embodiments, separated magnesium sulfite may be decomposed io magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereofis

[0914] Note: Na2SO3(s) may be separated from by a solid-liquidseparation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the ait, or any combination thereof,

[0915] (5)

[0916] Note: q m) ay comprise a solid-liquid suspension, such as milk oflime.

[0917] Note: CaSO3(s) may be separated using a solid-liquid separation.

[0918] (6)09I9| Note: '(6)' may comprise calciningwhich may employ a kiln.

[0920] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘(6)’.

[0921] (7))0922) Note: In some embodiments, CaO(s) may be employed to remove water vapor or facilitated drying of CaSO3(s) before or during decomposition of CaSO3(s) to

[0923] Note: In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium suifite to produce calcium sulfite and sodium hydroxide. In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide, which may comprise combining step "(5)' and step ‘(7)'.

[0924] Note: In some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-liquid suspension, or milk of Lime, or solid, or any combination thereof comprising calcium hydroxide.

[0925] (8)2 NaOH(aq or s) > 2 NaOH(aq or s) Water

[0926] Note: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution comprising a greater mass percent concentration of NaOH.

[0927] Note: in some embodiments, water may be removed and / or NaOH may be separated or precipitated by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0928] Note: In some embodiments, it may be desirable for NaOH to comprise a concentrated aqueous solution

[0929]

[0930] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid••••

[0931] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolvcd solids, may be separated from the liquid solution using a solid-liquid separation.

[0932] Note: CO2(g) may comprise captured CO3.

[0933] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesi um.

[0934] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[0935] Note: In some embodiments, acetic acid for step ‘(1)’ may comprise aqueous acetic acid produced or regenerated in step ‘(4)’.

[0936] (2) Ca(CH3COO)2(aq)+ Na2SO4(s or aq) -> 2Na(CH3COO)(aq)+ CaSO4(s)

[0937] Note: In some embodiments, Na2SO4(s) may be added directly to or dissolved in Ca(CH3COO)2(aq).

[0938] Note: In some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form Na2SO4(aq)before mixing with Ca(CH3COO)2(aq).

[0939] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. In some embodiments, water may be added to the process by Na2SO4being in the form of Na2SO4(aq) or an aqueous solution comprising sodium sulfate, wherein at least a portion of the water in Na2SO4(aq) may comprise water added to the process. In some embodiments, Na2SO4(aq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SO4(aq) may be provided to the process in the form of Na2SO4(aq.)In some embodiments, Na2SO4(aq) may be provided or sourced as a solid or Na2SO4(s), then dissolved in water to form Na2SO4(aq).

[0940] Note: In some embodiments, Ca(CH3COO)2(aq) may comprise Ca(CH3COO)2(aq)from step ‘(1)’,

[0941] (3) 2 Na(CH3COO)(aq)+ SO2(g or aq) + H2O(1 or aq) → Na2SO3(aq) + 2CH3COOH(aq)

[0942] Note: In some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2Na(CH3COO)(aq)+ SO2(g) may result in at least a portion of acetic add vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or white reactingNa(CH3COO)(aq)with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth.

[0943] Note: In some embodiments, NaCH3COO(aq) may comprise NaCH3COO(aq) from step ‘(2)’.

[9944] Note: In some embodiments, SO2: may comprise SO;:(g) from the calcination or decomposition of CaSCh(s) in step ‘(9)’,

[0945] (4) Na2SO3(aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq) + Na2SO3(s)

[0946] Note: CH3COOH may be more soluble in water than NaiSO3. In some embodiments, Na2SO3may be separated or precipitated from solution by, for example, including, but not limited IO, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[0947] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof In some embodiments, CH3COOH may evaporate with water vapor and / or condense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[0948] Note: In same embodiments, magnesium sulfite(aq) may be present in the Na2:SO3(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystallize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step ‘(4)' . In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof s

[0949] Note: NaiSO3(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[0950] (5) React an Alkaline-Earth -• Weak Acid, such as an Alkaline-Earth Carbonate, with Carbon Dioxide and / or Water to Form an Alkaline-Earth Bicarbonate• CaCO3(s) + CO2(g or aq) + H2O(aq) → Ca(HCO3)2(aq)• MgCO3(s) + CO2(g or aq)+ H2O(aq) → Mg(HCO3)2(aq)

[0951] Note: May be conducted under a pressurized CO2atmosphere or with concentrated carbonic acid or CO2(aq), For example, the CO2partial pressure during thereaction may be greater than, for example, I Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or any combination thereof.

[9952] Note; In some embodiments, CaCO2(s) or MgCO3(s) may comprise CaCO3(s) or MgCO3(s) from step '(10)'.

[0953] Note: In some embodiments, CO2(g or aq) may comprise CO2from step ‘(1 )\ or step '(•'O’: or any combination thereof.

[0954] (6) React an Alkali Sulfite with an Alkaline-Earth Bicarbonate to form an AlkaliBicarbonate and an Alkaline-Earth Sulfite• Na2SO3(s or aq +) Ca(HCO3)2(aq) → 2 NaHCO3(aq) +CaSO3(s)* Na2SO3(s (s or aq +) Mg(HCO3)2(aq) → 2 NaHCO3(aq) + MgSO3 (s)

[9955] Note: In some embodiments, Na2SOXs) may be dissol ved in water or may comprise an aqueous solution before mixing with an aqueous solution comprising Ca(HCO3)2(aq) or Mg(HCO3)2(aq).

[0956] Note: At least a portion ofCaSO3(s) or MgSO3(s) .may be separated by a solid- liquid separation.

[0957] Note: in some embodiments, NaHCO3may be sold as a product or employed as a carbon sequestration medium.

[0958] Note: In same embodiments, Na2SO3(s or aq) may comprise Na2SO3from step ( 4 ) .

[0959] Note: In some embodiments, Cai'HCO3h(aq) or Mg(HCO2)?(aq) may comprise Ca(HCO3)2(aq) or Mg(HCO3)2(aq) from step ‘(5)’.

[0960] (7) 2 NaHCO3(aq) → 2 NaHCO3(s) + Water

[0961] Note: In some embodiments, NaHCO3may be sold as a product and. / or employed as a carbon sequestration medium,

[0962] Note: In some embodiments, step ‘(7)’ may be combined with step ‘(8)’-

[0963] Note: In some embodiments, 2 NaliCO3iaq) may be decomposed into NasCO3(aq) and CO2(g) and water within an aqueous and / or under-pressure or pressurized environment, which may avoid or prevent the need for crystallizing or precipitating NaHCO3(s).

[0964] Note: In some embodiments, 2 NaHCO3(aq) may comprise NaHCO3(aq) from step ‘(6)f

[0965] Note: In some embodiments, at least a portion of residual dissolved MgSO2. or magnesium sulfite, if any, may be separated or precipitated during this step.

[0966] Note: Water may be separated from sodium bicarbonate or sodium carbonate using systems and methods for water separation described herein.

[0967] Note: in some embodiments, step 8 and step 9 may be combined in a single step, wherein, for example, sodium bicarbonate at an aqueous phase may be decomposed into aqueous sodium carbonate and carbon dioxide, which may comprise captured carbon dioxide.• In some embodiments, said aqueous sodium carbonate may be reacted with calcium oxide, or calcium hydroxide, or magnesium oxide, or magnesium hydroxide, or airy combination thereof to produce sodium hydroxide and calcium carbonate or magnesium carbonate.• In some embodiments, said aqueous sodium carbonate may be separated from water to produce solid sodium carbonate and / or said solid sodium carbonate may be dissolved in water and Z or said sodium carbonate may be reacted with calcium oxide, or calcium hydroxide, or magnesium oxide, or magnesium hydroxide, or any combination thereof to produce sodium hydroxide and calcium carbonate or magnesium carbonate.

[0968] (8) 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g or 1)

[0969] Note: CO2(g ) may comprise captured CO2.

[0970] Note: In some embodiments, Na2.CO2may be sold as a product and / or employed as a carbon sequestration medium.

[0971] Note: In some embodiments, step ‘(7)’ may be combined with steps(8)'.

[0972] Note: In some embodiments, 2 NaHCO2(aq) may be decomposed into Na2CO3(aq) and CO2(g) and water within an aqueous and Z or under-pressure or pressurized environment, which may avoid or prevent the need for crystallizing or precipitating NaHCO3(s).

[0973] Note: In some embodiments, 2 NaHCO2(s) may comprise NaHCO3from step ‘(6)' or step ‘(7)’,

[0974] (9) Calcine or decompose an alkaline-earth sulfite to an alkaline earth oxide and sulfur dioxide• CaSO3(s) → CaO(s) + SO2(g)• MgSO3(s) → MgO(s) + SO2(g)

[0975] Note: May comprise calcining CaSO3(s) or MgSO2(s), which may employ a kiln.

[0976] Note: CaSO3(s) or MgSO3(s) may be dried, or dehydrated, or both before or during calcining.

[0977] Note: CaSO3(s) or MgSO3(s) may comprise CaSO3(s) or MgSO3(s) from step ‘(6)’.

[0978] (10) React an alkaline-earth oxide or hydroxide with an alkali carbonate io produce an alkaline-earth carbonate and an alkali hydroxide• CaOls or aq) + NarCO3(s or aq) + Water 2 NaOH(aq) + CaCO3(s)» MgO(s or aq +) Na2CO3(s or aq) + Water → 2 NaOH(aq) + MgCOfrs)

[0979] Note: In some embodiments, CaO + Na2CO3(s or aq) + Water or MgO +Na2CO3(s or aq) + Water may be conducted in multiple steps. For example, in some embodiments, CaO or MgO may be reacted with water to form Cat OHMaq), or Ca(OH)3(s or aq), or Mg(OH)2(aq), or Mg(OH)2(s or aq), which may comprise Milk of Lime or Milk of Magnesia, or a solid-liquid suspension comprising calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na2CO3may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, a solution or solid-liquid mixture or suspension comprising Ca(OH)2(s or aq), or Milk of Lime, or Mg(OH)r, or Milk of Magnesia may be mixed with an aqueous solution comprising Na2CO3iaq), which may result in the formation of a solution comprising aqueous sodium hydroxide and a solid comprising calcium carbonate or magnesium carbonate.

[0980] Note: In some embodiments, at least a portion, of calcium carbonate or magnesium carbonate may be separated from at least a portion of sodium hydroxide using, .for example, a solid-liquid separation.

[0981] Note: CaO(s) or MgO(s) may comprise CaO(s) or MgO(s) from step ‘(9)’.

[0982] Note: Na2CO3(s (1 or aq m) ay comprise Na2CO3(s or aq) from step ‘ (7)’ or step '(8)'.

[0983] Note: In some embodiments, CaCO3or MgCO3may be transferred to step 5,

[0984] Example 54: Process for Producing Sodium Hydroxide with Sulfur Dioxide and Carbon Dioxide Intermediates

[0985] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion With Acetic Acid» CaCO3(s or aq) 2 CH3COOH(aq) → Ca(CH3COO)2(aq)+CO2(g)+H2O(aqorI)• Calcium Silicate(s) + 2 CH3COOH(raq) → Ca( CH3COO)2(aq) + Silicon Dioxide(s) + H2O(aq or I)• CaS(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + H2S(g)• CalciumfWeak Acid Anion) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq) + H2O(aq or I)

[9986] Note: Residual sol ids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[0987] Note: COdg) may comprise captured CO3.

[0988] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[0989] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[0990] Note: In some embodiment acetic acid for step b l)' may comprise aqueous acetic acid produced or regenerated in step ‘(4)’.

[9991] (2) Ca(CHbCOO)2(aq) + NaiSCfos (1 or aq) 2 NaCH3COO(aq) + CaSO3(s)

[0992] Note: In some embodiments, Na2SO3(s) may be added directly to or dissolved in Ca(CH3COO)2( aq) .

[0993] Note: In some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form. Na2SO4(aq) before mixing with Ca(CH3COO)a(aq),

[0994] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. .In some embodiments, water may be added to the process by Na2SO4being in the form of Na2SO4(aq) or an aqueous solutioncomprising sodium sulfate, wherein at least a portion of the water in Na2SO4(aq) may comprise water added to the process. Ill some embodiments, Na2SO4(aq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SO4(aq) may be provided to the process in the form of Na2SO4(aq) . In some embodiments, Na2SO4(aq) may be provided or sourced as a solid or Na2SO4( s), then dissolved in water to form Na2SO4(aq) .

[0995] Note: In some embodiments, Ca(CH3COO)2(aq) may comprise Ca(CH3COO)2(aq) from step ‘(1)’.

[0996] (3) 2 NaCH3COO(aq) + SO2(g or aq) +H2O (1 or aq) -> Na2SO3(aq) + 2CH3COOH(aq)

[0997] Note: In some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2 NaCFbCOO(aq) + SOc(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth,

[0998] Note: In some embodiments, NaCH3COO(aq) may comprise NaClfoCOO(aq) from step '(2)' .

[0999] Note: In some embodiments, SO2may comprise SO2(g) from the calcination or decomposition of CaSO3(s) in step ‘(9)’,

[1000] (4) Na2SO3(aq) + 2 CH3COOH(aq) 2 CH3COOH(aq) + Na2SO3(s)

[1001] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, Na2SO3may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1002] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments, CH3COOH may evaporate with, water vapor and / or condense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[1003] Note: In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) A 2 CH3COOHfaq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step ‘(4)’. In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereofis

[1004] Note: Na2SO2(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1005] (5) React an Alkaline-Earth - Weak Acid, such as an Alkaline-Earth Carbonate, with Carbon Dioxide and / or Water to Form an Alkaline-Earth Bicarbonate• CaCO3(s) + CO2(g or aq) + H2O(aq) → Ca(HCO33)2(aq)• MgCO3(s) + CO2(g or aq) + H2O(aq)) → Mg(HCO3)2(aq)

[1006] Note: May be conducted tinder a pressurized CO2atmosphere or with concentrated carbonic acid or CO3(aq.). For example, the CO3partial pressure during the reaction may be greater (ban, tor example, 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or any combination thereof

[1007] Note: In some embodiments, CaCO3(s) or MgCO2(s) '(1)'may comprise CaCO3(s) or MgCO3(s) from step ‘(9)’ .

[1008] Note: In some embodiments, CO2(g (1 or aq m) ay comprise CO2from step ‘(.I)’, or step or any combination thereof.

[1009] (6) React an Alkali Sulfite with an Alkaline-Earth Bicarbonate to form an AlkaliBicarbonate and an Alkaline-Earth Sulfite• NaSO3(s or aq) + Ca(HCO3)2(aq) → 2 NaHCO3(aq) A CaSORs)* NaSO3(s or aq) + Mg(HCO3)2(aq) + 2 NaHCO3(aq) + MgSO3(s)

[1010] Note: In some embodiments, NaSO3(s) may be dissolved in water or may comprise an aqueous solation before mixing with an aqueous solution comprising Ca(HCO3)2(aq) or Mg(HCO3)2(aq),

[1011] Note: At least a portion of CaSO3(s) or MgSO3(s) may be separated by a solid- liquid separation,

[1012] Note: In some embodiments, NaHCO3may be sold as a product or employed as a carbon sequestration medium.

[1013] Note: In some embodiments, .Na2SO3(s or aq) may comprise Na2SO3from step "(4)"

[1014] Note: In some embodiments, Ca(HCO3)2(aq) or Mg(HCO3)2(aq) may comprise Ca(HCO3 )2(aq) or Mg(HCO3)2(aq) from step "(5)".

[1015] (7) 2 NaHCO3(aq or s) → Na2CO3(aq or s) •+ CO3ig) + HsOlg or I)

[1016] Note: CO2(g) may comprise captured CO2.

[1017] Note: In some embodiments, NarCO3may be sold as a product and / or employed as a carbon sequestration medium.

[1018] Note: In some embodiments, NaHCO3may be precipitated or separated as 2 NaHCO2(s) and / or 2 NaHCO3(s) may be decomposed into Na2CO3(s) CO2. and H2O(g or 1).

[1019] Note: In some embodiments, NazCO2(s) may be dissolved in water before, for example, the reaction with calcium hydroxide or 'magnesium hydroxide in, for example, step 8.

[1020] Note: In some embodiments, 2 NaHCO3( aq) may be decomposed into NazCO3Caq) and CO2(g) and water within an aqueous and / or under-pressure or pressurised environment, which may avoid or prevent, the need for crystallizing or precipitating NaHCO3(s) and Z or to minimize or reduce water evaporation during, for example, CO2desorption.

[1021] Note: In some embodiments, 2 NaHCO3( aq) may comprise NaHCO3from step"(6)"

[1022] (8) Calcine or decompose an alkaline-earth sulfite to an alkaline earth oxide and sulfur dioxide• CaSO3(s) → CaO(s) + SO2(g)• MgSO3(s) → MgO(s) + SO2(g)

[1023] Note: May comprise calcining CaSO3(s) or MgSO2(s), which may employ a kiln.

