Method for producing alkali hydroxides or alkaline earth oxides using weak acid intermediates

Abstract

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

Description

[Technical field]

[0001] CROSS-REFERENCE TO RELATED APPLICATIONS For PCT purposes, this application claims priority to U.S. Provisional Patent Application No. 63 / 342,870, filed May 17, 2022, which is incorporated herein by reference.

[0002] For U.S. purposes, this application claims priority to U.S. Provisional Application No. 63 / 342,870, filed May 17, 2022, which is incorporated herein by reference.

[0003] For U.S. purposes, this application also claims priority to pending U.S. patent application Ser. No. 18 / 087,432, which is a continuation of U.S. patent application Ser. No. 17 / 744,161, filed May 13, 2022, which issued as U.S. Patent No. 11,542,219 on January 3, 2023. U.S. Patent Application No. 17 / 744,161 is a continuation-in-part of U.S. Patent Application No. 17 / 732,808, filed April 29, 2022, which is a continuation-in-part of U.S. Patent Application No. 17 / 590,483, filed February 1, 2022, which is a continuation-in-part of U.S. Patent Application No. 17 / 243,714, filed April 29, 2021, which was patented as U.S. Patent No. 11,236,033, and U.S. Patent Application No. 17 / 243,714 is a continuation-in-part of U.S. Patent Application No. 16 / 944,850, filed July 31, 2020, which patented as U.S. Patent No. 11,034,619, which claims priority from U.S. Provisional Patent Application No. 62 / 895,557, filed September 4, 2019, U.S. Provisional Patent Application No. 63 / 042,397, filed June 22, 2020, and U.S. Provisional Patent Application No. 62 / 890,254, filed August 22, 2019. This application also claims priority to U.S. Provisional Patent Application No. 63 / 188,275, filed May 13, 2021.

[0004] The above-mentioned continuation application, U.S. Patent Application No. 17 / 590,483, filed February 1, 2022, also claims priority to U.S. Provisional Patent Application No. 63 / 147,286, filed February 9, 2021, U.S. Provisional Patent Application No. 63 / 153,461, filed February 25, 2021, U.S. Provisional Patent Application No. 63 / 157,847, filed March 8, 2021, U.S. Provisional Patent Application No. 63 / 163,993, filed March 22, 2021, and U.S. Provisional Patent Application No. 63 / 179,822, filed April 26, 2021. All of the above applications are incorporated herein by reference. [Background technology]

[0005] Sodium hydroxide is commonly produced using the chlor-alkali process, which is energy intensive, requires rare metal anodes and cathodes, has a limited market, and produces hydrochloric acid that cannot be discharged into the environment. Conventional sodium hydroxide production is energy intensive and CO 2 Furthermore, the production of sodium hydroxide by conventional techniques is energy intensive and CO 2 It is a CO2-intensive, expensive and environmentally harmful process. 2 or deoxidization or CO removal. 2 It cannot be added to the ocean for removal. Commercial uses of hydrochloric acid often involve its reaction with carbonates, which results in the formation of CO 2 This can lead to the release of CO 2 The benefits of reduced emissions may be negated. In addition, when hydrochloric acid is released into the environment, it reacts with carbonates or bicarbonates present in the environment, releasing carbon dioxide and acidifying bodies of water such as the oceans. Sodium hydroxide is an important chemical used in a wide range of applications, for example, in pulp and paper manufacturing, lithium processing, soap manufacturing, rayon manufacturing, and aluminum smelting. Conventional sodium hydroxide production is energy intensive and CO 2 Reducing the energy, costs and emissions associated with sodium hydroxide production would have significant economic and environmental benefits. It consumes less energy and produces less CO 2 There is a great need for a low-emission, environmentally friendly method for producing sodium hydroxide.

[0006] The production of calcium oxide or calcium hydroxide or cement clinker in the prior art is carried out using CO 2 Emissions generated and captured can be difficult or expensive. 2Emission-free and / or essentially high purity captured CO 2 It would be highly desirable to develop a process for producing calcium oxide or calcium hydroxide or cement clinker that produces

[0007] Some embodiments of the present invention may relate to low carbon emission, low energy consumption, or carbon negative production of sodium hydroxide, or sodium carbonate, or sodium bicarbonate, or sodium sulfite, or sodium bisulfite, or gypsum, or alkaline earth sulfates, or alkali hydroxides, or alkali carbonates, or alkali bicarbonates, or alkali sulfites. Some embodiments of the present invention relate to ultra-low CO2 production of sodium hydroxide with calcium sulfate as a by-product. 2 Calcium sulfate is solid, practically insoluble in water, non-toxic, non-hazardous to the environment, and has a multi-billion ton annual market for gypsum board, concrete aggregate, fireproofing, gypsum, building materials, and other applications. Some embodiments of the invention may be capable of emitting more than 1 billion tons of CO per year. 2 The present invention may be expandable to emissions reduction or carbon removal or a combination thereof. Some embodiments of the present invention may enable a highly scalable and environmentally beneficial system and method for ocean deacidification that can be expanded to significantly increase ocean pH, revitalize marine ecosystems, and permanently sequester carbon dioxide. Additionally, some embodiments may reduce the required cost and energy consumption of alkali hydroxides, carbonates, and bicarbonates. Some embodiments may employ equipment that includes abundant and recyclable materials.