[1024] Note: CaSGs(s) or MgSOMs) may be dried, or dehydrated, or both before or during calcining.

[1025] Note: CaSO3(s) or MgSOa(s) may comprise CaSO3(s) or MgSO3(s) from step

[1026] (9) React an alkaline-earth oxide or hydroxide with an alkali carbonate to produce an alkaline-earth carbonate and an alkali hydroxide• CaO(s or aq) + Na2CO3(s or aq) + Water 2 NaOH(aq) + CaCO3(s)» MgO(s or aq +) Na2CO3(s or aq) + Water → 2. NaOH(aq) + MgCO3(s)

[1027] Note: In some embodiments, CaO + Na2CO3fs or aq) + Water or MgO + Na2CO3( s or aq) + Water may be conducted in multiple steps. For example, in some embodiments, CaO or MgO may be reacted with water to form Ca(OH)2(aq), or Ca(OH)2(s or aq), or Mg(OH)2(aq), or Mg(OH)2(s or aq), which may comprise Milk of Lime or Milk of Magnesia, or a solid-liquid suspension comprising calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na2CO3may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, a solution or solid-liquid mixture or suspension comprising Ca(OH).'(s or aq), or Milk of Lime, or Mg(OH)s, or Milk of Magnesia may be mixed with an aqueous solution comprising Na2COdaq), which may result in the formation of a solution comprising aqueous sodium hydroxide and a solid comprising calcium carbonate or magnesium carbonate.

[1028] Note: In some embodiments, at least a portion, of calcium carbonate or magnesium carbonate may be separated from at least a portion of sodium hydroxide using, for example, a solid-liquid separation.

[1029] Note: CaO(s) or MgO(s) may comprise CaO(s) or MgO(s) from step ‘(8)’.

[1030] Note: Na2CO2(aq) may comprise Na2CO3(aq) from step ‘(6)’ or step ‘ (7)'.

[1031] Note: In some embodiments, CaCO3or MgCO3may be transferred to step 5.

[1032] Note: In some embodiments, NaOH(aq) may be concentrated, or at least a portion of water may be removed. Separated or recovered waler may be transferred to or employed as a solvent or input in, for example, step ‘5' In some embodiments, NaOH(aq) may be concentrated to a concentrated solution, or 33wt% solution, or a 5(hvt% solution, or solid NaOH, or any comb ination thereof using one or more or any c ombination of water separation systems and / or methods.

[1033] Example 55: Process for Producing Sodium Bicarbonate and / or Calcium Oxide or Calcium Carbonate

[1034] (I) R eact Material comprising Calcium, or Magnesium, orOther Alka l ine Earth ~Weak Acid Anion with Acetic Add• CaCO3(s) or aq) →2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g) + H3O(aq or I)• Calcium Silicate(s) -r 2 CR3COOH(aq) Ca(CH3COO)2(aq) + Silicon Dioxide(s) + H2O(aq or I)• CaS(s) + 2 CH3OOOH(aq) → Ca(CH3COO)2(aq) + H2S(g)• Calcimn( Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq) + H2O(aq or 1)

[1035] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[1036] Note: O2(g) may comprise captured CO2.

[1037] Note: In some embodiments,O2(g) may be employed internally or employed in other steps. For example, in some embodiments, O2(g) may be employed in step '(5) '

[1038] Note: In some embodiments, CO2(g) may be utilized or sequestered or sold or comprise a product. For example, O2(g) may be utilized or sequestered or sold to a CO2, sequestration site or a CO2EOR application or an external application.

[1039] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[1040] Note: In some embodiments, acetie acid vapor and / or water vapor may be separated or recovered from CO2(g).

[1041] Note: In some embodiments, acetic acid for step '(7)'’ may comprise aqueous acetic acid produced or regenerated in step ‘(4)’.

[1042] (2) Ca(CH3CO)2(aq) + Na2SO4( s or a q)→ 2 NaCH3COO(aq) + CaSO4(s)

[1043] Note: In some embodiments, Na2SO4(s) may be added directly to or dissolved in Ca(CH3COO)2(aq),

[1044] Note: in some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form Na2SO4(aq) before mixing with Ca(CH3COO)2(aq).

[1045] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. In some embodiments, water may be added to the process by NarSOi being in the form of Na2SO^aq) or an aqueous solution comprising sodium sulfate, wherein, at least a portion of the water in Nat SOd' aq j may comprise water added to the process. In some embodiments, NaaSOdaq) may be provided or sourced as an aqueous solution. For example, in some embodiments, NaiSOdaq) may be provided to the process in the form of NacSOd'aq). In some embodiments, NacSOdaq) may be provided or sourced as a solid or NatSCM s), then dissolved in water to form NacSOdaq).

[1046] Note: In some embodiments, Ca(CH3COO)2(aq) may comprise Ca(CH3COO)daq) from step

[1047] (3) 2 NaCH3COO(aq) + SO2(g or aq) + H2O(1 or aq) → Na2SO3(aq) + 2 CH3COOH(aq)

[1048] Note: In some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2 Na(CH3COO (aq )+ SO2(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with ormay absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth.

[1049] Note: In some embodiments, Na(CH3COO (aq) maycomprise Na(CH3COO (aq) from step ‘(2)’.

[1050] Note: In some embodiments, SO2: may comprise SO;:(g) from the calcination or decomposition of CaSO3(s) in step ‘(7)’.

[1051] (4) Na2SO3(aq) ± 2 CH3COOH(aq) → 2 CH3COOH(aq) + Na2SO3(s)

[1052] Note: CH3COOH may be more soluble in water than NaiSO3, In some embodiments, Na2SO3 may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[1053] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof In some embodiments, CH3COOH may evaporate with water vapor and / or condense with water vapor, which may result is a distillate or condensate comprising ClhCOOH(aq).

[1054] Note: In same embodiments, magnesium snlfite(aq) may be present in the Na2:SO2(aq) + 2 CH3COOH(aq). In some embodiments. if present, magnesium sulfite may begin io precipitate or crystalize before Na2SO3. hi some enibodimeiits magnesium sulfite solid may be separated during step ‘(4)' . In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium stdfrte, or decomposed together with calcium sulfite, or any combination thereof s

[1055] Note: NaiSO3(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1056] (5) React an Alkaline-Earth .. Weak Acid, such as an Alkaline-Earth Carbonate, with Carbon Dioxide and / or Water to Form an Alkaline-Earth Bicarbonate• CaCO3(s) + CO2(g or aq) + H2O( aq ) → Ca(HCO3)2(aq)• MgCO3(s) + CO2(g or aq) F HsO( aq ) → Mg(HCO3)2(aq)

[1057] Note: May be conducted under a pressurized CO2atmosphere or with concentrated carbonic acid or CO3(aq). For example, the CO2partial pressure during the•reaction may be greater than, for example, I Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or any combination thereof.

[1658] Note; In some embodiments, CaCO2(s) or MgCO3(s) may comprise CaCC3(s) or MgCO3(s) from step '(8)'

[1659] Note; In some embodiments, CaCO3(s) or MgCO3(s) may comprise an input, such as limestone, or dolomite.

[1060] Note: In some embodiments, CO2(g (1 or aq m) ay comprise CO2from step “(1

[1061] Note: In some embodiments, CO3(g or aq) may comprise CO2from an emissions source, or another CO2source, or captured CO2, or any combination thereof. For example, in some embodiments, CO3(g or aq) may comprise, including, but not limited to, one or more or any combination of the following: CO2from a blue hydrogen or blue ammonia facil ity, or an ammonia facility, oran ethanol plant, or a carbon capture plant.

[1062] (6) React, an Alkali Sulfite with an Alkaline-Earth Bicarbonate to form an AlkaliBicarbonate and an Alkaline-Earth Sulfite• Na2SO3(s or aq) + Ca(HCO3)2(aq) → 2 NaHCO3(aq) + CaSO3(s)• Na2SO3(s or aq +) Mg(HCO3)2(aq) → 2 NaHCO3(aq) + MgSO3('s)

[1063] Note: In some embodiments, Na2SOu's) may be dissolved in water or may comprise an aqueous solution befote or during mixing with an aqueous solution comprising Ca(HCO3)2(aq) or Mg(HCO3)2(aq).

[1064] Note: At least a portion ofCaSO3('s) or MgSO3(s) may be separated by a solid- liquid separation.

[1065] Note: In some embodiments, NaHCO3may be sold as a product or employed as a carbon sequestration medium.

[1066] Note: In some embodiments, NaHCO2may be concentrated and / or crystalized into a solid, such as, for example, solid sodium bicarbonate or solid sodium carbonate.

[1067] (7) Decompose an Alkaline-Earth Sulfite into an Alkaline-Earth Oxide and SulfurDioxide• CaSO3(s) → CaO(s) + SO2(g)• MgSO2;(s) → MgO(s) + SO2(g)

[1068] Note: May comprise calcining CaSO3(s) or MgSO3(s), which may employ a kiln.

[1069] Note: CaSO2(.s) or MgSO3(s)may be dried, or dehydrated, or both before or during calcining.

[1070] Note: CaSO3(s) or MgSO2(s) may comprise CaSOh's) or MgSO3(s) from step‘(6)'-

[1071] Note: CaO or MgO may comprise a valuable product if desired. For example, CaO or MgO may comprise an ultra-low carbon emissions CaO or MgO product. In some embodiments, calcium oxide, or calcium hydroxide, or magnesium oxide, or magnesium hydroxide, or any combination thereof may comprise a product or may be sold or may be sold. In some embodiments, calcium oxide, or calcium hydroxide, or magnesium oxide, or magnesium hydroxide, or any combination thereof may comprise a product or may be sold or may be sold from the present example embodiment.

[1072] (8) React an Alkaline-Earth Oxide or Hydroxide with Carbon Dioxide to form anAlkaline Earth Carbonate• CaO(s) + CO2(g) → CaCO3(s)• MgO(s) + CO3(g) → MgCO3(s)• CaO(s) + H2O → Ca(OH)2(s or aq)• MgO(s) + H2O → Mg(OH)Xs (1 or aq)• Ca(OH)2(s (1 or aq v) + CO2(g) CaCO3(s) + HsO• Mg(OH)2(s or aq +) CO2(g) → MgCO2(s) + H2O

[1073] Note: In some embodiments, CaO(s) or MgO(s) may be reacted with water to form Ca(OH)2(aq), or Ca(OH)2(s or aq), or Mg(OH)2(aq), or Mg(OH)2('s or aq), or any combination thereof which may comprise Milk of Lime, or Milk of Magnesia, or a solid- liquid suspension comprising calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH)2or Mg(OH)2may be reacted with a carbonate salt, such as sodium carbonate or sodium bicarbonate, to form CaCO2or MgCOy or may be reacted with CO2to form CaCO3or MgCO3. For example, said sodium carbonate or sodium bicarbonate may comprise sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassium bicarbonate, or alkali carbonate, or alkali bicarbonate, or any combination thereof employed in or as a CO2absorption solution.

[1074] Note: In some embodiments, CO2(g) may comprise CO2in or from a point source CO2emissions source. For example, CO2(g) may comprise flue gas, or dilute CO2, or high purity CO2, or captured. CO2.

[1075] Note: In some embodiments, CO2(g) may comprise CO2in or from air. For example, CO2(g) may comprise air which may comprise at least a portion of CO2even if at a very dilute concentration. For example, calcium oxide may be capable of reacting with very low concentrations or very dilute concentrations of CO2if desired. For example, CO2(g) may Comprise a carbonate salt, such as sodium carbonate or potassium carbonate, wherein the carbonate may comprise carbonate originating from the reaction of carbon dioxide in the air with a sodium or potassium or other alkali salt, such as sodium hydroxide or potassium hydroxide, forming foe alkali carbonate salt, and / or wherein the reaction of calcium oxide or calcium, hydroxide with foe alkali carbonate may result in the regeneration or fonnation of an alkali hydroxide or alkali oxide or other alkali salt which may be employed to absorb carbon dioxide from the air a regenerate or re-form foe alkali carbonate salt.

[1076] Note: In some embodiments, CaCO3or MgCO3may comprise a valuable product, in some embodiments, CaCO3or MgCO3may comprise precipitated calcium carbonate. In some embodiments, CaCCh or MgCO3may comprise a carbon sequestration medium.

[1077] Note: In some embodiments, for example, including, but not limited, to. Example 53, or Example 54, or Example 55, or Example 61, or Example 62, or any combination thereof may comprise processes operating separately and / or simul taneously. For example, in some embodiments, CO: produced in step ‘(1 )' of Example 53 or Example 54 may comprise an input to Example 55,

[1078] Example 56: Process for Producing Calcium Carbonate from CafWA) usingAmmonium Chlorid[

[1079] ( 1 ) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth Weak Acid. Anion with Ammonium Chloride• Ca(WA)(s) + 2 NH4CI(s or g or aq) → CaCl2(s or aq) + 2 NH3g or aq) + H2O(g or aq)

[1080] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid phase or at a solid-gas mixture phase. For example, 2 NH4CI(s) and Ca(WA)(s) may be heated, which may result in the vaporization. of NH4CI into NH3(g)and HCl(g), wherein the HCI(g) may react with the Ca(WA)(s) to form, for example, CaCl2(s) and / or ( WA) and / or water.

[1081] Note: In some embodiments, WA may comprise, for example, including, but not limited to, one or more or any combination of die following; a silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide.

[1082] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid-liquid phase or a solid-aqueous phase. For example, 2 NH4Cl(aq) and Ca(WAXs) may be mixed, and / or may react to form, for example, CaCl2(aq) and 2 NH3(aq or g).

[1083] (2) CaCl2(s) + Water → CaCl2(aq)

[1084] Note: In some embodiments, CaCl2from step 1 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[1085] (3) Ammonia or weak base may be dissolved in water or aqueous solution to form aqueous ammonia, and / or ammonia may be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate.• CaCl2(aq) + 2 NH3(g) CaCl^aq) + 2 NH3((gaq) )• 2 NH3(g) + Water NH3((gaq))• 2 NH3(g or aq) + CO2(g) + H2O(1 or aq) -> (NH4)2CO3(aq)• 2 NH3(g or aq) - 2 CO2(g) + 2 H2O(1 or aq) → 2 NH4HCO3(aq)• (NH4)2CO3(aq) + CO2(g) + H2O(I or aq) → 2 NH4HCO3(aq)

[1086] Note: In some embodiments, NH3( fgr)om step 1 may comprise a gas and / or may be dissolved in CaCl2(aq).

[1087] Note: In some embodiments, NH3may be dissolved in water and / or reacted widi CO2separately from CaCl2.

[1088] (4) Calcium chloride may be reacted with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate.• CaCl2(aq) + 2 NH3((gaq)) + CO2(g) + H2O 2 NH»Cl(aq) + CaCO3(s)• CaCl2(aq) + 2 NH3(aq) + 2 CO2(g) + H:O 2 NH4CI(aq) + CaCO3(s) + CO2(g)• CaCl2(aq) + ( NH4)2CO3(aq) 2 NH4CI(aq) + CaCO3(s)♦ CaCT:(aq) + 2 NH4HCO3(aq) → 2 NH4CI(aq) + CaCO3(s) + CO2(g)

[1089] Note: In some embodiments, if excess CO2is present or CO: is in die product, in some embodiments, said excess CO2may be transferred to die inputs or reactants of step 4 and / or die inputs or reactants of step 3.

[1090] Note: In some embodiments, a CaCI2(aq) + NH3(aq) solution may be produced in step 1 and / or may be transferred to step 4, potentially skipping step 2 and step 3.

[1091] Note: In some embodiments, CO2(g) may comprise captured CO: from another embodiment described herein. For example, in some embodiments, CO:(g) may comprise CO: from the reaction of calcium carbonate with acetic acid.

[1092] Note: In some embodiments, CaCO3(s) may be transferred to or may comprise an input to one or more or any combination of embodiments described herein. For example, CaCCb(s) may be an input to a process for producing sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[1093] Note: In some embodiments, CO:(g) may comprise CO2from an emissions source, or a point source, or air, or from an external source, or any combination thereof.

[1094] ]ote: In some embodiments, 2 NH4XI(aq) may be transferred to step I .

[1095] Note: In some embodiments, 2 NH4Cl(aq) may be transferred to step 5.

[1096] (5) 2 NH4Cl(aq) 2 NH4Cl(s) + Water

[1097] Note: In some embodiments, 2 NH4Cl(s) may be transferred to step 1 [

[1098] Note: In some embodiments, Water may be transferred to step 3 and / or step 4.

[1099] Note: In some embodiments, the present example embodiment may be integrated with other embodiments described herein to further increase the CO2conversion or CO: removal potential, or enable the production of chemicals without requiring a CO: output exiting the process, or to enable the use of other Ca(WA) inputs or less reactive Ca(WA) inputs, or any combination thereof.• For example, in some embodiments, CaCO2may be transferred from the present embodiment to a second embodiment, then the captured CO: from the second embodiment may be transferred to the present embodiment. For example, in some embodiments, the CO2transferred between the present embodiment and the second embodiment may comprise an intermediate in the production of a chemical, such as.for example, including, but not limited to, one or more or any combination of the following: sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.• For example, in some embodiments, CO2in the production of CaCO3 may be from an emissions source or air, and / or the produced CaCO? may be transferred from the present embodiment to a second embodiment, such as an embodiment for producing sodium carbonate or sodium bicarbonate, which may increase the net CO: conversion or CO2removal potential of said second embodiment.

[1100] Example 57; Process for Producing Alkali Hydroxide with Carbon Dioxide

[1101] (I) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth - Weak Acid Anion with Ammonium Chloride• Ca(WA)(s) + 2 NH4Cl(s) or g or aq) CaCl2(s or aq) + 2 NFb(g or aq) + H2O(g or aq)

[1102] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid phase or at a solid-gas mixture phase. For example, 2 NHtCl(s) and Ca( WAXs) may be heated, which may result in the vaporization of NH4Cl into NH3(g) and HCl(g), wherein the HCl(g) may react with the Ca(WA)(s) to form, for example. CaCl2(s) and / or (WA) and / or water.

[1103] Note: In some embodiments, WA may comprise, for example, including, but not limited to, one or more or any combination of die following; a silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide.

[1104] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid-liquid phase or a solid-aqueous phase. For example, 2 NH4CI(aq) and Ca(WAXs) may be mixed, and / or may react to form, for example, CaCl2(aq) and 2 NH3(aq or g).

[1105] (2) CaCl2(s) + Water CaCl2(aq)

[1106] Note: In some embodiments, CaCl2from step 1 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[1107] (3) Ammonia or weak base may be dissolved in water or aqueous solution to form aqueous ammonia, and / or ammonia may be dissolved in water and / or reacted with carbon dioxide co form ammonium carbonate or ammonium bicarbonate.• CaCI2(aq) + 2 NH3(g) → CaCI2(aq) + 2 NH3(aq)• 2 NH3(g) + Water → NH3(aq)• 2 NH3((g) or aq) + CO2(g) + H2O(l or aq) → ( NH4HCO3(aq)• 2NH3(g or aq) + 2 CO2(g) + 2 H2O(l or aq) → 2 NH4HCO3(aq)• (NH4)2CO3(aq) + CO2(g) + H2O(l or aq) → (NH4)2CO3(aq)

[1108] Note: In some embodiments, NH< from step 1 may comprise a gas and / or may be dissolved in CaCI2(aq).|1109] Note: In some embodiments, NH3may be dissolved in water and / or reacted with CO2separately from CaCl2.

[1110] (4) Calcium chloride may be reacted with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate.• CaCI2(aq) + 2 NH3(aq) + CO2(g) + H2O→ 2 NH4CI(aq) +CO3(s)• CaCl2(aq) + 2 NH3(aq) + 2 CO2(g) + H2O→ 2 NH4CI(aq) + CaCO3(s) + CO2(g)• CaCI2(aq) + ( NH4)2CO3(aq) → 2 NH4CI(aq) + CaCO3(s)• CaCI2(aq) + 2 NH4H CO3(aq) 2 NH4Cl(aq) + CaCO3(s) + CO2(g)

[1111] Note: In some embodiments, if excess CO: is present or CO2is in the product, in some embodiments, said excess CO2may be transferred to the inputs or reactants of step 4 and / or the inputs or reactants of step 3.

[1112] Note: In some embodiments, a CaCI2(aq) + NH3(aq) solution may be produced in step 1 and / or may be transferred to step 4, potentially skipping step 2 and step 3.

[1113] Note: In some embodimentCs,O2(g) ) may comprise captured CO2from another embodiment described herein. For example, in some embodiments, CO2(g) may comprise CO2from the reaction of calcium carbonate with acetic acid.

[1114] Note: In some embodiments, CaCO3(s) may be transferred to or may comprise an input to one or more or any combination of embodiments described herein. For example,CaCO3(s) may be an input to a process for producing sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[1115] Note: In some embodiments, CO2(g) may comprise CO: from an emissions source, or a point source, or air, or from an external source, or any combination thereof.

[1116] Note: In some embodiments, 2 NH4Cl(aq) may be transferred to step 1[

[1117] Note; th sone embodiments, 2 NH4Cl(aq) may be transferred to step 5.

[1118] (5) 2 NH4Cl(aq) 2 NH<Cl(s) + Water

[1119] Note: In some embodiments, 2 NH4CI( s) may be transferred to step 1 .

[1120] Note: tn some embodiments. Water may be transferred to step 3 and / or step 4.

[1121] (6) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth - Weak Acid Anion with Acetic Acid• Ca(Xh(s or aq) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g) + H2O(l or aq)• Calcium Silicate(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + Silicon Dioxide(s) + H2O(l or aq)• CaS(s) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + H2S(g) + H2O(1 or aq)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + Weak Add(s, or g, or I, or aq) + H2O(l or aq)(1122) Note; Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[1123] Note: CO2(g) may comprise captured CO2.

[1124] Note: In some embodiments, CO2may be transferred to step 4.

[1125] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[1126] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).(1127] (7) Ca(CH3COO)2(aq) + Na2SO4(s or aq) → 2 NaCH3COO(aq) + CaSO4(s)

[1128] Note; In sone embodiments, NajSO^s) may be added directly to or dissolved inCa(CH3COO)2(aq).

[1129] Note: In some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form Na2SO4(aq) before mixing with Ca(CH3COO)2(aq).

[1130] Note: In some embodiments, waler may be added to foe process to make up for water which may leave foe process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. In some embodiments, water may be added to foe process by Na2SO4being in the form of Na2SO4(aq) or an aqueous solution comprising sodium sulfate, wherein at least a portion of foe water in Na2SO4(aq) may comprise water added to foe process. In some embodiments, Na2SO4(aq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SO4(aq) may be provided to the process in the form of Na2SO4(aq). In some embodiments, Na2SO4(aq) may be provided or sourced as a solid or Na2SO4^s), then dissolved in water to form Na2SO4(aq).

[1131] (8) 2 NaCH3COO(aq) + SO2(g or aq) + H2O(l or aq) → Na2SO4(aq) + 2 CH3COOH(aq)

[1132] Note: In some embodiments, SO2(g) may comprise other gases in addition toSO2(g). In some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in foe remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering foe present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from foe remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[1133] (9) Na2SO3(aq) + 2 CH3COOH(aq) → 2 CH3COOH(aq) + Na2SO3( s)

[1134] Note: CH3COOH may be more soluble in water than Na2SO4i. In some embodiments, Na2SO4j may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1135] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combinationthereof. In some embodiments, CHsCOOH may evaporate with water vapor and / or condense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[1136] Note: In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step ‘(9)’. In some embodiments, separated magnesium sulfite may be decomposed io magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof.

[1137] Note: Na2SO3(s) may be separated, from CH3COOH(aq) by a solid- liquid separation, which may include , but is not limited to, filter, or centrifuge, or decanter, or separation, systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1138] (10) Na2SO3(s or aq) + Ca(OH)2(s or aq) * 2 NaOH(aq or s) + CaSO3(s)

[1139] Note: Ca(OH)?(s or aq) may comprise a solid-liquid suspension, such as milk of lune.

[1140] Note: CaSO3(s) may be separated using a solid-liquid separation.

[1141] (11) CaSO3(s) → CaO(s) + SO2(g)

[1142] Note: *(1 1)’ may comprise calcining CaSCb(s), which may employ a kiln.

[1143] Note: CaSO3(s) may be dried, or dehydrated, or both before or during ‘(1 1)’-

[1144] (12) CaO(s) + Water( g or I or aq) Ca(OH)2(s or aq)

[1145] Note: In some embodiments, CaO(s) may be employed to remove water vapor or facilitated drying of CaSO3(s) before or during decomposition of CaSO3(s) to CaO(s).

[1146] Nate: In some embodiments, calcium oxide may be reacted directly with an. aqueous solution comprising sodium sulfite to produce calcium sulfite and. sodium hydroxide. In some embodiments, calcium oxide may be reacted directly with an aqueous solution comprising sodium sulfite to produce calcium sulfite and sodium hydroxide, which, may comprise combining step ‘(10)’ and step "(12)'.[.1147] Note: in some embodiments, calcium oxide may be reacted with water to produce an aqueous solution, or solid-l iquid suspension, or milk of lime, or solid, or any combination thereof comprising, calcium hydroxide.

[1148] (13) 2 NaOH(aq or s) → 2 NaOH(aq or s) + Water

[1149] Note: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution comprising a greater mass percent concentration of NaOH.

[1150] Note: in some embodiments, water may be removed and. / or NaOH may be separated or precipitated by, for example, including, but not limited, to, evaporation, or distillation, or -crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[1151] Note: In some embodiments, it may be desirable for NaOH to comprise a concentrated aqueous solution.Example 58: Process for Producing Alkali Hydroxide with Carbon Dioxide,Alkali Carbonate, and / or Sulfur Dioxide Intermediates

[1153] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth - Weak .Acid Anion with Ammonium ChlorideCa(WA)(s) v 2 NH4CI(s or g or aq) CaCL2(s or aq) + 2 NH3(g or aq) + H2O(g or aq)

[1154] Note: in some embodiments, the reaction of Ca( WA) with ammonium chloride may be conducted at a solid phase or at a solid-gas mixture phase. For example, 2 NH4Cl(s) and Ca(WA)(s) may be heated, which may result in the vaporization of NH4CI into NH;«(g) and HCl(g), wherein the HCl(g) may react with the Ca(WA)(s) to form, for example, CaCI2(s) and- / or ( WA) and / or water.

[1155] Note: In some embodiments, WA may comprise, for example, including, but not limited to, one or more or any combination of rhe following; a silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide.

[1156] Note: In some embodiments, the reaction of Cat W A) with ammonium chloride may be conducted at a solid-liquid phase or a solid-aqueous phase. For example, 2 NH4Cl(aq) and Ca( WA)(s) may be mixed, and / or may react to form, for example, CaCh(aq) and 2 NH3(aq or g),

[1157] (2) CaCl2fs) -i- Water→ 4k CaChC.aq)

[1158] Note: In some embodiments, CaCh from step 1 may comprise a solid and. / or may be dissol ved in water to form an aqueous solution.

[1159] (3) Ammonia or weak base may be dissolved in water or aqueous solution to form aqueous ammonia, and / or ammonia may be dissolved in. water and. / or reacted, with carbon dioxide to form ammonium carbonate or ammonium bicarbonate.CaCl2(aq) + 2 NH;=(g) -> CaCl2(aq) + 2 NB(aq)2 NH3(g) + Water NHrfaq)2 Nl'btg or aq) + CO2(g) + H2O(1 or aq) (NH4)2CO.;(aq)2NH?(g or aq) 2 CO2(g) + .2 H3O(l or aq) 2 NHtHCOsfaq) (NH4)?.CO3(aq) + COXg) + HcOfl or aq) ->2 NH4HCOs(aq)

[1160] Note; In some embodiments, ,NFb from step 1 may comprise a gas and / or may be dissolved in CaCl2(aq),

[1161] Note: In some embodiments, NHr may be dissol ved in water and / or reacted, with CO2separately from CaCh.

[1162] (4) Calcium chloride may be reacted, with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate.CaCl2(aq) + 2 NH3(aq) + CO2(g) + HsO → 2 NH4Cl(aq) + CaCO3(s)CaCl2(aq) * 2 NH3(aq) + 2. CChfg) + H2O 2 NH4Cl(aq) -r CaCO3(s) + CO2(Mg)CaCl2(aq) + (NH4)2CO3(aq)→ 2 NH4Cl(aq) + CaCOa(s)CaCl2(aq) + 2 NH4H CO3(aq)→ 2. NH4Cl(aq) + CaCOqs) + CO2(g)

[1163] Note: In some embodiments, if excess CQ?. is present or CO2is in the product, in some embodiments, said excess CO2may be transferred to (he inputs or reactants of step 4 and / or the inputs or reactants of step 3.[.1164] Note: hi some embodiments, a CaCl2(aq) +• NHs(aq) solution may be produced in step 1 and / or may be transferred, to step 4, potentially skipping step 2 and step 3.

[1165] Note: In some embodiments, CO2(g) may comprise captured CO2frOm another embodiment described herein. For example, in some embodiments, CO2.(g) may comprise CO2from the reaction of calcium, carbonate with acetic acid.

[1166] Note: In some embodiments, CaCO3(s) may be transferred to or may comprise an input to one or more or any combination of embodiments described herein. For example, CaCO3(s) may be an input to a process for producing sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[1167] ]ote: In some embodiments, CO2(g) may comprise CO2from an emissions source, or a point source, or air, or from an external source, or any combination thereof.

[1168] Note: In some embodiments, 2 NH4Cl(aq) may be transferred to step L

[1169] Note: In some embodiments, 2 NH4Cl(aq) may be transferred to step 5.

[1170] (5) 2 NH»Ci(aq) 2 NH4Cl(s) Water

[1171] Note: In some embodiments, 2 NH4Cl(s) may be transferred to step 1 .

[1172] Note: In some embodiments, Water may be transferred to step 3 and / or step 4.

[1173] (6) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid. CaCO3(s or aq)→ 2 CH3COOH(aq)→ Ca(CH3COO)2(aq) + CO:(g) + H2O(aq or I) Calcium Siiicate(s) + 2 CHsCOOHtaq) -> Ca(CH3COO(aq) + Silicon Dioxide(s) + H2O(aq or I). CaS(s) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + H2S(g)Calcium Weak Acid Anion.) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + WeakAcidfs, or g, or 1, or aq) + H2O(aq or 1)

[1174] Note: Residual solids or undissoived solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation-

[1175] Note: CO2(g) may comprise captured CO2.

[1176] Note: In some embodiments, CO2may be transferred to step 4.

[1177] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments. for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[1178] Note: in some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g),

[1179] Note: In some embodiments, acetic acid for step ‘(6)’ may comprise aqueous acetic acid produced- or regenerated in step ‘(9)’.

[1180] (7) Ca(CH3COO)2(aq) + Na2SO4(s or aq)→ 2 NaCH3COC(aq) → CaSO4(s)

[1181] Note: In some embodiments, Na2SO4(s) may be added directly to or dissolved in Ca(CH3COO)2(aq),

[1182] Note: In some embodiments, Na2SO4(s) may be dissolved in water or an aqueous solution to form Na2SO4(aq) before mixing with Ca(CH3COO)2(aq).

[1183] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof In some embodiments, water may be added to the process by Na2SO4being in the form of Na2SO4(aq) or an aqueous solution comprising sodium sulfate, wherein, at least a portion of the water in Na2SO4(aq) may comprise water added to the process. In some embodiments, NazSCkfaq) may be provided or sourced, as an. aqueous solution.. For example, in some embodiments, Na2SO4(aq) may be provided to the process in the form of Na2SO4(aq). In some embodiments, Na2SO4(aq) may be provided or sourced as a solid or Na2SO4(s), then dissolved in water to form Na2SO4(aq).

[1184] Note: In some embodiments, Ca(CH3COO)2(aq) may comprise Ca(CH3COO)2(aq) from step "(6)’.

[1185] (8) 2 NaCHsCOOfaq) + SOi(g or aq) + FbO(l or aq) NazSOafaq) + 2CH3COOH (aq)

[1186] Note: In some embodiments, SO2(g) may comprise other gases in addition toSO2(g). In some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after tire reaction, hr some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or .may absorb at least a portion of acetic acid- vapor from, the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3C(Otaq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from, remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slum', or alkaline earth oxide, or alkaline earth.

[1187] Note: In some embodiments, NaCHrCOOfaq) may comprise NaCH3COO( aq) from step ‘(7)’.

[1188] Note: In some embodiments, SO2: may comprise SO;:(g) from the calcination or decomposition of CaSO3(s) in step ‘( 14)’.

[1189] (9) Na2SO3(aq) + 2 CH3COOH(aq) 2 CH3COOH(aq) + Na2SO3(s)

[1190] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, Na2SO3may be separated or precipitated from solution by, for example, including. but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[1191] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In. some embodiments, CH3COOH may evaporate with, water vapor and / or condense with, water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[1192] Note: In some embodiments, magnesium sulfite(aq) may be present in the Na2SO3(aq) + 2 CH3COOH(aq). In some embodiments. if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO3. In some embodiments magnesium sulfite solid may be separated during step "(9)". In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof.s

[1193] Note: Na2SO3(s) may be separated from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described In the art, or any combination thereof.