[0008] Some embodiments of the present invention may relate to low carbon emission, 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 clinker, 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 relate to ultra-low CO2 production of calcium oxide, or magnesium oxide, or cement. 2 Some embodiments may enable CO 2 Capture process, or CO 2 Air Recovery Process, or CO 2 Removal process, or CO 2 Conversion process, or CO 2 A process for separating or extracting CO from a solution containing carbonates, or bicarbonates, or any combination thereof. 2 The process may include a method for recovering or separating the carbon dioxide from the calcium oxide. Some embodiments of the present invention may enable the production of calcium oxide or cement with the inherent production of high purity high pressure carbon dioxide, due to the nature of the process, which may reduce the cost and energy required to produce calcium oxide or cement with low or no emissions. Some embodiments may employ equipment that includes abundant and recyclable materials.

[0009] Advantages of some embodiments include lower energy consumption, lower cost or CO 2 Low emissions, CO 2 These include emission negative outputs, utilization for carbon dioxide removal, absence of strong acid products, abundance of materials, and global scalability. [Brief description of the drawings]

[0010] [Figure 1] A process for producing calcium oxide and recovered carbon dioxide using carboxylic acid and sulfur dioxide as intermediates. [Figure 2A] FIG. 2A is a process for producing calcium oxide and weak acid derivatives using carboxylic acids and sulfur dioxide as intermediates. [Figure 2B] FIG. 2B is a process for producing calcium oxide and weak acid derivatives using carboxylic acids and sulfur dioxide as intermediates. [Figure 3A] FIG. 3A is a process for producing magnesium oxide and weak acid derivatives using carboxylic acids and sulfur dioxide as intermediates. [Figure 3B] FIG. 3B is a process for producing magnesium oxide and weak acid derivatives using carboxylic acids and sulfur dioxide as intermediates. [Figure 4A] FIG. 4A is a process for producing alkaline earth oxides and recovered carbon dioxide using carboxylic acid, alkali, and sulfur dioxide as intermediates. [Figure 4B] FIG. 4B is a process for producing alkaline earth oxides and recovered carbon dioxide using carboxylic acid, alkali, and sulfur dioxide as intermediates. [Figure 4C] FIG. 4C is a process for producing alkaline earth oxides and recovered carbon dioxide using carboxylic acid, alkali, and sulfur dioxide as intermediates. [Figure 5A] FIG. 5A is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 5B] FIG. 5B is a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 5C] FIG. 5C is a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 5D] FIG. 5D is a process for the preparation of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 5E] FIG. 5E is a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 5F] FIG. 5F is a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 6A] FIG. 6A is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali and sulfur dioxide as intermediates. [Figure 6B] FIG. 6B is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkalis and sulfur dioxide as intermediates. [Figure 7A] FIG. 7A shows a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acid, alkali and sulfur dioxide as intermediates, with at least a portion of the alkali sulfite being separated by membrane. [Figure 7B] FIG. 7B shows a process for producing alkaline earth oxides and weak acid derivatives using carboxylic acid, alkali and sulfur dioxide as intermediates, with at least a portion of the alkali sulfite being separated by membrane. [Figure 8] The process for producing alkaline earth oxides and weak acid derivatives using carboxylic acid, alkali and sulfur dioxide as intermediates involves membrane separation of at least a portion of the alkali sulfite. [Figure 9A] FIG. 9A is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 9B] FIG. 9B is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 9C] FIG. 9C is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 9D] FIG. 9D is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10A] FIG. 10A is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10B] FIG. 10B is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10C] FIG. 10C is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10D] FIG. 10D is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10E] FIG. 10E is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 10F] FIG. 10F is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 11A] FIG. 11A is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 11B] FIG. 11B is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 11C] FIG. 11C is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 12A] FIG. 12A is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 12B] FIG. 12B is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 12C] FIG. 12C is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 13A]FIG. 13A is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid such as a carboxylic acid and sulfur dioxide as intermediates. [Figure 13B] FIG. 13B is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid such as a carboxylic acid and sulfur dioxide as intermediates. [Figure 13C] FIG. 13C is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid such as a carboxylic acid and sulfur dioxide as intermediates. [Figure 13D] FIG. 13D is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid such as a carboxylic acid and sulfur dioxide as intermediates. [Figure 13E] FIG. 13E is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid, such as a carboxylic acid, and sulfur dioxide as intermediates. [Figure 13F] FIG. 13F is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using an acid, such as a carboxylic acid, and sulfur dioxide as intermediates. [Figure 14A] FIG. 14A is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 14B] FIG. 14B is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 14C] FIG. 14C is a process for producing alkali carbonate and removing or capturing or converting CO2 from the alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Figure 