[1194] (10) React an Alkaline-Earth - Weak Acid, such as an Alkaline-Earth Carbonate, with Carbon Dioxide and / or Water to Form an Alkaline-Earth BicarbonateCaCO3(s) + CO2('g or aq) + H2O(aq) → Ca(HCO2)2(aq)MgCO3(s)+ CO2(g or aq) + H2O(aq) → Mg(HCO3)2(aq)

[1195] Note: May be conducted under a pressurized CO2atmosphere or with concentrated carbonic acid, or CO2(aq). For example, the CO2partial pressure during thereaction may be greater than, for example, I Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6Bar, or 7 Bar, or S Bar, or 9 Bar, or 10 Bar, or any combination thereof'

[1196] Note; in some embodiments, CaCO-(s) or MgCO2(s) may comprise CaCCh(s) or MgCO3(s) from step '(14)’.

[1197] Nate: In. some embodiments, (Xhfg or aq) may comprise CO2from step ‘ (6)7, or step '( 13)', or atty combination thereof.

[1198] (11) React an Alkali Sulfite with an Alkaline-Earth Bicarbonate to form an Alkali Bicarbonate and an Alkaline-Earth Sulfite Na2SO3or aq) + Ca(HCOs)2(aq) 2 NaHCOs(aq) + CaSO3(s) Na2SO3(s or aq) + .Mg(HCO.02(aq) 2 NaHCOs(aq) + MgSO3(s)

[1199] Note: in some embodiments, Na2SOXs) may be dissolved, in water or may comprise an aqueous solution before mixing with att aqueous solution comprising CH(HCO3)2(aq) or Mg(HCO3)2(aq).

[1200] Note: At least a portion of CaSO3(s) or MgSO3(s) may be separated by a solid- liquid separation.

[1201] Note: in some embodiments, NaHCO3may be sold as a product or employed as a carbon sequestration medium.

[1202] Note: In some embodiments, Na2SO3(s or aq) may comprise Na2SOx from step‘(4)2

[1203] Note: In some embodiments, Ca(HCO3)2(aq) or Mg(HCO2)2(aq) may comprise Ca(HCO3)(aq) or Mg(HCO3)2(aq) from step ‘(5)’.

[1204] (12) 2 NaHCOs(aq) → N^COs(aq) + CO2(g) + H2O(g or I)

[1205] Note: CO->(g) may comprise captured COr,|1206] Note: In some embodiments, Na2CO3may be sold as a product and Z or employed as a carbon sequestration medium.

[1207] Note: in some embodiments, 2 NaHCO3(aq) may be decomposed into Na2CO3(aq) and CO2(g) and water within an aqueous and / or under-pressure or pressurized environment, which may avoid or prevent the need, for crystallizing or precipitatingNaHCO3(s) and / or to minimize or reduce water evaporation during, for example, CO2desorption.[1208J Note: In some embodiments, 2 NaHCO3(aq) may comprise NaHCOs from step( 1 1 ) '.P 209| (13) Calcine or decompose an alkaline-earth sulfite to an alkaline earth oxide and sulfur dioxide• CaSO3(s) → CaO(s) + SO2(g)• MgSO3(s) → MgO(s) + SO2(g)[1210| Note: May comprise calcining CaSO3(s) or. MgSO3(s) which may employ a kiln.[12111 Note: CaSO3(s) or MgSOs(s) may be dried, or dehydrated, or both before or during calcining.[1212$ Note: CaSO3(s) or MgSO.?(s) may comprise CaSO3(s) or MgSO3(s) from stepX I IV.

[1213] (14) React an alkaline-earth oxide or hydroxide with an alkali carbonate to produce an alkaline-earth carbonate and an alkali hydroxide. CaO(s or aq) + Na2CO3(s or aq) → Water NaOH(aq) + CaCO3(s)MgO(s or aq) + Na2CO3(s or aq) → Water NaOH(aq) + MgCO3(s)

[1214] Note: In some embodiments, CaO 1 Na2COs(s or aq) + Water or MgO Na?.CO <s or aq) -t- Water may be conducted in multiple steps. For example, in some embodiments, CaO or MgO may be reacted, with water to form Ca(OH)2(aq), or Ca(OH)2(s or aq), or Mg(OH)2(aq), or Mg(OH)2(s or aq), which may comprise Milk of Lime or Milk of Magnesia, or a solid-liquid suspension comprising calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na2CO3may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, a solution or solid-liquid mixture or suspension comprising Ca(OH)2(s or aq), or Milk of Lime, or Mg(OH)2, or Milk of Magnesia may be mixed with an aqueous solution comprisi ng Na2CO3(aq), which may result in t.be formation of a solution comprising aqueous sodium hydroxide and a solid comprising calcium carbonate or magnesium carbonate.

[1215] Note: In some embodiments, at least a portion of calcium carbonate or magnesium carbonate may be separated from at least a portion of sodium hydroxide using, for example, a solid-liquid separation.

[1216] Note: CaO(s) or MgO(s) may comprise Ca()(s) or MgCXs) from step "(13)'.

[1217] Note; Na2CO2faq) may comprise NazCChfaq) from. step "(I I)' or step "(12)\

[1218] Note: in some embodiments,. CaCOs or MgCCh may be transferred to step 10.

[1219] Note: In some embodiments, NaOH(aq) may be concentrated, or at least a portion of water may be removed. Separated or recovered water may be transferred to or employed, as a solvent or input in, for example, step ‘ HE. In some embodiments, NaOH(aq) may be concentrated to a concentrated solution, or 33wt% solution, or a. 5()wt% solution, or solid NaOH, or any combination thereof using one or more or any combination of water separation systems and. / or methods.

[1220] Ex am ole 59: Process for Prod ucing Alkaline- Earth Oxide or Alkaline-EarthHydroxide with Carbon Dioxide, Sulfur Dioxide, and / or Alkali Intermediate

[1221] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Ammonium ChlorideCa(WA)ts) + 2 NH-iCKs or g or aq) CaCI2(s or aq) v 2 NHs(g or aq) + H2O(g or aq)

[1222] Note: In some embodiments, the reaction of Ca( WA) with ammonium chloride may be conducted at a solid phase or at a solid-gas mixture phase. For example, 2 NHiiClts) and Ca(WA)(s) may be heated, which may result in the vaporization of NH4CI into NH3(g) and HCI(g), wherein the HCl(g) may react with the Ca(WA)(s) to form, for example, CaCh(s) and. / or ( WA) and / or water.

[1223] Note: In some embodiments, W A may comprise, for example, including, but not limited to, one or more or any combination of the following; a silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide.

[1224] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid-liquid phase or a solid-aqueous phase. For example, 2 NH4CI(aq) and Ca( WA)(s) may be mixed, and / or may react to form, for example, CaCh(aq) and 2 NH3(aq or g).

[1225] (2) CaClXs) + Water CaCh(aq)

[1226] Note: In some embodiments, CaCh from step 1 may comprise a solid and / or may be dissol ved in water to form an aqueous solution.

[1227] (3) Ammonia or weak base may be dissolved in water or aqueous solution to form aqueous ammonia, and / or ammonia may be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate.• CaCh(aq) + 2 NHfrg) -> CaCh(aq) + 2 NHfraq)• 2 NH3(g) + Water → NWaq)• 2 NHfrg (1 or aq ) + CO2(g)4ftO(l (1 or aq +) (NHfrjCOfraq)• 2NH?(g (1 or aq4) 2 COfrg)42 H2O(l or aq) 2 NH^HCOfraq)• (NMOiCO3(aq)4CO2(g) + H3Ofl or aq) “^2 NH-iHCO3faq.)

[1228] Note: In some embodiments, NH? from step 1 may comprise a gas and / or may be dissolved in CaCh(aq).

[1229] Note: In some embodiments, Nffc may be dissolved in water and / or reacted with CO2separately from CaCh.

[1230] (4) Calcium chloride may be reacted with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate.

[1231] CaCh(aq)42 NH3(aq) fe CO2(g) + HJO "9 2 NlbQ(aq) + CaCO3(s)

[1232] CaCh(aq)42 NH3(aq)42 CO2(g)4H»O 2 NHK'l(aq)4CaCO3(s)4COfrg) p233] CaCb(aq)4(NHaJjCO3(aq) → 2 NH*Cl(aq) + CaCO3(s)

[1234] CaCh(aq)42 NHtHCO2(aq) 2 NftCl(aq) -v CaCOds) + CO2(g)

[1235] Note: In some embodiments, if excess CO2is present or CO:; is in the product, in some embodiments, said excess CO2may be transferred to the inputs or reactants of step 4 and / or the inputs or reactants of step 3.

[1236] Note: in some embodiments, a CaCb(aq) +• NBh(aq) solution may be produced in step 1 and / or may be transferred to step 4, potentially skipping step 2 and step 3.

[1237] Note: In some embodiments, CO2(g) may comprise captured CO2from another embodiment described herein. For example, in some embodiments, CO2(g) may comprise CO2from the reaction of calcium carbonate with acetic acid.

[1238] Note: In some embodiments, CaCO2(s) may be transferred to or may comprise an input to one or more or any combination of embodiments described herein. For example, CaCOb(s) may be an input to a process for producing sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof

[1239] Note; In some embodiments, CO2(g) may comprise CO2from an emissions source, or a point source, or air, or from an external source, or any combination thereof. f :124O| Note: In some embodiments, 2 NFFCi(aq) may be transferred to step I.

[1241] Note: in some embodiments, 2 NFUCl(aq) may be transferred to step 5.

[1242] (5) 2 NWCK'aq) → 2 N%Cl($) + Water

[1243] Note: In some embodiments, 2 NH-iCRs) may be transferred to step 1.

[1244] Note: in some embodiments. Water may be transferred to step 3 and / or step 4.

[1245] (6) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid + Ca€O2(s or aq) •+ 2 CH3COOHi'aq) Ca(CH3COO)?(aq) + CO2(g) • Calcium Siiicate(s) + 2 CH3COOH(aq) → Ca(CHrCOO)2(aq) + Silicon Dioxide(s)• CaS(s) + 2 CH.vCOOH(aq) → Ca(CH3COO)2(aq) + H3.S(g)• CalcRim(Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH3COO)d'aq) + Weak Acidfs, or g, or 1, or aq)

[1246] Note: Residua(s olids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[1247] Note: If CO2(g) is produced, it may be desirable sfoaird CO2(g) to be produced at a high partial pressure CO3(g), or purity' CO2(gj, or to comprise captured CO2tg).

[1248] Note: CaCO3may be from step ‘4’.

[1249] Note: CO2may be transferred to step '3’ or step ‘4’.

[1250] (7) Ca(CH.tCOO)2(aq) + Na2.SO.t(s or aq) < 2 NaCH3COO(aq) + CaSO5(s)

[1251] Note: CaSO2(s) may be separated using a solid-liquid separation.

[1252] Note: In some embodiments, NaiSO3(s or aq) may comprise a solid comprising sodium sulfite, which may be added to or dissolved in a solution comprising calcium acetate.

[1353] Note: In some embodiments, Na2SO3fs or aq) may comprising an aqueous solution comprising sodium sulfite and acetic add.

[1254] (8) 2 NaCH3COO(aq) + SOafg or aq) + H2O(1 (1 or aq +) Na2SQ?(aq) + 2 CH3COOH(aq)

[1255] Note: in some embodiments, SO2(g) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodimen ts, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth

[1256] (9) NfeSOKaq) + 2 CH3COOH(aq) → 2 CH3COOH(aq or 1) + Na2SO3(s)

[1257] Note: CH3COOH may be more soluble in water than Na2SO3. In some embodiments, NazSO3may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[1258] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments, CH3COOH may evaporate with water vapor and / or condense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq).

[1259] Note: In some embodiments, magnesium stilfite(aq) may be present in the Na2.SO2(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO>. In some embodiments magnesium sulfitesolid may be separated during step ‘(9)'. In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof, s

[1260] Note: NatSOKs) may be separated from CHCOOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1261] Note; In some embodiments, a feed solution Comprising sodium sulfite and acetic acid may be evaporated, wherein a portion of acetic acid and water vapor evaporate and Z or are condensed to form an a separated acetic acid solution, and / or the remaining solution comprises aqueous acetic acid and a higher concentration of sodium sulfite than in the concentration of sodium sulfite in the feed solution.

[1262] (10) CaSO3(s) CaO(s) + SOfog)

[1263] Note: ‘(I 0)’ may comprise calcining CaSOi(s), which may employ a kiln.Note: CaSOj(s) may be dried, or dehydrated, or both before, or duringK(10)

[1265] Example 60 : Process for Producing Al kali Carbona te or Alkali Bic ar bon ate with Carbon Dioxide, Alkali Carbonate, and / or Sulfur Dioxide Intermediates

[1266] (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Ammonium Chloride• Ca(WA)($) + 2 NH3Clfs or g or aq) CaChCs or aq) + 2 NH3(g or aq) + HjOfg or aq)

[1267] Note; In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid phase or at. a solid-gas mixture phase. For example, 2 NH-tC'Xs) and Ca(WA)(s) may be heated, which may result in the vaporization of NEUCl into NEEff g) and HCI(g), wherein the HCl(g) may react with the Ca(WA')(s) to form, for example, CaCh(s) and / or (WA) and / or water.

[1268] Note: In some embodiments, WA may comprise, for example, including, but not limited to, one or more or any combination of the following; a silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide.

[1269] Note: In some embodiments, the reaction of Ca(WA) with ammonium chloride may be conducted at a solid-liquid phase or a solid-aqueous phase. For example, 2 NFkCI(aq) and Ca(WA)($) may be mixed, and / or may react to form, for example, CaCh(aq) and 2 NHj(aq or g).

[1270] (2) CaCHs) + Water + CaCh(aq)(.1271} Note: In some embodiments, CaCb: from step 1 may comprise a solid and / or may be dissolved m water to form an aqueous solution.

[1272] (3) Ammonia or weak base may be dissolved in water or aqueous solution to form aqueous ammonia, and / or ammonia may be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate.

[1273] Note: In some embodiments, NH3from step I may comprise a gas and / or may be dissolved in CaCb(aq).

[1274] Note: in some embodiments, NH3may be dissolved in water and / or reacted with CO2separately from CaCh.

[1275] (4) Calcium chloride may be reacted with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any comb ination thereof t o form ammonium chloride and calcium carbonate.

[1276] Note: In some embodiments, if excess CO2is present or CO3 is in the product, in some embodiments, said excess CO2, may be transferred to the inputs or reactants of step 4 and / or the inputs or reactants of step 3.

[1277] Note: In some embodiments, a CaCb(aq) + NFlM'aq) solution may be produced in step 1 and / or may be transferred to step 4, potentially skipping step 2 and step 3.

[1278] Note; In some embodiments, CO2(g) may comprise captured CO2from another embodiment described herein. For example, in some embodiments, CO2(g) may comprise CO2from the reaction of calcium carbonate with acetic acid.

[1279] Note: in some embodiments, CaCO3(s) may be transferred to or may comprise an hiput to one or more or any combination of embodiments described herein. For example, CaCO3(s) may be an input to a process for producing sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate^ or sodium carbonate, or any combination thereof.)1280) Note: In some embodiments, CO2(g) may comprise CO2from an emissions source, or a point source, or air, or from an external source, or any combination thereof.

[1281] Note: In some embodiments, 2 NHdCl(aq) may be transferred to step 1 .) 12821 Note: In some embodiments, 2 NBUCl(aq) may be transferred to step 5. p283| (S) 2 NFhCI(aq) 2 NH-iCI(s) + Water

[1284] Note: In some embodiments, 2 Nl-UCl(s) may be transferred to step 1 .

[1285] Note: In some embodiments, Water may be transferred to step 3 and / or step 4.)1286) (6) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth ~Weak Acid Anion with Acetic Acid• CaCO3(s oraq) + 2 CHtCOOH(aq) (MCFl:O)0).<(aq) + CO3(g) + HsO(aq or 1)• Calcium Silicate(s) + 2 CH3COOH(aq) CaCCH3COO)2(aq) + Silicon Dioxide(s) + EbO(aq or I)• CaS(s) •+ 2 CHtCOOH(aq) Ca(CH3COO)2(aq) + HsS(g)• CaIcium(Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH$COO)2(aq)+Weak Acid(s, or g, or 1, or aq) + H3O(aq or 1)

[1287] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.)1288) Note: CaCO3may be from steps4\

[1289] Note: CO2(g) may comprise captured CO3.

[1290] Note: In some embodimenis, CO:>(g) may be employed internally or employed in other steps. For example, in some embodiments, CO2(g) may be employed in step ‘(10)’.