15A] FIG. 15A is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 15B] FIG. 15B is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 15C] FIG. 15C is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 16A] FIG. 16A is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 16B] FIG. 16B is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 16C] FIG. 16C is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 17A] FIG. 17A is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 17B] FIG. 17B is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 17C] FIG. 17C is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 18] It is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 19]It is a process for the production of alkaline earth oxides and weak acid derivatives using carboxylic acids, alkali (such as ammonia or ammonium) and sulfur dioxide as intermediates. [Figure 20A] FIG. 20A is a process for producing or recovering ammonia from ammonium sulfate. [Figure 20B] FIG. 20B is a process for producing or recovering ammonia from ammonium sulfate. [Figure 20C] FIG. 20C is a process for producing or recovering ammonia from ammonium sulfate. [Figure 21A] FIG. 21A is a process for producing or recovering ammonia from ammonium sulfate. [Figure 21B] FIG. 21B is a process for producing or recovering ammonia from ammonium sulfate. [Figure 21C] FIG. 21C is a process for producing or recovering ammonia from ammonium sulfate. [Figure 22A] FIG. 22A is a process for producing or recovering ammonia from ammonium sulfate. [Figure 22B] FIG. 22B is a process for producing or recovering ammonia from ammonium sulfate. [Figure 22C] FIG. 22C is a process for producing or recovering ammonia from ammonium sulfate. [Figure 23A] FIG. 23A is a process for producing or recovering ammonia from ammonium sulfate. [Figure 23B] FIG. 23B is a process for producing or recovering ammonia from ammonium sulfate. [Figure 23C] FIG. 23C is a process for producing or recovering ammonia from ammonium sulfate. [Figure 24] A process in which alkaline earth sulfites are pyrolyzed or calcined to form alkaline earth oxides and sulfur dioxide, and / or the sulfur dioxide is absorbed using a recycled carrier gas, for example to enable the use of zero-emission heat and / or to enable low concentrations of diatomic oxygen. [Diagram 25] A process in which alkaline earth sulfites are pyrolyzed or calcined to form alkaline earth oxides and sulfur dioxide, and / or a recycled carrier gas is used to absorb the sulfur dioxide. [Figure 26A] FIG. 26A is a process for producing alkali hydroxide from alkali chloride using carboxylic acid and sulfur dioxide as intermediates. [Figure 26B] FIG. 26B is a process for producing alkali hydroxides from alkali chlorides using carboxylic acids and sulfur dioxide as intermediates. [Figure 26C] FIG. 26C is a process for producing alkali hydroxides from alkali chlorides using carboxylic acids and sulfur dioxide as intermediates. [Figure 26D] FIG. 26D is a process for producing alkali hydroxides from alkali chlorides using carboxylic acids and sulfur dioxide as intermediates. [Figure 27] This is a process for producing alkali sulfates from alkali chlorides and alkaline earth sulfates using ammonia and carbon dioxide as intermediates. [Figure 28A] FIG. 28A shows a process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide as intermediates. [Figure 28B] FIG. 28B shows a process for producing alkali sulfate from alkali chloride and alkaline earth sulfate using ammonia and carbon dioxide as intermediates. [Figure 28C] FIG. 28C shows a process for producing alkali sulfates from alkali chlorides and alkaline earth sulfates using ammonia and carbon dioxide as intermediates. [Figure 29] This process uses ammonia and carbon dioxide as intermediates, alkali chlorides and alkaline earth sulfates to produce alkali sulfates, and captures CO2. [Diagram 30]A process using alkali chlorides and alkaline earth sulfates to produce alkali sulfates with ammonia and carbon dioxide, capture CO2, and / or produce urea. [Figure 31A] FIG. 31A is a process for producing alkali hydroxide from alkali sulfite using acid and sulfur dioxide as intermediates. [Figure 31B] FIG. 31B is a process for producing alkali hydroxide from alkali sulfite using acid and sulfur dioxide as intermediates. [Figure 31C] FIG. 31C is a process for producing alkali hydroxide from alkali sulfite using acid and sulfur dioxide as intermediates. [Figure 32A] FIG. 32A is a process for absorbing or reacting sulfur dioxide in an alkali acid-anion, such as an alkali carboxylate, in a manner that can minimize or reduce potential residual vapors in the residual gas. [Figure 32B] FIG. 32B is a process for absorbing or reacting sulfur dioxide in an alkali acid-anion, such as an alkali carboxylate, in a manner that can minimize or reduce potential residual vapors in the residual gas. [Diagram 33] This is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates. [Diagram 34] This is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid, sulfur dioxide and carbon dioxide as intermediates. [Diagram 35] This is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid, sulfur dioxide and carbon dioxide as intermediates. [Figure 36A] It is a process for producing alkali hydrogen carbonates or carbonates from alkali sulfates using carboxylic acids and sulfur dioxide as intermediates and carbon dioxide as an input and intermediate. [Figure 36B] (As stated above.) [Figure 37]It is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid, magnesium, sulfur dioxide and carbon dioxide as intermediates. [Figure 38] It is a process for producing alkali hydroxide from alkali sulfate using carboxylic acid, magnesium, sulfur dioxide and carbon dioxide as intermediates. [Figure 39A] FIG. 39A is a process for producing alkali bicarbonate or carbonate from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates and carbon dioxide as an input and intermediate. [Figure 39B] FIG. 39B is a process for producing alkali bicarbonate or carbonate from alkali sulfate using carboxylic acid and sulfur dioxide as intermediates and carbon dioxide as an input and intermediate. DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