[1291] Note; In some embodiments, CO2t'g) may be utilized or sequestered or sold or comprise a product. For example, C€h(g) may be utilized or sequestered or sold to a CO2sequestration site or a CO2EOR application or an external application,

[1292] Note: In some embodiments, some chemicals comprising calcium may comprise aportion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[1293] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g)

[1294] Note: In some embodiments, acetic acid for step ‘(6)’ may comprise aqueous acetic acid produced or regenerated in step ‘(9)’.

[1295] (2) Ca(C.H3COO)2(aq) + Na2SO^s or aq) → 2 NaCH3COOf'aq) - CaSOfrs)

[1296] Note: In some embodiments, Na2SO<s) may be added directly to or dissolved in CatCH3COO)2(aq),

[1297] Note: In some embodiments, NSJSOACS) may be dissolved in water or an aqueous solution to form Na2SCMaq) before mixing with Ca(CH3COO).:(aq).

[1298] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. In some embodiments, water may be added to the process by NaiSO.i being in the form of NteSOdaq) or an aqueous solution comprising sodium sulfate, wherein at least a portion of the water in Na2SCWaq) may comprise water added to the process. In some embodiments, Na2SChtaq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SCMaq) may be provided to the process in the form of Na2SOfraq). In some embodiments, NarSOfoaq) may be provided or sourced as a solid or Na2SOMs), then dissolved in water to form Na2SOaCaq).

[1299] Note: In some embodiments, Ca(CH.tCOO)2(aq) may comprise Ca(CH3COO)2(aq) from step ‘(6)’.

[1300] (8) 2 NaCH3COO(aq) + SO2(g (1 or aq ) + H2O(I (1 or aq) Na2SOfraq) + 2CI-bCOOH(aq)

[1301] Note: in some embodiments, SO2(g) may comprise other gases in addition to SO2(g). Ill some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a porti on of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COOtaq) entering the present step may be pie-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCI-frCOOiaq) with SOe(g). In some embodiments, acetic acid vapor may be removed from remaining gases using, for exampie,including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate — water slurry, or alkaline earth oxide, or alkaline earth,

[1302] Note; In some embodiments, NaCH3CQO(aq) may comprise NaCHCQ()(aq} from step ‘(7)’.

[1303] Note: In some embodiments, SO2may comprise S£h(g) from the calcination or decomposition of CaSO3(s) in step “(ll)',

[1304] (9) Na2SOfraq) - 2 CH?COOH(aq) → 2 CH3COOH(aq) + Na2SO3(s)

[1305] Note: CHrCOOH may be more soluble in water than Na2SO-a. In some embodiments, Na2SO2may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1306] Note: In some embodiments, CH3COOH and / or water may be separated from Na2SO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof In some embodiments, CH3COOH may evaporate with water vapor and / or condense with water vapor, which may result in a distillate Or condensate comprising CH3COOHtaq).

[1307] Note: In some embodiments, magnesium sitlfite(aq) may be present in the Na2SO3(aq) + 2 CH3COO Hl aq). In some embodiments, if present, magnesium sul fite may begin to precipitate or crystalize before Na-rSCh. In some embodiments magnesium sulfite solid may be separated during step ‘(9)’. In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof-S

[1308] Note: Na2SO3(s) may be separated from CH3COOH (aq) by a solid-liquid separation, which may include, but is not limited io, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1369] (10) React an Alkaline-Earth - Weak Acid, such as an Alkaline-Earth Carbonate, with Carbon Dioxide and / or Water to Form an Alkaline-Earth Bicarbonate* CaCO2(s) + CO2(g (1 or aq ) + H2O(aq) Ca(HCO3)2( aq)• MgCO3(s) + CO2(g (1 or aq) H2O(aq) → Mg(HCO3)2( aq)

[1310] Note: May be conducted under a pressurized CO2atmosphere or with concentrated carbonic acid or CO2(aq). For example, the CO2partial pressure during the reaction may be greater than, for example, 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bai; or 8 Bar, or 9 Bar, or 10 Bar, or any combination thereof.

[1311] Note: In some embodiments, CaCO2(s) or MgCO3(s) may comprise CaCO2(s) or MgCO3(s) from step "(13)’.

[1312] Note: In some embodiments, Ca.CO3(s) or MgCOK.s) may comprise an input, such as limestone, or dolomite.

[1313] Note: In some embodiments, CO2(g or aq) may comprise CO2from step '(6)’.

[1314] Note: In some embodiments, COtCg or aq) may comprise CO2from an emissions source, or another CO2source, or captured CO2, or any combination thereof. For example, in some embodiments, CO2(g or aq) may comprise, including, but not limited to, one or more or any combination of the following: CO2from a blue hydrogen or blue ammonia facility, or an ammonia facility, or an ethanol plant, or a carbon capture plant.|13.1S| (II) React an Alkali Sulfite with an Alkaline-Earth Bicarbonate to form an Alkali Bicarbonate and an Alkaline-Earth Sulfite11316( Note: In some embodiments, Na2SO3(s) may be dissolved in. water or may comprise an aqueous solution before or during mixing with an aqueous solution comprising Ca(HCO3)2(aq) or Mg(HCO03(aq).

[1317] Note: At least a portion of CaSO3(s) or MgSO3(s) may be separated by a solid- liquid separation.

[1318] Note: In some embodiments, NallCO3may be sold as a product or employed as a carbon sequestration medium,

[1319] Note; In some embodiments, NaHCCb may be concentrated and / or crystalized into a. solid, such as. for example, solid sodium bicarbonate or solid sodium carbonate.

[1320] (12) Decompose an Alkaline-Earth Sulfite into an Alkaline-Earth Oxide andSulfur Dioxide• CaSO3(s) CaO(s) + SO2.(g)• MgSO3(s) -> MgO(s) + SO2(g)

[1321] Note: May comprise calcining CaSO3(s) or MgSO3(s), which may employ a kiln,

[1322] Note: CaSCh(s) or MgSO3(sjmay be dried, or dehydrated, or both before or during calcining.

[1323] Note: CaSO3(s) or MgSOa(s) may comprise CaSO3(s) or MgSO3(s) from step ( I D’.

[1324] Note: CaO or MgO may comprise a valuable product if desired. For example,CaO or MgO may comprise an ultra-low carbon emissions CaO or MgO product.

[1325] (13) React an Alkaline-Earth Oxide or Hydroxide with Carbon Dioxide to form anAlkaline Earth Carbonate + CaO(s) + CO2(g) CaCO2fo)• MgOCs) + CO2(g) MgCO3(s)

[1326] Note: In some embodiments, CaO(s) or MgO(s) may be reacted with water to form Ca(OH)r(aq), or Ca(OH)2(s or aq), or Mg(OH):(aq), or Mg(OHk(s or aq), or any Combination thereof which may comprise Milk of Lime, or Milk of Magnesia, or a solid- liquid suspension comprising calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH)r or Mg(OH)2may be reacted with a carbonate salt, such as sodium carbonate or sodium bicarbonate, to form CaCO3or MgCO3, or may be reacted with CO3to form CaCO3or MgCO2. For example, said sodium carbonate or sodium bicarbonate may comprise sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassiumbicarbonate, or alkali carbonate, or alkali bicarbonate, or any combination thereof employed in or as a CO2absorption solution,

[1327] Note; In some embodiments, CO2(g) may comprise CO2in or from a point source CO2emissions source. For example, CO2(g) may comprise One gas, or dilute CO2, or high purity CO2, or captured CO2,

[1328] Note: In some embodiments, CO2(g) may comprise CO2in or from air. For example, COrig) may comprise air which may comprise at least a portion of CO2even if at a very dilute concentration. For example, calcium oxide may be capable of reacting with very low concentrations or very dilute concentrations of CO2if desired . For example, CO2(g) may comprise a carbonate salt, such as sodium carbonate or potassium carbonate, wherein the carbonate may comprise carbonate originating from the reaction of carbon dioxide in the air with a sodium or potassium or other alkali salt,, such as sodium hydroxide or potassium hydroxide, forming the alkali carbonate salt, and / or wherein the reaction of calci um oxide or calcium hydroxide with the alkali carbonate may result in the regeneration or formation of an alkali hydroxide or alkali oxide or other alkali salt which may be employed to absorb carbon dioxide from the air a regenerate or re-form the alkali carbonate salt.

[1329] Note: In some embodiments, CaCO2or MgCO3may comprise a valuable product In some embodiments, CaCO2or MgCO2may comprise a carbon sequestration medium.( .1330 } Exam pie 61: Process for Producing Sodiant flvdroxide with Sulfur Dioxide,Carbon Dio side, Carboxylic Acid, and Magnesio m Intermediates1 (1) React Material comprising Calcium, or Magnesium, or Other Alkaline Earth - Weak Acid Anion with Acetic Acid• CaCO2(s or aq) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + CO2(g) + H2O(aq or 1)• Calcium Silicate(s) + 2. CH3COQHfoq) Ca(CH3COO)2(aq) Silicon Dioxide(s) + HsO(aq or I)• CaS(s) + 2 CHtCOOH(aq) → Ca( CH3COO)2(aq) + H?S(g)• CalciumfWeak Acid Anion) + 2 CH3COOH(aq) → Ca(CH3COO)?(aq) + Weak Acid(s, or g, or 1, or aq) + HtO(aq or I.)

[1332] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[1333] Note: CO2(g) may comprise captured CO2.

[1334] Note: In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input material may comprise a mixture of calcium and magnesium.

[1335] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[1336] Note: In some embodiments, acetic acid for step h l)’ may comprise aqueous acetic acid produced or regenerated in step 44)’.

[1337] (2) Ca(CH3COOfriaq) + Na2SOds (1 or aq) 2 NaCH3COO(aq) + CaSO*(s)

[1338] (3) 2 NaCH3COO(aq) + SO2(g (1 or aq +) H3O(i (1 or aq -4) Na2SO3(aq) + 2CHCOOH(aq)

[1339] (4) Na2SOfraq)+ 2 CH3COOH(aq) → 2 CH5COOH(aq) + Na2SO3(s)

[1340] (5) MgCO3(s) + CO2(g or aq) FhO(aq) "4 MgfHCO3Xaq)

[1341] Note: May be conducted under a pressurized CO2atmosphere or with concentated carbonic acid or CO2(aq). For example, the CO2partial pressure during the reaction may be greater than, for example, 0.5 Bar, or I Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 111 Bar, or arty combination thereof.

[1342] Note: In some embodiments, MgCO;?(s) may comprise MgCO2(s) from the reaction of MgO or Mg(OH):> with CO2.

[1343] Note: In some embodiments, CO3fg (1 or aq m) ay comprise CO2from step (1 )’, or step ’ (9)’, or any combination thereof. For example, in some embodiments, the reaction of MgO or Mg(OHh with CO2, may comprise capturing CO2from the calcination or decomposition of calcium carbonate and t or may enable the calcium carbonate calciner io produce dilute carbon dioxide or flue gas carbon dioxide because carbon dioxide in said dilute or flue gas carbon dioxide may be captured by the reaction with magnesium oxide and / or magnesium hydroxide. p344| (6) Na2SOx(s or aq) + Mg(HCO2Maq) 2 NaHCOdaq) + MgSOa(s)

[1345] Note: In some embodiments, Na2SO,?('s) may be dissolved in water or may comprise an aqueous solution before mixing with an aqueous solution comprising Mg(HCO2)2(aq).

[1346] Note: At least a portion of CaSO3(s) or MgSO3(s) may be separated by a solid- liquid separation.

[1347] Note: In some embodiments, NaHCO3may be sold as a product or employed as a carbon sequestration medium.

[1348] Note: In some embodiments, Na2.SO3(s or aq) may comprise NaiSO3from step (4 >\

[1349] Note: In some embodiments, Mg(HCO3Maq) may comprise Mg(HCO3Maq) from step ‘(5)’-

[1350] Note: In some embodiments, residual MgSO3may be present as, for example, MgSO3(aq) in the solution comprising sodium bicarbonate, In some embodiments, it may be desirable to separate at least a portion of residual MgSO3from at least a portion of sodium bicarbonate. For example, in some embodiments, said separation may comprise, including, but not limited to, one or more or any combination of the following: electrodialysis, or selective electrodialysis, or monovalent selective electrodialysis (MSED), or divalent selective electrodialysis (DSED), or concentrating, or cooling precipitation, or reverse osmosis, or membrane based process, or nanofiitration.

[1351] (7) MgSO3(s) MgO(s) + SO2(g)

[1352] Note: The thermal decomposition of magnesium sulfite may be conducted with less energy and / or at lower temperatures than the thermal decomposition of calcium sulfite

[1353] Note: Sulfur dioxide formed may be employed, for example, in the reaction of alkali acetate or alkali carboxylate with sulfur dioxide,

[1354] (8) React Magnesium Oxide or Magnesium Hydroxide with Carbon Dioxide toForm Magnesium Carbonate• MgO(s) + CO2(g) MgCO2(s) • MgO(s) + H2O(1 or g or s) Mg(OH)2.(s or aq) + Mg(OH)3(s or aq) + CO2(g) MgCO2(s) + H2O(1 or g or s)

[1355] Note; In. some embodiments, the CO2(g) may comprise SO2(g) t) from the decomposition of calcium carbonate.

[1356] Note: In some embodiments, the CO3(g) may comprise CO3(g.) from an emissions source, or point source, or air.

[1357] Note: MgCO3(s) may comprise the MgCO2(s) In the reaction of MgCO3(s) CO2+H2O.

[1358] (9) NaHCO3(aq) -> 2 NaHC€h(s) + Water

[1359] Note: In some embodiments, NaHCO3(s) may be formed by process or cycle comprising concentrating and cooling precipitation, or a precipitation or crystallization process, or any combination thereof

[1360] Note: In some embodiments, NaHCOi may be sold as a product and / or employed as a carbon sequestration medium.

[1361] Note: In some embodiments, 2 NaHCO3(aq) may be decomposed into NarCO3(aq) and CO2(g) and water within an aqueous and / or under-pressure or pressurized environment, which may avoid or prevent the need for crystallizing or precipitating NaHCOj(s). jl362| Note: In some embodiments, at least a portion of residual dissolved MgSO3or magnesium sulfite, if any, may be separated and / or precipitated.

[1363] Note: Water may be separated from sodium bicarbonate or sodium carbonate using systems and methods for water separation, or systems and methods for salt precipitation or crystallization, or any combination thereof

[1364] (10) 2 NaHCOi(s) → Nn2CO2(s) + CO2(g) + HcOfg or I)

[1365] Note: CO2(g) may comprise captured CO2.

[1366] Note: In some embodiments, Na2.C0a may be sold as a product and / or employed as a carbon sequestration medium,

[1367] Note: In some embodiments, NaiCOi(s) may be dissolved in water or an aqueous solution and / or comprise the NazCO3(s) i» the reaction of Ca(OHh and Na2CO3(s)

[1368] (11) Calcine or decompose an alkaline-earth carbonate to form an alkaline earth oxide and carbon dioxide. CaCCh(s) •> CaO(s) + CO2(g)• MgCOi(s) MgO(s) + CO:'(g)

[1369] Note: In some embodiments, it may be desirable to decompose calcium carbonate or magnesium carbonate in a manner which the carbon dioxide is high purity, or in a mannerwhich the carbon dioxide is captured, or in a manner which the carbon dioxide is dilute but then captured, or any combination thereof.

[1370] Note: In some embodiments, carbon dioxide from the decomposition of calcium carbonate or magnesium carbonate may comprise the carbon dioxide in the reaction of magnesium oxide or magnesium hydroxide and carbon dioxide,

[1371] (12) React an alkaline-earth oxide or hydroxide with an alkali carbonate to form an alkaline-earth carbonate and an alkali hydroxide• CaO(S or aq) + Na2CO3(s (1 or aq +) Water → 2 NaOH(aq) + CaCOfrs) » MgO(s or aq) + NazCO3fs (1 or aq +) Water→ 2 NaOH(aq) + MgCOrt s)• Ca(OHh(s or aq) + NazCO3(s or aq) 2 NaOH(aq) + CaCO2(s)• MgO(s or aq) + NazCOzfs (1 or aq +) 'Water 2 NaOH(aq) + MgCQj(s)

[1372] Note: In some embodiments, CaO+ NazCO3(s or aq) h Water or MgO + NazCO^s or aq) + Water may be conducted in multiple steps. For example, in some embodiments, CaO or MgO may be reacted with water to form Ca(OH.h(s), Ca(OH)2(aq), or Ca(OH )e< s or aq), or MgCOH)2(aq), or Mg(0Hh.(s or aq), which may comprise Milk of Lime or Milk of Magnesia, or a solid-liquid suspension comprising calcium hydroxide ormagnesium hydroxide. For example, in some embodiments, NazCO3may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, a solution or solid-liquid mixture or suspension comprising Ca(OH)2(s or aq), or Milk of Lime, or Mg(0H)2, or Milk of Magnesia may be mixed with an aqueous solution comprising NazCO3(aq), which may resul t in the formation of a solution comprisin g aqueous sodium hydroxide and a solid comprising calcium carbonate or magnesium carbonate.

[1373] Note: In some embodiments, at least a portion of calcium carbonate or magnesium carbonate may be separated from at least a portion of sodium hydroxide using, for example, a solid-1 Squid separation .

[1374] Exam nle 62 ; P r press for Producing Sodium Bicarbon ate, or SodiumCarbonate, and / or Calcia m Oxide o r Calciam Ca rbonate

[1375] (I) .React Material comprising Calcium, or Magnesium, or Other Alkaline Earth -Weak Acid Anion with Acetic Acid• CaCCb(s or aq) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + CO2(g) H2O(aq or I)• Calcium S iiicate(s) ? 2 CH3COOH(aq) CaOH3COO)2(aq) + Silicon Dioxtde(s) + FfeO(aq or 1)• CaS(s) + 2 CH3COOH(aq) → Ca(CH£OO)2(aq) + H2S(g)• Calcium(Weak Acid Anion) + 2 CH3COOH(aq) Ca(CH3COO)2(aq) + Weak Acid(s, or g, or 1, or aq) + H2O (aq or I)

[1376] Note: Residual solids or undissolved solids, such as silicon dioxide or other undissolved solids, may be separated from the liquid solution using a solid-liquid separation.

[1377] Note: CO2tg) may comprise captured CO2.

[1378] Note: In some embodiments, CO2(g) may be employed .internally or employed in other steps.

[1379] Note: In some embodiments, C02(g) may be utilized or sequestered or sold or comprise a product. For example, CO2(g) may be utilized or sequestered or sold to a CO2sequestration site or a CO2EOR application or an external application.

[1380] Note; In some embodiments, some chemicals comprising calcium may comprise a portion of magnesium. In some embodiments, for example, input chemicals or input materia! may comprise a mixture of calcium and magnesium.

[1381] Note: In some embodiments, acetic acid vapor and / or water vapor may be separated or recovered from CO2(g).

[1382] (2) Ca(CH3COO)2((aq) + NarSO4Cs or aq) → 2 NaCH3COO(aq) + CaSO3(s)

[1383] Note: In some embodiments, Na2SO4s) may be added directly to or dissolved in Ca(CH3COO)2(aq).Note: In some embodiments, Na2SO4 (s) may be dissolved in water or an aqueous solution to form NmSCMaq) before mixing with Ca(CH3COO):(aq).

[1385] Note: In some embodiments, water may be added to the process to make up for water which may leave the process, for example, if NaOH(aq) is an output, or another aqueous solution is an output, or any combination thereof. In some embodiments, water may be added to the process by Na?S€h being in the form of Na2StXaq) or an aqueous solution comprising sodium sulfate, wherein at least a portion of the water in NarSCM :aq) may comprise water added to the process. In some embodiments, NarSOdaq) may be provided or sourced as an aqueous solution. For example, in some embodiments, Na2SO4aq) may beprovided to the process in the .form of NfoSOfraq). In some embodiments, Na2SO*(aq) may be provided or sourced as a solid or Na2SO^s), then dissolved in water to form NacSO^iaq).

[1386] Note: In some embodiments, Ca(CH3COO),>(aq) may comprise Ca(C&COO)2(aq) from step h l)'.

[1387] (3) 2 NaCMCOO(aq) + SOfrg or aq) + tOfl (1 or aq +) Na2SCh(aq) v 2 CH3COOH(aq)

[1388] Note: In some embodiments, SOrig) may comprise other gases in addition to SO2(g). In some embodiments, the reaction of 2 NaCH3COO(aq) + SO2(g) may result in at least a portion of acetic acid vapor in the remaining gases during or after the reaction. In some embodiments, NaCH3COO(aq) entering the present step may be pre-contacted with or may absorb at least a portion of acetic acid vapor from the remaining gases. In some embodiments, the reactor or absorption column may be configured to absorb acetic acid vapor in NaCH3COO(aq) before or while reacting NaCH3COO(aq) with SO2.(g), In some embodiments, acetic acid, vapor may be removed from remaining gases using, for example, including, but not limited to, one or more or any combination of the following: alkaline earth carbonate, or alkaline earth - weak acid, or alkaline earth carbonate - water slurry, or alkaline earth oxide, or alkaline earth.

[1389] Note: In some embodiments, NaCH3COOtaq) may comprise NaCH3COO(aq) from step ‘(2)’.

[1390] Note: In some embodiments, SO2may comprise SCh(g) from the calcination or decomposition of CaSO3(s) in step ‘(7)’.

[1391] (4) NaaSO3(aq) + 2 CH3COOH(aq) 2 CH3COOH(aq) + Na2SO3(s)

[1392] Note: CH3C'OOH may be more soluble in water than Na2SO3. In some embodiments, NmSO2may be separated or precipitated from solution by, for example, including, but not limited to, evaporation, or distillation, or crystallization, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof.

[1393] Note: In some embodiments, CH3COOH and / or water may be separated from NarSO3by, for example, evaporation, or distillation, or crystallization, or any combination thereof. In some embodiments, CH3COOH may evaporate with water vapor and Z orcondense with water vapor, which may result in a distillate or condensate comprising CH3COOH(aq),

[1394] Note; In some embodiments, magnesium sulfite(aq) may be present in the Na2SCh(aq) + 2 CH3COOH(aq). In some embodiments, if present, magnesium sulfite may begin to precipitate or crystalize before Na2SO3, In some embodiments magnesium sulfite solid may be separated during step ‘(4)’. In some embodiments, separated magnesium sulfite may be decomposed to magnesium oxide, or decomposed separately from calcium sulfite, or decomposed together with calcium sulfite, or any combination thereof. s

[1393] Note; Na2SO3(s) may be separated .from CH3COOH(aq) by a solid-liquid separation, which may include, but is not limited to, filter, or centrifuge, or decanter, or separation systems or methods described herein, or separation systems or methods described in the art, or any combination thereof

[1396] (5) MgCO3(s) + CO2.(g or aq) a- H3O(aq) Mg(HCOOXaq)

[1397] Note: May be conducted under a pressurized CO2atmosphere or with concentrated carbonic acid or COdaq), For example, the CO2partial pressure during the reaction may be greater than, for example, 0.5 Bar, or 1 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or 6 Bar, or 7 Bar, or 8 Bar, or 9 Bar, or 10 Bar, or any combination thereof.

[1398] Note: fo some embodiments, MgCO3(s) may comprise MgCO3(s) from thereaction of MgO or Mg(OH)? with CO2,

[1399] Note: In some embodiments, CO2(g of aq) may comprise CO2from step 1)\ or step "(9)’, or any combination thereof. For example, in some embodiments, the reaction of MgO or MgfOH)? with CO2may comprise capturing CO2from the calcination or decomposition of calcium carbonate and / or may enable the calcium carbonate calciner to produce dilute carbon dioxide or flue gas carbon dioxide because carbon dioxide tn said dilute or flue gas carbon dioxide may be captured by the reaction with magnesium oxide and / or magnesium hydroxide;

[1400] (6) Na2SO3fs or aq) + Mg(HCO3)?(aq) 2 NaHCO2(aq) + MgSO.j(s)

[1401] Note: In some embodiments, Na2SOa(s) may be dissolved in water or may comprise an aqueous solution before mixing with an aqueous solution comprising Mg(HCO2)a(aq),

[1402] Note: At least a portion of CaSO3(s) or MgSO3(s) may be separated by a solid- liquid separation.

[1403] Note: In some embodiments, NallCO3may be sold as a product or employed as a carbon sequestration medium,

[1404] Note; In some embodiments, Nar.SO3(s or aq) may comprise NajSOj from step +(4)'

[1405] Note; in some embodiments, Mg(HCO3Xaq) may comprise Mg(HCO3h(aq) from step ‘(5)’-

[1406] Note: In some embodiments, residual MgSO3may be present as, for example, MgSO3(aq) in the solution comprising sodium bicarbonate, In some embodiments, it may be desirable to separate at least a portion of residual MgSCti from at least a portion of sodium bicarbonate. For example, in some embodiments, said separation may comprise, including, but not limited io, one or more or any combination of the following: electrodialysis, or selective electrodialysis, or monovalent selective electrodialysis (MSED), or divalent selective electrodialysis (DSED), or concentrating, or cooling precipitation, or reverse osmosis, or membrane based process, or nanofiltration,

[1407] (7) MgSO3(s) MgO(s) + SO2(g)

[1408] Note: The thermal decomposition of magnesium sulfite may be conducted with less energy and / or at lower temperatures than the thermal decomposition of calcium sulfite.

[1409] Note: Sulfur dioxide formed may be employed, for example, in the reaction of alkali acetate or alkali carboxylate with sulfur dioxide,

[1410] (8) React Magnesium Oxide or Magnesium Hydroxide with Carbon Dioxide toForm Magnesium Carbonate• MgO(s) + CO2(g) MgCO3(s) • MgO(s) + H3O(i or g or s) Mg(OH)2.(s or aq)* Mg(OH)3(s or aq) + CO2(g) MgCO2(s) + or g or s)

[1411] Note: In some embodiments, the CO2(g) may comprise C O2(g) from the decomposition of calcium carbonate.

[1412] Note: in some embodiments, the CO2(g) may comprise COfr'g.) from an emissions source, or point source, or air, or any combination tfeereof.

[1413] Note: MgCOMs) may comprise the MgCC)2(s) In the reaction of MgCO3(s) + CO2+ H2O• Note: In some embodiments, carbon dioxide from the decomposition of calcium carbonate or magnesium carbonate may comprise the carbon dioxide in the reaction of magnesium oxide or magnesium hydroxide and carbon dioxide.Note: In some embodiments, CaOCs) or MgO(s) may be reacted with water to form Ca(OHh(aq), or Ca(OH) j(s or aq), or Mg(OH)?.(aq), or Mg(OH):’(s or aq), or any combination thereof which may comprise Milk of Lime, or Milk of Magnesia, or a solid-liquid suspension comprising calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH h or Mg(OH>? may be reacted with a carbonate salt, such as sodium carbonate or sodium bicarbonate, to form CaCO3or MgCO2, or may be reacted with CO2to form CaCO3or MgCO3, For example, said sodium carbonate or sodium bicarbonate may comprise sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassium bicarbonate, or alkali carbonate, or alkali bicarbonate, or any combination thereof employed in or as a CO2absorption solution. Note: In some embodiments. CO2(g ) may comprise CO2in or from a point source CO2emissions source. For example, CO-(g) may comprise flue gas, or dilute COx or high purity CO2, or captured CO2.Note: In some embodiments, CO2(g) may comprise CO2in or from air. For example, CO2fg) may comprise air which may comprise at least a portion of CO2even if at a very dilute concentration. For example, calcium oxide may be capable of reacting with very low concentrations or very dilute concentrations of CO2if desired. For example, CO2(g ) may comprise a carbonate salt, such as sodium carbonate or potassium carbonate, wherein the carbonate may comprise, carbonate originating from the reaction of carbon dioxide in the air with a sodium or potassium or other alkali salt, such as sodium hydroxide or jxitassium hydroxide, forming the alkali carbonate salt, and / or wherein the reaction of calcium oxide or calcium hydroxide with the alkali carbonate may result in the regeneration or formation o f an alkali hydroxide or alkali oxide or other alkali salt which may be employed to absorb carbon dioxide from the air a regenerate or re-form the alkali carbonate salt.Note: In some embodiments, CaCO2or MgCO3may comprise a valuable product. In some embodiments, CaCO3orMgCOi may comprise precipitated calcium carbonate.In some embodiments,. CaGO3or MgCO3may comprise a carbon sequestration medium.EXAMPLE DESCRIPTION ALKALINE EARTH O3( IDE PRODUCTION SYSTEMS AND METHODSDescription

[1414] Some embodiments of the present invention may pertain to systems and methods for producing alkaline earth oxides, or alkaline earth hydroxides, or cement, or cl inker. Some embodiments of the present invention may pertain to producing alkaline earth oxides, or alkaline earth hydroxides, or cement, or clinker, which may comprise a chemical or material comprising calcium, or magnesium, or other alkaline earth.

[1415] Some embodiments may involve producing alkaline earth oxides, or alkaline earth hydroxides, or cement, or clinker using an input material comprising an alkaline-earth weak acid material. For example, in some embodiments, the alkaline-earth weak: acid material may comprise a carbonate, which may include, but ss not limited to, one or more or any combination of the following: calcium carbonate, or magnesium carbonate, or limestone, or calcium-magnesium carbonate, or dolomite, or any combination thereof. For example, in some embodiments, the alkaline-earth weak acid material may comprise a silicate material, which may include, but is not limited to, one or more or any combination of the following: a calcium silicate, or a magnesium silicate, or orthosilicate, or fluorosilicate, or metasilicate, ar pyrosilicate, or aluminosilicate, or silicon oxide, or silicon material, or any combination thereof In some embodiments, the alkaline-earth weak acid material may comprise a sulfide material, which may include, but is not limited to, one or .more or any combination of the following: a calcium sulfide, or a magnesium sulfide, or any combination thereof. For example, in some embodiments, the alkaline-earth weak acid material may comprise a metal oxide or metal oxide derivative anion material, which may include, but is not limited to, one or more any combina t ion of the following: aluminate, or ferrate, ferrite, or zincate, or manganate, or clay, or permanganate. In some embodiments, the alkaline-earth weak acid material may comprise an alkaline earth metal in a compound with an anion or acid derivative or any combination thereof wherein the anion or acid derivative may comprise a derivative or may originate from an acid with a lower acid strength or weaker acid strength than sulfur dioxide, or aqueous sulfur dioxide, or sulfurous acid, or sulfite, or any combination thereof. In some embodiments, the alkaline-earth weak acid material maycomprise metal oxides or metal hydroxides which may possess overlapping or similar chemistry or similar properties to calcium, or magnesium, or other aikaiine-earths. In some embodiments, the alkaline-earth weak acid material may comprise impurities. In some embodiments, the alkaline-earth weak acid material may comprise, including, but not limited to, one or mom or any combination of any of the aforementioned chemistries or properties.

[1416] In some embodiments producing cement, or clinker, or any combination thereof, it may be desirable to mix elay, or silicon material, or other cement raw mix components with the alkaline earth at one or more or a combination of points in the process. For example, in some embodiments, raw mix components may be added to calcium sulfite or magnesium sulfite before or during decomposing the sulfite into sulfur dioxide. For example, in some embodiments, raw mix components may be added to calcium oxide or magnesium oxide before or during sintering or fusing to form cement or clinker.

[1417] Some embodiments may involve producing alkaline earth oxides, or alkaline earth hydroxides, or cement, or clinker, or any combination thereof using an input material comprising an alkaline-earth weak, acid material. In some embodiments, the alkaline-earth weak acid material may be reacted with or mixed with an acid with an acid strength greater than the "weak acid' and an acid strength weaker than salfurous acid. In some embodiments, the alkaline-earth weak acid material may be reacted with or mixed with an acid with an acid strength greater than the ‘weak acid' and an acid strength weaker than sulfurous acid, which may result in the formation of an aqueous solution comprising a salt comprising the alkaline earth and an anion of the acid with an acid strength greater than the ' weak acid' and an acid strength weaker than sulfurous acid, In some embodiments, the alkaline-earth weak acid material may be reacted with or mixed with an acid which displaces the weak acid from the alkaline earth or reacts with the alkaline earth. In some embodiments, the alkaline-earth weak acid material may be reacted with or mixed with an acid which displaces the weak acid from the alkaline earth or reacts with the alkaline earth, which may result tn the formation of an aqueous solution comprising a salt comprising the alkaline earth and an anion of the acid which can displace the weak acid from the alkaline earth. For example, some carboxylic acids, such as formic acid, or acetie acid, or propanoic acid, may have an acid strength greater than some weak acids and weak acid derivatives, such as carbonates, or bicarbonates, or sulfides, or silicates, and / or may react with the alkaline earth weak acid material to produce an aqueous solution comprising an alkaline earth - carboxylic acid anion and / or a displaced weak acid. For example, in some embodiments, it may be desirable to react the alkaline earth-• weak acid material with an acid or aqueous acid to form an aqueous alkaline earth solution. For example, in some embodiments, an alkaline-earth weak acid solid comprising calcium carbonate may be reacted with an acid comprising acetic acid, which may result in the formation of a dissolved alkaline earth carboxylic acid anion solution comprising dissolved aqueous calcium acetate and a displaced weak acid comprising carbonic acid, or aqueous carbon dioxide, or gaseous carbon dioxide, or any combination thereof. For example, in some embodiments., an alkaline-earth weak acid solid comprising a calcium silicate may be reacted with an acid comprising acetic acid, which may result in the formation of a dissolved alkaline earth -- carboxylic acid anion solution comprising dissolved aqueous calcium acetate and a displaced weak acid comprising silicon dioxide solid.