[0011] Example Chemistry Example 1: Manufacturing process of calcium oxide or cement or clinker (1) Reaction of materials containing calcium, or magnesium, or other alkaline earth-weak acid anions with acetic acid, which may include, but is not limited to, one or more of the following or any combination thereof: ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0012] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0013] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0014] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0015] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0016] (2) Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq)+H 2 O(l or aq) → CaSO 3 (s)+2CH 3 COOH(aq)

[0017] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0018] NOTE: In some embodiments, SO 2 (g) is SO 2 In addition to (g), other gases may be included. In some embodiments, SO 2 The residual gas after absorbing or reacting at least a portion of (g) may contain a certain amount of acetic acid vapor. In some embodiments, SO 2The residual gas after absorbing or reacting at least a portion of (g) may contain a certain amount of acetic acid vapor, which may include acetic acid evaporated from the product of reacting step "(2)". In some embodiments, the residual gas containing at least a portion of the acetic acid vapor may be a mixture of SO 2 (g) before reaction with Ca(CH 3 COO) 2 (aq), which converts at least a portion of the acetic acid vapor into Ca(CH 3 COO) 2 (aq) and / or can be removed from the residual gas. In some embodiments, acetic acid vapor can be removed from the residual gas using, for example, but not limited to, one or more of 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-aqueous suspension, or alkaline earth hydroxide-aqueous solution, or water, or alkali carbonate, or alkali bicarbonate, or alkali hydroxide, or any combination thereof.

[0019] NOTE: In some embodiments, the 2CH 3 Residual aqueous magnesium sulfite may be present in "2CHCOOH(aq)" that was transferred from reaction "(2)" to reaction "(1)". In some embodiments, the residual aqueous magnesium sulfite may be present in "2CHCOOH(aq)" that was transferred from reaction "(2)" to reaction "(1)". 3 In some embodiments, at least a portion of the aqueous magnesium sulfite solution may remain in the "2CHCOOH(aq)" that was transferred from reaction "(2)" to reaction "(1)". 3 Additional magnesium sulfite in solution beyond the solubility limit of magnesium sulfite may remain in solution as Ca(CH 3 COO) 2 (aq) or Mg(CH 3 COO) 2 (aq) and SO 2 (g or aq), or sulfite, or bisulfite, or any combination thereof, may be precipitated or co-precipitated during reaction with the sulfite.

[0020] NOTE: In some embodiments, the 2CH 3 Residual aqueous magnesium sulfite may be present in the "COOH(aq)". In some embodiments, a portion of the residual aqueous magnesium sulfite may be concentrated and / or separated using, but not limited to, one or more of heating, or cooling, or reverse osmosis, or a 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, where the pore size or characteristics of the membrane may allow for the permeation of at least a portion of the acetic acid and the rejection of at least a portion of the magnesium sulfite, and / or the resulting concentrated magnesium sulfite solution may be cooled to produce at least a portion of a magnesium sulfite precipitate.

[0021] (3) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0022] Note: "(3)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0023] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(3)”.

[0024] Example 2: Manufacturing process of magnesium oxide or cement or clinker (1) Reaction of materials containing calcium, magnesium, or other alkaline earth weak acid anions with acetic acid MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO)2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0025] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0026] NOTE: In some embodiments, the 2CH 3 COOH(aq) is a mixture of a certain amount of MgSO 3 (aq), which may contain residual MgSO 3 It is sometimes called (aq).

[0027] (2) Mg(CH 3 COO) 2 (aq)+SO 2 (g or aq)+H 2 O(l or aq) → MgSO 3 (s)+2CH 3 COOH(aq)

[0028] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0029] Note: 2CH 3 Residual MgSO in COOH(aq) solution 3 (aq) may be present.

[0030] (3) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0031] Note: "(3)" is MgSO, for which a kiln may be used.3 (s) baking.

[0032] Note: MgSO 3 (s) is dried or dehydrated, or both, before or during "(3)".

[0033] Example 3: Process for producing calcium oxide or cement or clinker using alkaline intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0034] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0035] Note: CO 2 (g) When CO is generated, 2 (g) High partial pressure CO 2 (g) or purity CO 2 CO generated or captured in (g) 2 It may be desirable to include (g).

[0036] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq) → 2NaCH 3 COO(aq)+CaSO 3 (s)

[0037] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0038] NOTE: In some embodiments, Na 2 SO 3 (s or aq) may comprise a solid containing sodium sulfite, which may be added to or dissolved in a solution containing calcium acetate.

[0039] NOTE: In some embodiments, Na 2 SO 3 (s or aq) may comprise an aqueous solution containing sodium sulfite and acetic acid.

[0040] (3) 2NACH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0041] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas.3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0042] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq or l)+Na 2 SO 3 (s)

[0043] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0044] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, thereby forming CH 3 A distillate or condensate containing COOH(aq) may result.

[0045] NOTE: In some embodiments, Na2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0046] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0047] NOTE: In some embodiments, the feed solution containing sodium sulfite and acetic acid can be distilled off, where a portion of the acetic acid and water vapor evaporates and / or condenses to form a separate acetic acid solution, and / or a remaining solution containing aqueous acetic acid and a higher concentration of sodium sulfite than the sodium sulfite concentration in the feed solution.

[0048] (5) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0049] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0050] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0051] NOTE: In some embodiments, SO 2 (g) NaCH 3 React with COO(aq) to give Na 2 SO 3 (aq) is formed, followed by Na 2 SO 3 Ca(CH 3 COO) 2 (aq) and CaSO 3 It may be preferable or desirable to form a fluororesin having a fluororesin structure such that the fluororesin structure has a fluororesin structure that is fluororesin-compatible with the fluororesin structure. This may be for example, but not limited to, one or more of the following potential advantages, or any combination thereof: In some embodiments, SO 2 It may be desirable to absorb (g) in an absorber tower. Deposit formation may be problematic in an absorber tower due to, for example and without limitation, the deposits clogging packing or plates, or impeding gas flow, or impeding liquid flow, or forming scaling, or any combination thereof. Ca(CH 3 COO) 2 (aq) and SO 2 (g) reacts with CaSO 3 Precipitates containing (s) may form, which may be problematic in some absorption towers or gas absorption processes. For example, Na 2 SO 3 can be dissolved in water, which may be desirable in an absorption tower, so NaCH 3 COO(aq) and SO 2 In the reaction with (g), the majority of the salt may remain in the aqueous or liquid phase throughout the reaction, if desired. In some embodiments, SO 2 (g) is SO 2 If gases are included in addition to (g), the acetic acid vapor is 2 May be present in the residual gas during or after the reaction of (g) with acetate. NaCH 3 COO(aq) and SO 2 When (g) comes into contact with the aqueous phase, this 2 SO3 (aq) and / or acetic acid, and the reactor or absorber is configured to form NaCH 3 The COO(aq) may be configured to absorb or recover at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) and SO 2 When (g) comes into contact with the aqueous phase, this 2 SO 3 (aq) and / or acetic acid, and the reactor or absorber may be 3 COO(aq) is SO 2 (g) NaCH entering the reactor or absorber before or during substantial reaction with 3 The COO(aq) may be configured to absorb or recover at least a portion of the acetic acid vapor from the residual gas. 3 By using COO(aq), residual SO that may be present in the residual gas 2 (g), which gives Ca(CH 3 COO) 2 (aq) is residual SO 2 This avoids possible solid formation or solid handling problems that may occur when reacting with (g). For example, in some embodiments, the ability of the reaction products to constitute an aqueous or pumpable phase may enable the design or configuration of an absorber tower, or absorber, or reactor, or any combination thereof, that can facilitate recovery of acetic acid vapor and / or reduce the potential amount or concentration of acetic acid vapor in the residue gas. For example, SO 2 (g) is a method for removing SO 2 from an absorber because it may be at a lean concentration or low partial pressure, or may comprise a gas mixture, or may improve the efficiency of absorption, or may facilitate the recovery or removal of any acid vapor from the residual gas, or may facilitate the recovery or removal of acetic acid vapor from the residual gas, or may eliminate, minimize, or reduce the concentration or partial pressure of acetic acid vapor in the residual gas, or any combination thereof. 2(g) may be desirable to absorb. For example, in some embodiments, the process used to decompose calcium sulfite into calcium oxide and sulfur dioxide may form a gas mixture containing sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in the gas mixture may be less than 1 atm, or less than 0.9 atm, or less than 0.8 atm, or less than 0.7 atm, or less than 0.6 atm, or less than 0.5 atm, or less than 0.4 atm, or less than 0.3 atm, or less than 0.2 atm, or less than 0.1 atm, or less than 0.05 atm, or any combination thereof, and / or the volume percent concentration of sulfur dioxide in the gas mixture may be less than 100%, or less than 90%, or less than 80%, or less than 70%, or less than 60%, or less than 50%, or less than 40%, or less than 30%, or less than 20%, or less than 10%, or less than 5%, or any combination thereof. Higher rate or efficiency of absorption. Solid-liquid separation can be made easier, more straightforward, or with higher yields. For example, in some embodiments, the formation and / or separation of precipitates can be more controllable when the rate of precipitation depends on the mixing of two liquids rather than on the precipitation reaction from a gas and a liquid.

[0052] Example 4: Manufacturing process of magnesium oxide or cement or clinker using alkaline intermediate (1) Reaction of calcium, magnesium, or other alkaline earth weak acid anions with acetic acid MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0053] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0054] Note: CO 2 (g) When CO is generated, 2 (g) High partial pressure CO 2 (g) or purity CO 2 CO generated or captured in (g) 2 It may be desirable to include (g).