[1418] In some embodiments, the reaction of an alkaline earth weak acid with an acid may be gas evolving, or solid evolving, or liquid evolving or aqueous solution evolving, or any combination thereof, In some embodiments, the ‘weak acid’ may be displaced by the acid which may be stronger than the weak acid and / or weaker than sulfurous acid. In some embodiments, the weak acid may be displaced and may form a gas or aqueous solution, which may include, but it not limited to, one or more or any combination of the following: carbon dioxide, or carbonic acid, or hydrogen sulfide, or hydrosulfuric acid. In some embodiments, it may be desirable for evolved gas or gas comprising the displaced weak acid to be captured or isolated. For example, the reaction of an alkaline earth weak acid with an acid may be conducted in an environment or container such that evolved gas may pressurize, or accumulate, or be produced at a partial pressure greater than the partial pressure of the chemical in ambient air or the Earth's atmosphere. For example, the reaction of an alkaline earth weak acid with an acid may be conducted in an. environment or container such that evolved gas may comprise a volumetric concentration greater than the volumetric concentration greater than the volumetric concentration of the gas in the Earth's atmosphere or ambient air. For example, a solid comprising calcium carbonate or magnesium carbonate may be reacted with acetic acid to form calcium acetate and a gas comprising carbon dioxide, wherein the reactor may be configured to enable file pressurization or accumulation of carbon dioxide gas such that the carbon dioxide gas produced is at a partial pressure, for example, greater than 0.01 Bar, or 0. ] Bar, or 0.3 Bar, or 0.5 Bar, or 0.7 Bar, or 1.0 Bar, or 2 Bar, or 3 Bar, or 4 Bar, or 5 Bar, or any combination thereof or , for example, a concentration greater than 1 vol%, or 5vol%, or 10vol%, or 20vol%, or 30vol%, or 40vol%, or 50vol%, or 60vol%, or 70vol%, or 80vol%, or 90vol%, or 95vol%, or any combination thereof. In someembodiments, it may be desirable for the gas evolving reaction to be conducted in a batch configuration, due to, for example, the fast reaction kinetics and / or the ability to achieve greater evolved gas partial pressures. In some embodiments, it may be desirable for the gas evolving reaction to be conduc ted in a semi-continuous, or continuous fashion or configuration. In some embodiments, it may be desirable for the gas produced to be stored, or transferred, or converted, or transported, or utilized, or sequestered, or further compressed, or further treated, or any combination thereof. For example, if carbon dioxide is produced, it may be desirable to, including, but not limited to. one or more or any combination of the following: convert the carbon dioxide into a valuable product, or convert the carbon dioxide into a sequestration product, or compress the carbon dioxide, or liquefy the carbon dioxide, or turn the carbon dioxide in to a supercritical fluid, or transfer the carbon dioxide to a utilization application, or sequester the carbon dioxide, or employ the carbon dioxide in enhanced oil recovery, or any combination thereof. For example, if hydrogen, sulfide is produced, it may be desirable to, including, but not limited to, one or more or any combination of the following: convert to sul fur, or employ in the Claus process, or produce heat, or combust, or produce sulfur dioxide, or produce sulfur dioxide makeup, or convert sulfate to sulfit e or sulfide, or produce power, or produce steam, or produce sulfurous acid, or produce sulfuric acid, or employ in an application, or transport, or store, or any combination thereof.

[1419] In some embodiments, the reaction of an alkaline earth weak acid with an. acid may be gas evolving, or solid evolving, or liquid evolving or aqueous solution evolving, or any combination thereof. In some embodiments, the ‘weak acid’ may be displaced by the acid which may be stronger than the weak acid and / or weaker than suiforous acid. In some embodiments, the weak acid may be displaced and may form a solid, which may include, but it not limited to, one or morn or any combination of the following: silicon dioxide, or silicon oxide, or metal oxide. For example, a calcium silicate may be reacted with acetic acid to form aqueous calcium acetate and a solid comprise, silicon dioxide. The solid silicon dioxide may be separated from the aqueous calcium acetate by, for example, a solid-liquid separation. In some embodiments, the solid may be utilized. For example, silicon dioxide may be employedas an aggregate for concrete production. In some embodiments, the solid may be discarded. In some embodiments, a solid forming reaction may be desirable because, for example, a solid farming reaction may avoid, or minimize, or prevent, or reduce the potential production of and / or handling of a greenhouse gas, such as carbon dioxide, or a relatively toxic gas.such as hydrogen sulfide. A solid forming reaction may enable the production of calcium oxide of cement while potentially reducing, or preventin g the co-production of carbon dioxide.

[1420] The aqueous alkaline earth cation - acid anion salt solution may be reacted with sulfur dioxide gas, or suifutous acid, or dissolved sulfur dioxide, or any combination thereof io produce, for example, an alkaline earth cation - sulfite anion salt and / or an acid. In some embodiments, the alkaline earth cation - sulfite may be produced mostly as a solid precipitate, while the acid may comprise an aqueous solution. For example, in some embodiments, the produced the alkaline earth cation ~ sulfite may comprise a solid which may be separated from the aqueous acid by a solid-liquid separation system or method. In some embodiments, residual dissolved alkaline earth cation - sulfite may be present in the aqueous acid. In. some embodiments, said residual dissolved alkaline earth cation - sulfite may remain present in the aqueous acid while, for example, the aqueous acid is recirculated or recycled in the process. In some embodiments, a portion of said residual dissolved alkaline earth cation - sulfite may be recovered or precipitated, using, for example, including, but not limited to, one or more or any combination of the following: cooling, or reverse osmosis concentrating. or nanofiltration concentration, or electrodialvsis. or eiectrodialvsis reversal, or precipitation, or evaporation. For example, in some embodiments employing calcium sulfite, calcium sulfite may be sufficiently insoluble where it may be less desirable or undesirable to recover residual dissolved calcium sulfite from the aqueous acid solution. For example, in some embodiments employing magnesium sulfite, magnesium sulfite may be sufficiently soluble where it may be desirable to recover residual dissolved magnesium sulfite from the aqueous acid solution,

[1421] In some embodiments, aqueous alkaline earth cation - acid anion salt solution may be reacted with a gas comprising sulfur dioxide to produce an alkaline earth cation — sulfite anion salt and an acid. In some embodiments, the alkaline earth cation — sulfite anion salt may comprise a solid. In some embodiments, the acid may comprise an aqueous solution. In some embodiments, sulfur dioxide gas may be at a dilute concentration in the gas comprising sulfur dioxide. In some embodiments, if the sulfur dioxide gas forms from the decomposition of calcium sulfite, it may be desirable for the concentration of sulfur dioxide gas to be dilute because, for example, the decomposition temperature and the decomposition rate may have a relationship with the concentration or partial pressure of sulfur dioxide gas formed, wherein, for example, the lower the concentration or partial, pressure of sulfurdioxide gas formed the higher the rate of calcium sulfite decomposition and / or the lower the required temperature to decompose the calcium sulfite. For example, in some embodiments, a dilute concentrarion of sulfiir dioxide gas may comprise a concentration lower than. lvol%, or 5vol%, or 10vol%, or 20vol%, or 30vol%, or 4()vol%, or S0vol%, or 60vol%, or 70vol%, or 80vol%, or 90vol%, or 100volH, or any combination thereof For example, in some embodiments, a dilute concentration of sulfur dioxide gas may comprise a sulfur dioxide gas partial pressure lower than (101 Bar, or 0,05 Bar, or 0.1 Bar, or 0.2 Bar, or 0.3 Bar, or 0.4 Bar, or 0.5 Bar, or 0.6 Bar, or 0.7 Bar, or 0.8 Bar, or 0.9 Bar, or 1 .0 Bar, or any combination thereof. In some embodiments, sulfur dioxide gas may be at a high concentration in the gas comprising sulfur dioxide. For example, in some embodiments, a high concentration of sulfur dioxide gas may comprise a concentration greater than 1 vol%, or 5vol%, or 10vol%, or 20vol%, or 30vol%, or 40vo1%, or 50vol%, or 60vol%, or 70vol%, or 80vol%, or 90vol%, or 100vol%, or any combination thereof. For example, in some embodiments, a high concentration of sulfur dioxide gas may comprise a. sulfur dioxide gas partial pressure greater than 0.01 Bar, or 0.05 Bar, or 0. 1 Bar, or 0.2 Bar, or 0.3 Bar, or 0.4 Bar, or 0.5 Bar, or 0.6 Bar, or 0.7 Bar, or 0.8 Bar, or 0,9 Bar, or 1.0 Bar, or 2.0 Bar, or 3.0 Bar, or 4.0 Bar, or 5.0 Bar, or any combination thereof.|'l '4221 In some embodiments, the reaction of a gas comprising sulfur dioxide with a solid or aqueous alkaline earth cation - acid anion salt may be conducted in a gas liquid contactor. For example, the reaction of a gas comprising sulfur dioxide wit h an aqueous alkaline earth cation - acid anion salt may be conducted in a gas-liquid contactor, which may include, but is not limited to, one or more or any combination of the following: an absorption column, or a spray tower* or bubble column, or a static mixer, or a mixer, or a sparger, or a membrane contactor, or packed column, or a plate column, or a disc column, or a column, or a precipitator, In some embodiments, it may be desirable for the reaction of a gas comprising sulfur dioxide with an aqueous alkaline earth cation - acid anion salt to be conducted in a reactor configured to handle precipitate or solid formation. For example, in some embodimen ts, it may be desirable for the reaction of a gas comprising sulfur dioxide with an aqueous alkaline earth cation - acid anion salt to be conducted in a bubble column or a sparger. In some embodiments, the formed alkaline earth sulfite, which may comprise a solid, may settle or may otherwise be separated by a solid-liquid separation from the aqueous acid solution. In some embodiments, the formed alkaline earth sulfite may settle within the reactor. In some embodiments, the formed alkaline earth sulfite may remain suspended withinthe reactor and / or may be separated from the aqueous acid solution after the mixture is transferred from the reactor. In sonic embodiments, the reactor may comprise a batch, or semi-batch, or continuous, or any combination thereof operation or configuration. In some embodiments, the solid phase formation reaction may enable fast reaction kinetics and / or high absorption or reaction efficiency due to, for example, the lack of accumulation of sul fur dioxide or sulfite ion in the aqueous phase. In some embodiments, an aqueous calcium acetate solation may be contacted with a gas comprise sulfur dioxide, which may result in the formation of solid calcium sulfite precipitate and an aqueous solution comprising acetic acid. The aqueous acetic acid may be separated from the solid calcium sulfite precipitate by a solid-liquid separation.

[1423] In some embodiments, the reaction of an alkaline earth cation - acid anion salt with sulfur dioxide may form an alkaline earth sulfite and an acid, wherein said formed acid may possess a vapor pressure. For exampie, the reaction of calcium acetate with sulfur dioxide may form calcium sulfite and acetic acid, wherein acetic acid may possess a vapor pressure. In some embodiments, it may be desirable io minimize or prevent losses of acid due to release of acid vapor, or carryover or slip of acid vapor, or any combination thereof• For example, in some embodiments, if a gas stream comprising sulfur dioxide comprises other gases or comprises dilute sulfur dioxide, acid vapor may be present in the remaining gases during or after the reaction of sulfur dioxide with an alkaline earth acid and the formation of acid and alkaline earth sulfite. For example, in some embodiments, as a dilute sulfur dioxide gas Is contacted with an alkaline earth acid, sulfur dioxide may react or absorb to form alkaline earth sulfite and / or an acid, wherein a portion of the formed acid may evaporate as acid vapor or acid vapor pressure into the remaining gases. In some embodiments, for example, it maybe desirable to design a sulfur dioxide absorption column or absorption process to contact a solution comprising alkaline earth acid with the gas lean In sulfur dioxide and rich in acid vapor. For example, in some embodiments, aqueous solution comprising alkaline earth acid entering an absorption process, which may not have substantially reacted with sulfur dioxide, may comprise little free acid or acid unreacted with alkaline earth or may comprise solution with the least, or near lowest, or lowest concentration or vapor pressure. For example, in some embodiments, a sulfur dioxide absorption may be configured such that first, a gas rich in sulfur dioxide and lean in acid vapor is contacted with a solution comprising alkaline earthacid to form alkaline earth sulfite and an aqueous solution comprising an acid and a gas lean in sulfur dioxide and rich in acid vapor, then, second, the gas lean in sulfur dioxide and rich in acid vapor may be contacted with solution comprising alkaline earth acid which is lean in aqueous acid or free acid, absorbing at least a portion of the acid vapor and forming a solu tion comprising alkaline earth acid relatively rich in aqueous acid or free acid and a gas lean in sulfur dioxide and lean in acid vapor For example, in some embodiments, an aqueous solution comprising alkaline earth acid .may be first contacted with a gas rich in acid vapor and lean in sulfur dioxide, which may result in the absorption of acid vapor and the formation of a solution comprising aqueous alkaline earth acid relatively rich in in dissolved acid or free acid; then, second, the aqueous alkaline earth acid relatively rich in absorbed acid or free acid may be contacted with a gas rich in sulfur dioxide and lean in acid vapor to form alkaline earth sulfite and a solution comprising aqueous acid. For example, some embodiments may utilize the inherently low concentration of acid, or low acid vapor pressure, or any combination thereof of some solutions comprising alkaline earth acid to absorb acid vapor. In some embodiments, it may be desirable to contact gas comprising acid vapor and / or absorb acid vapor into a solution comprising alkaline earth acid, for example, substantially before reacting the alkaline earth acid with sulfur dioxide because, for example, the reaction of alkaline earth acid with sulfur dioxide may produce acid or free acid and / or increase the solution’s acid vapor pressure. For example, in some embodiments, an aqueous solution comprising calcium acetate may be first contacted with a gas comprising remaining gases and / or acetic acid vapor, which may result in the formation of an aqueous solution comprising calcium acetate with dissolved or absorbed acetic acid vapor and / or a gas comprising remaining gases comprising a lower concentration of acetic acid vapor. For example, in some embodiments, the aqueous solution comprising calcium acetate with dissolved or absorbed acetic acid vapor may be then, second, contacted with a gas comprising sulfur dioxide, which may result in the formation of calcium sulfite and an aqueous solution comprising acetic acid. For example, in some embodiments, the aqueous solution comprising calcium may enter the process at the first step, then may be transferred into the second step, then may exit the process at or after the second step. For example, in some embodiments, the gas may enter theprocess at the second step, then may be transferred into the first step, then may exit the process at or after the first step. o For example, in. some embodiments, a sttifur dioxide absorption process with acid vapor recovery or removal may comprise an absorption column, wherein a higher elevation portion of the column, or the ‘top portion’, may comprise absorbing acid vapor into the alkaline acid salt solution to form alkaline acid salt solution with dissolved acid vapor, and then the lower elevation portion of the column, or ‘bottom portion', may comprise absorbing or reacting sulfur dioxide into the alkaline acid salt solution with dissolved acid vapor transferred from the higher elevation portion of the column. For example, in some . embodiments, a gas comprising sulfur dioxide may enter the absorption process in the bottom portion of the absorption column and / or the remaining gases after sulfur dioxide absorption may exit the top portion of the absorption column. o For example, in some embodiments, a sulfur dioxide absorption process with acid vapor recovery may comprise at least two absorption steps, comprising a first absorption step and a second absorption step. The first absorption step may be configured to absorb acid vapor slip or carryover. The second absorption step may be configured to absorb sulfur dioxide. An aqueous solution comprising an alkaline earth acid may enter the absorption process in the first absorption step, then may be transferred into the second absorption step, and then may exit the second absorption step as a solid comprising an alkaline earth sulfite and an aqueous solution comprising an acid. A gas comprising sulfur dioxide may enter the absorption process in the second absorption step, then may be transferred into the first absorption step, and then may exit the first absorption step as a gas lean in sulfur dioxide. In the second absorption step, a gas comprising sulfur dioxide may be reacted with an aqueous solution comprising an alkaline earth acid and absorbed acid vapor, wherein a solution comprising alkaline earth acid and absorbed acid vapor may enter the second absorption step and then exit as a solid comprising alkaline earth sulfite and an aqueous solution comprising an acid; and / or wherein a gas comprising sulfur dioxide may enter the second absorption step and then exit as a gas comprising remaining gases and acidvapor. In some embodiments, gas may enter the second absorption step near the bottom of the absorption step and / or I squid or solution may enter the second absorption step near the top of the absorption step. In the first, absorption step, a gas comprising remaining gases and acid vapor may be contacted with an aqueous solution comprising an alkaline earth acid, wherein a solution comprising alkaline earth acid may enter the first absorption step and exit as a solution comprising tin alkaline earth acid and absorbed acid vapor; and / or wherein a gas comprising remaining gases and acid vapor may enter the first absorption step and exit as a gas comprising remaining gases with a lower concentration of acid vapor. In some embodimen ts, gas may enter the first absorption step near the bo ttom of the absorption step and / or liquid or solution may enter the first absorption step near the top of the absorption column. In some embodiments, remaining gases may comprise unabsorbed gases, or gases remaining after absorption, or gases exiting an absorption process, or gases exiting an adsorption process, or any combination thereof,• For example, in some embodiments, alkaline earth acid may be reacted with high pressure, or high purity, or liquid, or aqueous, or solid, or any combination thereof sulfur dioxide. For example, in some embodiments, acid vapor release, or sl ip, or production may be prevented by employing, for example, high pressure, or high parity, or liquid, or aqueous, or solid, or any combination thereof sulfur dioxide in the reaction of alkaline earth acid with sulfur dioxide. For example, in some embodiments, by employing high pressure, or high, purity, or liquid, or aqueous, or solid, or any combination thereof sulfur dioxide in the reaction of alkaline earth acid and sulfur dioxide, a lower proportion of acid vapor may evaporate or form. In some embodiments, for example, an aqueous solution comprising calcium acetate may be reacted with liquid sulfur dioxide, which may result in the formation of a solid comprising calcium sulfite and an aqueous solution comprising acetic acid and / or minimal remaining gases, if any, into which a portion acetic acid may evaporate.• For example, in some embodiments, acid vapor may be removed or further removed from a gas comprising acid vapor, or acid vapor slip, or acid vapor carryover, or any combination thereof by, tor example, con tacting or reacting said gas with an alkali hydroxide, or alkali carbonate, alkali - weak acid or an alkaline earth oxide, oralkaline earth hydroxide, or alkaline earth carbonate, or alkaline earth - weak acid, or ammonium hydroxide, or ammonium carbonate, or a bicarbonate, or an ammonium weak acid, or any combination thereof t o form, for example, an alkali acid, or alkaline earth acid, or ammonium - acid, or any combination thereof. In some embodiments, alkali acid, or alkaline earth - acid, or ammonium - acid, or any combination thereof may be, for example, added to a process, or a process described herein employing alkali acid, or alkaline earth - acid, or ammonium - acid, or any combination thereof.» For example, in some embodiments, water produced or sourced without or with a low concentration of dissolved acid, or a low vapor pressure of acid, or a vapor pressure of acid lower than the vapor pressure of acid in a gas, or any combination thereof may be employed to absorb at least a portion of acid vapor from a gas. For example, in some embodiments, water added to the process as makeup water, or to makeup for water removed from the process in aqueous solutions exiting the process, or water added in the nature of process operations, or any combination thereof may be contacted with gas comprising acid vapor to remove or absorb at least a portion of acid vapor,• For example, in some embodiments, a portion of acid vapor may be recovered or absorbed by contacting remaining gases comprising acid vapor with a solvent with which the acid vapor is soluble. In some embodiments, it may be desirable for the solvent to enable or allow for the separation or regeneration of absorbed acid and / or solvent and / or may enable or allow for the separation of the acid from the solvent after absorption of the acid vapor into the solvent. In some embodiments, the solvent may comprise a liquid with a significantly lower vapor pressure, or significantly lower vapor pressure of the acid, or higher bailing point, or any comb ination thereof than the acid, or remaining gases comprising acid vapor, or any combination thereof. For example, in some embodiments, remaining gases comprising acid vapor comprising acetic acid may be contacted with a solvent comprising, including, but not limited to, one or more or any combination thereof: a glycol* or glycol ether, or glycol polymer* or glycol ether polymer, or an ester, or any combination thereof. For example, in some embodiments, it may be desirable for the absorbed acid to be regenerated or desorbed from the solvent by heating, or stripping, or steam stripping, or distillation, or fractional distillation. In someembodiments, it may be desirable to absorb acid vapor into water. In some embodiments, it may be desirable to absorb acid vapor into a solvent from which the acid may be separated by extractive distillation, or azeotropic distillation, or melt separation, or pressure swing, or electrical method, or other separation method described herein, or a separation method in the art. In some embodiments, it may be desirable to absorb acid vapor into a solvent from which the acid may be separated by a separation method described herein, or a separation method in the art, or any combination thereof. In some embodiments, it may be desirable to absorb and concentrate the acid in the solvent, which may result in a partially separated acid, or a concentrated acid solution.• For example, in some embodiments, acid vapor may be adsorbed to a solid or adsorbent with which the acid vapor has affinity. For example, in some embodiments, acid vapor may be adsorbed to a solid or adsorbent with which the acid vapor has affinity and from which the adsorbed acid may be separated. For example, in some embodiments, acid may be regenerated or separated from an adsorbent by heat, or stripping, or steam stripping, or electrical method, or pressure swing, or any combination thereof.• For example, in some embodiments, acid vapor may be separated or recovered, by cryogenic separation, or cooling, or condensing, or absorbing in a cooled solution, or liquefaction, or deposition, or any combination thereof.