[0055] (2) Mg(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq) → 2NaCH 3 COO(aq)+MgSO 3 (s)

[0056] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0057] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0058] (4)Na 2 SO 3 (aq)+2CH 3COOH(aq) → 2CH 3 COOH(aq or l)+Na 2 SO 3 (s)

[0059] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0060] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 In some embodiments, magnesium sulfite, if present, may be precipitated or crystallized prior to addition of Na 2 SO 3 This allows Na to precipitate or crystallize before 2 SO 3 This may allow for at least a partial separation of the magnesium sulfite from the

[0061] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0062] NOTE: In some embodiments, the CH 3 COOH is distilled off and / or condensed together with water vapor to form CH 3 A distillate or condensate containing COOH(aq) can be formed.

[0063] (5) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0064] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0065] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0066] NOTE: In some embodiments, SO 2 (g) NaCH 3 React with COO(aq) to give Na 2 SO 3 (aq) is formed, followed by Na 2 SO 3 Mg(CH 3 COO) 2 (aq) and MgSO 3 This may be preferred, for example and without limitation, due to one or more or any combination of the following potential advantages: In some embodiments, SO 2 It may be desirable to absorb Mg(CH)(g) in an absorber tower. Deposit formation may be problematic in an absorber tower due to, for example and without limitation, the deposits clogging packing or plates, or impeding gas flow, or impeding liquid flow, or forming scaling, or any combination thereof. 3 COO) 2 (aq) and SO 2 (g) reacts with MgSO 3Precipitates containing (s) may form, which may be problematic in some absorption towers or gas absorption processes. NaCH 3 COO(aq) and SO 2 The reaction with (g) can optionally remain in aqueous or liquid solution throughout the reaction. 2 SO 3 is soluble in water, which may be desirable in an absorber tower. For example, SO 2 (g) The absorption tower is designed to absorb SO because it may be at a dilute concentration, or at a low partial pressure, or constitute a gas mixture, or to improve absorption efficiency, or to facilitate recovery or removal of any acid vapors from the residual gas, or any combination thereof. 2 (g) may be desirable to absorb. For example, in some embodiments, the process used to decompose calcium sulfite into calcium oxide and sulfur dioxide may form a gas mixture containing sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in the gas mixture may be less than 1 atm, or less than 0.9 atm, or less than 0.8 atm, or less than 0.7 atm, or less than 0.6 atm, or less than 0.5 atm, or less than 0.4 atm, or less than 0.3 atm, or less than 0.2 atm, or less than 0.1 atm, or less than 0.05 atm, or any combination thereof, and / or the volume percent concentration of sulfur dioxide in the gas mixture may be less than 100%, or less than 90%, or less than 80%, or less than 70%, or less than 60%, or less than 50%, or less than 40%, or less than 30%, or less than 20%, or less than 10%, or less than 5%, or any combination thereof. In some embodiments, SO 2 (g) is SO 2 If gases are included in addition to (g), the acetic acid vapor is 2 SO may be present in the residual gas during or after the reaction of (g) with acetate. 2 (g) is NaCH 3When it comes into contact with COO(aq), this is the Na 2 SO 3 (aq) and / or acetic acid, and the reactor or absorber is configured to form NaCH 3 The COO(aq) may be configured to absorb or recover at least a portion of the acetic acid vapor from the residue gas. 2 (g) is NaCH 3 When it comes into contact with COO(aq), this is the Na 2 SO 3 (aq) and / or acetic acid, and the reactor or absorber may be 3 COO(aq) is SO 2 (g) NaCH entering the reactor or absorber before or during substantial reaction with 3 The COO(aq) may be configured to absorb or recover at least a portion of the acetic acid vapor from the residue gas. 3 By using COO(aq), residual SO that may be present in the residual gas 2 (g), which gives Ca(CH 3 COO) 2 (aq) is residual SO 2 This avoids possible solid formation or solid handling problems that may occur when reacting with (g). Higher rate or efficiency of absorption. Solid-liquid separation can be made easier or more straightforward or with higher yields. For example, the formation and / or separation of precipitates can be more controllable when the rate of precipitation depends on the mixing of two liquids rather than from a gas and a liquid.

[0067] Example 5: Calcium oxide or cement or clinker production process using alkaline intermediate with recycling separation process (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO)2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0068] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0069] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq)+CH 3 COOH(aq) → 2NaCH 3 COO(aq)+CH 3 COOH(aq)+CaSO 3 (s)

[0070] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0071] Note: CH 3 COOH(aq) and Na 2 SO 3 Na(aq) from membrane-based separation 2 SO 3 (aq) in the retentate 3 Since COOH(aq) is present, CH 3 COOH(aq) may be present.

[0072] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0073] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → Na 2 SO 3 (aq)+2CH 3 2CH different from COOH(aq) 3 COOH(aq)

[0074] Note: CH 3 A portion of the COOH(aq) can be separated using separation processes, such as membrane-based processes like reverse osmosis, to separate Na 2 SO 3 (aq). In some embodiments, CH 3 COOH(aq) may have a hydration radius or molar mass small enough to permeate the membrane, while the membrane is 2 SO 3 (aq) can be blocked. In some embodiments, Na 2 SO 3 (aq)+2CH 3 COOH(aq) is 2CH 3 The permeate containing COOH(aq) and Na 2 SO 3 (aq)+2CH 3 and a retentate containing COOH(aq).

[0075] (5) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0076] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0077] Note: CaSO3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0078] Example 6: Magnesium oxide or cement or clinker production process using alkaline intermediate with recycling separation process (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0079] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0080] (2) Mg(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq)+CH 3 COOH(aq) → 2NaCH 3 COO(aq)+CH 3 COOH(aq)+MgSO 3 (s)

[0081] Note: MgSO3 (s) can be separated using solid-liquid separation.

[0082] Note: CH 3 COOH(aq) and Na 2 SO 3 Na(aq) from membrane-based separation 2 SO 3 (aq) in the retentate 3 Since COOH(aq) is present, CH 3 COOH(aq) may be present.

[0083] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0084] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2Na 2 SO 3 (aq)+2CH 3 CH different from COOH(aq) 3 COOH(aq)

[0085] Note: CH 3 A portion of the COOH(aq) can be separated using separation processes, such as membrane-based processes like reverse osmosis, to separate Na 2 SO 3 (aq). In some embodiments, CH 3 COOH(aq) may have a hydration radius or molar mass small enough to permeate the membrane, while the membrane is 2 SO 3 (aq) can be blocked. In some embodiments, Na 2 SO 3 (aq)+2CH 3 COOH(aq) is 2CH 3 The permeate containing COOH(aq) and Na 2SO 3 (aq)+2CH 3 and a retentate containing COOH(aq).

[0086] (5) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0087] Note: "(5)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0088] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0089] Example 7: Preparation of sodium hydroxide from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(l or aq) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(l or aq) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g)+H 2 O(l or aq) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2O(l or aq)

[0090] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0091] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0092] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0093] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0094] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0095] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0096] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0097] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[0098] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0099] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0100] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0101] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0102] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0103] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0104] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0105] (5)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0106] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0107] Note: CaSO3 (s) can be separated using solid-liquid separation.

[0108] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0109] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0110] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0111] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0112] NOTE: In some embodiments, CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0113] NOTE: In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide. In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide, which may include combining step "(5)" and step "(7)".

[0114] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0115] (8) 2NaOH(aq or s) → 2NaOH(aq or s) + Water

[0116] NOTE: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution containing a higher mass percent concentration of NaOH.

[0117] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0118] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0119] Example 8: Production of sodium hydroxide from sodium sulfate using alkaline earth precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0120] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0121] (2) Mg(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+MgSO 4 (s or aq)

[0122] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0123] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0124] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0125] Note: Na 2 SO 3 is separated into CH 3The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0126] (5)Na 2 SO 3 (s or aq) + Mg(OH) 2 → (s or aq) 2NaOH (aq or s) + MgSO 3 (s)

[0127] Note: Mg(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0128] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0129] (6) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0130] Note: "(6)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0131] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0132] (7) MgO(s) + water (g or l or aq) → Mg(OH) 2 (s or aq)

[0133] Note: MgO(s) is MgSO 3 To remove water vapor before or during the decomposition of MgO(s) from Mg(s), or MgSO 3 It can be used to accelerate the drying of (s).

[0134] (8) 2NaOH(aq or s) → 2NaOH(s) + Water

[0135] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0136] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0137] Example 9: Preparation of sodium hydroxide from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0138] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0139] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0140] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0141] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0142] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0143] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0144] (5)Na 2 SO 3 (s or aq) + Mg(OH) 2 (s or aq) → 2NaOH(aq or s) + MgSO 3 (s or aq)

[0145] Note: Mg(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0146] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0147] (6) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0148] Note: "(6)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0149] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0150] (7) MgO(s) + water (g or l or aq) → Mg(OH) 2 (s or aq)

[0151] Note: MgO(s) is MgSO 3 To remove water vapor before or during the decomposition of MgO(s) from Mg(s), or MgSO 3 It can be used to accelerate the drying of (s).

[0152] (8) 2NaOH(aq or s) → 2NaOH(s) + water, or 2NaOH(aq) → 2NaOH(aq, more concentrated) + water

[0153] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0154] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0155] NOTE: Residual MgSO 3 (aq) may be present or dissolved in a solution containing NaOH(aq). In some embodiments, during the concentration of NaOH(aq) or during the removal of at least a portion of the water from NaOH(aq), residual MgSO 3 At least a portion of the MgSO may be precipitated or separated or recovered. For example, in some embodiments, 3 (aq) is less soluble in water than NaOH(aq). Separated or recovered MgSO 3 can be transferred to step (6), for example.

[0156] Example 10: Preparation of sodium carbonate from sodium sulfate using alkaline earth precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0157] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0158] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0159] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0160] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0161] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0162] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0163] (5)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0164] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0165] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0166] Note: In some embodiments, prior to step (5), Na 2 SO 3 (s) is dissolved in water to give Na 2 SO 3 (aq) can be formed. In some embodiments, water can be supplied from within the process, or water can be supplied from an external source, or any combination thereof. For example, if net water is consumed, or if water is in the sodium hydroxide or sodium carbonate product, or if water is in the product, or any combination thereof, it may be desirable to supply a portion of the water from an external source.