[1424] In sonic embodiments, a solid or aqueous alkaline earth cation -- acid anion salt may be reacted with an aqueous solution comprising aqueous sulfur dioxide, or aqueous sulfurous acid, ar any combination thereof. In some embodiments, the aqueous sulfur dioxide, or aqueous sulfurous acid, or any combination thereof may comprise a solution comprising sulfur dioxide and water, with lower than 5wt% other chemicals. In some embodiment, the aqueous sulfur dioxide, or aqueous sulfurous acid, or any combination thereof may comprise a solution comprising sulfiir dioxide and water, with greater than 5wi% other chemicals. In some embodiments, the aqueous sulfur dioxide, or aqueous sulfurous acid, or any combination thereof may comprise a solution comprising aq ueous sulfur dioxide and another acid. For example, in some embodiments, the aqueous sulfur dioxide, or aqueous sulfurous acid, or any combination thereof may further comprise acetic acid. In some embodiments, an aqueous alkaline earth cation ••• acid anion salt may be reacted with an aqueous solution comprising aqueous sulfur dioxide, or aqueous sulfurous acid, or anycombination thereof, which may result in the formation of an alkaline earth sulfite, which may comprise a solid or solid precipitate, and an aqueous acid. The alkaline earth sulfite solidmay be separated from the aqueous acid in a solid-liquid separation. For example, a solution comprising calcium acetate may be reacted with an aqueous solution comprising sulfur dioxide, which may result in the formation of solid calcium sulfite and aqueous acetic acid. The aqueous acetic acid may be separated from the solid calcium sulfite by a solid-liquid separation. In some embodiments, the reactor may comprise a batch, or semi-batch, or continuous, or any combination thereof operation or configuration. In some embodiments, the acid may need to be further concentrated or waterremoved to make up for, for example, any water added or dilution of the acid during tire reaction with aqueous sulfur dioxide. In some embodiments, the acid formed from the reaction, or concentrating, or any combination thereof' may comprise an. aqueous solution, a solid, or a liquid, or any combination thereof.

[1425] In some embodiments, a solid or aqueous alkaline earth cation - acid anion salt may be reacted with liquid sulfur dioxide, or solid sulfur dioxide, or supercritical sulfur dioxide, or any combination thereof.

[1426] In some embodiments, a solid or aqueous alkaline earth cation ~ acid anion salt may be reacted with a solid or aqueous alkali sulfite. In some embodiments, a solid or aqueous alkaline earth cation - acid anion salt may be reacted with a solid or aqueous alkali sulfite, which may result in the formation of an alkaline earth sulfite, which may comprise a solid, and an alkali cation - acid anion salt, which may comprise an aqueous salt or dissolved salt. In some embodiments, an aqueous solution comprising alkali cation - acid anion salt may be separated from the alkaline earth sulfite solid using, for example, a solid-liquid separation. In some embodiments, the reaction may comprise mixing an aqueous solution comprising an alkali sulfite with an aqueous solution comprising an alkaline earth cation - acid anion salt, which may result in forming an alkaline earth sulfite precipitate. It may be desirable to conduct the reaction in a mixing reactor, or mixer, or continuous mixer, or continuous stirred reactor, or any combination thereof because, for example, the reaction may possess relatively fast reaction kinetics. The rate of solid formation, or the location of solid formation, or the rate of production of reaction products, or any combination thereof may be controlled due to, for example, the input reagents being at a liquid phase.

[1427] In some embodiments, it may be desirable to react the solution comprising an alkaline earth cation - acid anion salt with a salt comprising a sulfite. In some embodiments,it may be desirable to react the solution comprising an alkaline earth cation - acid anion salt with a salt comprising a sulfite because, for example, the absorption of sulfor dioxide gasmay be conducted at a gas or liquid phase and / or may be separate from a solid formation step, which may a void challenges related to solid handling in a gas absorbing environment. In some embodiments it may be desirable to react the solution comprising an alkaline earth cation - acid anion salt with a salt comprising a sulfite to enable fast reaction kinetics and / or easier or more controlled solid-liquid separation and / or faster solid-liquid separation. In some embodiments, a solution comprising an alkaline earth cation - acid anion salt may be reacted with an alkali sulfite, which may result in the formation of an alkaline earth sulfite and an alkali acid. In some embodiments, the alkaline earth sulfite which forms may comprise a solid.

[1428] In some embodiments, for example, an aqueous calcium acetate solution may be mixed with an aqueous sodium sulfite solution, or solid sodium sulfite, or any combination thereof, which may result in the formation of aqueous sodium acetate and solid calcium sulfite. Some embodiments may involve employing a cation or base which forms soluble salts with the sulfite and / or the acid. For example, some embodiments may employ ammonia or ammonium. In some embodiments, for example, an aqueous calcium acetate solution may be mixed with an aqueous ammonium sulfite solution, or solid ammonium sulfite, or any combination thereof, which may result, in the formation of solution comprising aqueous ammonium acetate and a solid comprising calcium sulfite.

[1429] In some embodiments, an alkaline earth sulfite may be thermally decomposed or thermally converted. In some embodiments, an alkaline earth sulfite may be thermally decomposed in an alkaline earth oxide and sulfiir dioxide gas. For example, in some embodiments, calcium sulfite may be thermally decomposed into calcium oxide and sulfor dioxide gas. For example, in some embodiments, calcium sulfite may, in the presence of Other raw mix materials, be thermally converted into clinker or cement. The thermal conversion or decomposition of an alkaline earth sulfite may be conducted hi, for example, a calciner or kiln. It may be desirable for the thermal conversion or decomposition to be conducted in a low oxygen environment, or to be eondueted at a desirable temperature range, or any combination thereof.

[1430] In some embodiments, alkaline earth sulfite may be wet, or comprise hydrated alkaline earth sulfite, or any combination thereof. In some embodiments, it may be desirableto dry, or dc*wet, or dehydrate, or any combination thereof the alkaline earth sulfite. For example, in some embodiments, alkaline earth oxide, which may be produced by the process, may be employed as a desiccant to indirectly dry or remove water from the alkaline earth sulfite and / or produce alkaline earth hydroxide. For example, In some embodimen ts, a gas. such as an inert gas or nitrogen gas, may be circulated between contacting the alkaline earth sulfite and the alkaline earth oxide, wherein, for example, water vapor and / or heat may be transferred from the alkaline earth sulfite to the alkaline earth oxide. In some embodiments, residual heat from the alkaline earth oxide and / or clinker may be employed to facilitate the drying of the alkaline earth sulfite. In some embodiments, waste heat may be employed facilitate the drying of the alkaline earth sulfite. In some embodiments, heat from the reaction of alkaline earth oxide and water to form alkaline earth hydroxide may be employed to facilitate the drying of the alkaline earth sulfite. In some embodiments, a kiln, or heater, or preheater, or any combination thereof, which may be desired to facilitate the dehydration of alkaline earth sulfite or the liberation of water from alkaline earth sulfite, may be employed to dry or dehydrate the alkaline earth sulfite. In some embodiments, a. heat pump may be employed to facilitate the drying of an alkaline earth sulfite. In some embodiments, it may be desirable to dry the alkaline earth sulfite in a low oxygen environment, to, for example, prevent or inhibit the oxidation of alkaline earth sul fite, or the formation of alkaline earth sulfate, or any combination thereof In some embodiments, the temperature of heat requited for dehydrating an alkaline earth sulfite may be substantially lower than the temperature of heat required to thermally decompose an alkaline earth sulfite into an alkaline earth oxide and sulfur dioxide. It may be desirable to employ potentially lower cost sources of beat or energy to dry and / or dehydrate alkaline earth sulfite. For example, it may be desirable to employ a heat pump, or waste heat, or solar heat, or recovered heat, or any combination (.hereof as a heat source or energy source for the thermal decomposition of an alkaline earth sulfite. t1431| In some embodiments, alkaline earth oxide may be reacted with water or water vapor to produce an alkaline earth hydroxide. For example, in some embodiments, the reaction of alkaline earth oxide with water may ...

Claims

CLAIMS1 . A process comprising: reacting a material comprising calcium carbonate with a solution comprising aqueous carboxylic acid to form a gas comprising carbon dioxide and a solution comprising aqueous calcium carboxylate; reacting the solution comprising aqueous calcium carboxylate with sodium sulfate to form a solution comprising aqueous sodium carboxylate and a solid comprising calcium sulfate; reacting the solution comprising aqueous sodium carboxylate with sulfur dioxide to form sodium sulfite and an aqueous carboxylic acid; separating said sodium sulfite from said aqueous carboxylic acid; reacting sodium sulfite to form a solid comprising calcium sulfite: and decomposing said calcium sulfite to form calcium oxide and sulfur dioxide.

2. The process of claim I wherein the reacting sodium sulfite to form a solid comprising calcium sulfite comprises: reacting the sodium sulfite with calcium hydroxide to form an aqueous solution comprising sodium hydroxide and a solid comprising calcium sulfite.

3. The process of claim 1 wherein the reacting sodium sulfite to form a solid comprising calcium sulfite comprises: first reacting calcium carbonate with carbon dioxide and water to form a solution comprising aqueous calcium bicarbonate; and then reacting the solution comprising aqueous calcium bicarbonate with sodium sulfite to form a solution comprising aqueous sodium bicarbonate and a solid comprising calcium sulfite.

4. The process of claim 3 which further comprises: decomposing said sodium bicarbonate to form sodium carbonate and carbon dioxide; reacting said calcium oxide with water to form calcium hydroxide; and reacting said sodium carbonate with said calcium hydroxide to form an aqueous solution comprising sodium hydroxide and a solid comprising calcium carbonate.

5. The process of claim 3 further comprising decomposing said sodium bicarbonate to form sodium carbonate and carbon dioxide.

6. The process of claim 5 further comprising reacting said sodium carbonate with calcium hydroxide to form an aqueous solution comprising sodium hydroxide and a solid comprising calcium carbonate.

7. The process of any one of claims 1, 2, or 3 which further comprising reacting calcium oxide with water to form calcium hydroxide.

8. The process of any one of claims .1 , 2, or 3 wherein said aqueous carboxylic acid is selected from formic acid, or acetic acid, or propanoic acid, or any mixture thereof9. The process of any one of claims 1 , 2, or 3 wherein said reacting the solution comprising aqueous sodium carboxylate with sulfur dioxide is conducted in an absorption column comprising a first stage and a second stage.

10. The process of any one of claims 1, 2, or 3 wherein at least a portion of the calcium oxide is reacted with carbon dioxide to form calcium carbonate. 1 1. A process comprising: reacting a material comprising calcium carbonate with a solution comprising aqueous carboxylic acid to form a gas comprising carbon dioxide and a solution comprising aqueous calcium carboxylate; reacting the solution comprising aqueous calcium carboxylate with sodium sulfite to form a solution comprising aqueous sodium carboxylate and a solid comprising calcium sulfite; decomposing said calcium sulfite to form calcium oxide and sulfur dioxide; reacting the solution comprising aqueous sodium carboxylate with sulfur dioxide to form sodium sulfite and carboxylic acid; separating at least a portion of said sodium sulfite from said aqueous carboxylic acid.

12. The process of claim 11 further comprising reacting calcium oxide wi th water to form calcium hydroxide.

13. The process of claim 11 or claim 12 further comprising capturing at least a portion of the carbon dioxide,14. The process of any one of claims .1 1, 12, or 13 wherein said carboxylic acid is selected from formic acid, or acetic acid, or propanoic acid, and said carboxylate is selected from formate, or acetate, or propanoate.

15. The process of any one of claims I I, .12, or 13 wherein said reacting the solution comprising aqueous sodium carboxylate with sulfur dioxide is conducted in an absorption column comprising a first stage arid a second stage.

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