[0167] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0168] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0169] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0170] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0171] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0172] Note: In some embodiments, CaO is Na 2 SO 3 (s or aq) or an aqueous solution containing sodium sulfite. For example, in some embodiments, step "(5)" can be combined with step "(7)".

[0173] NOTE: In some embodiments, the water may be supplied from within the process, or the water may be supplied from an external source, or any combination thereof. For example, if net water is consumed, or if water is in the sodium hydroxide or sodium carbonate product, or if water is in the product, or any combination thereof, it may be desirable to supply a portion of the water from an external source.

[0174] (8) 2NaOH(aq or s)+CO 2 (g) → Na 2 CO 3 (s or aq)+H 2 O(l or aq or g)

[0175] NOTE: In some embodiments, CO 2may include gases having a dilute concentration of carbon dioxide, including, but not limited to, the CO 2 Source or CO 2 In some embodiments, NaOH(aq) can potentially be obtained from, for example, CO in air. 2 (g) and other very low CO 2 (g) A wide range of CO concentrations, including 2 (g) It can react with concentration.

[0176] NOTE: In some embodiments, NaOH (aq or s) is added to the ocean or sea, and CO in the ocean or air is added. 2 Or CO 2 It may react with derivative ions or species and / or increase the pH of the ocean.

[0177] Note: Na 2 CO 3 (s or aq) can be further reacted with carbon dioxide and / or water to form sodium bicarbonate.

[0178] Note: Na 2 CO 3 (s) can be precipitated and / or separated from the remaining solution. After precipitation, NaOH(s) can be added and / or dissolved in the remaining solution to form, e.g., Na 2 CO 3 It can replenish the sodium lost during the precipitation and separation of (s).

[0179] NOTE: In some embodiments, the "feed" solution to the concentration process may contain Na 2 CO 3 (aq) may be concentrated at high temperatures using energy-efficient concentration methods such as reverse osmosis or electrodialysis or heat recovery distillation, and / or the resulting concentrate or retentate may be cooled to a 2 CO 3 (s) can be partially precipitated. In some embodiments, Na 2 CO 3The remaining solution after precipitation and separation of (s) may be concentrated by removing Na prior to heating the combined solution and / or prior to concentrating the combined solution using an energy-efficient concentration method. 2 CO 3 (aq) may be mixed with the feed. In some embodiments, the water recovered during concentration, e.g., water permeate, or diluent, or condensate, may be, but is not limited to, one or more of: used to dissolve sodium sulfite to form aqueous sodium sulfite, or transferred to the reaction of calcium oxide with water to produce calcium hydroxide, or transferred to dissolve sodium sulfate, or any combination thereof.

[0180] Note: CaSO 3 SO derived from the burning of 2 (g) may be further concentrated, compressed, or purified.

[0181] Note: CaSO 3 SO derived from the burning of 2 (g) can be absorbed in water or an aqueous solution to form sulfurous acid or aqueous sulfur dioxide.

[0182] NOTE: A weak acid or weak acid anion may include an acid or acid anion having an acid strength less 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.

[0183] NOTE: A weak acid or weak acid anion can include an acid or acid anion that has a higher pKa than acetate, or carboxylate, or sulfite.

[0184] Note: Acetic acid is an example of an acid with an acid strength greater than that of a "weak acid" and less than that of sulfurous acid or aqueous sulfur dioxide.

[0185] Note: An example of an acid with a pKa lower than that of a "weak acid" and lower than that of sulfurous acid or aqueous sulfur dioxide is acetic acid.

[0186] Note: Exemplary alkaline earths can include calcium. Other alkaline earths, which can include beryllium (Be), or magnesium (Mg), or calcium (Ca), or strontium (Sr), or barium (Ba), or radium (Ra), or any combination thereof, can be used in place of or in addition to calcium.

[0187] Example 11: Process for producing calcium oxide or cement or clinker using ammonia intermediate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

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

[0189] Note: CO 2 (g) When CO is generated, 2 (g) High partial pressure CO 2 (g) or purity CO2 CO generated or captured in (g) 2 It may be desirable to include (g).

[0190] (2) Ca(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 3 (s or aq) → 2NH 4 CH 3 COO(aq)+CaSO 3 (s)

[0191] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0192] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0193] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+(NH 4 ) 2 SO 3 (s)

[0194] Note: CH 3 COOH is (NH 4 ) 2 SO 3 In some embodiments, the water can be removed and / or (NH 4 ) 2 SO 3may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a zero waste method described in the art, or a separation system or method described in the art, or any combination thereof.

[0195] NOTE: In some embodiments, (NH 4 ) 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, if present, at least a portion of the magnesium sulfite is (NH 4 ) 2 SO 3 In some embodiments, at least a portion of the magnesium sulfite may be replaced with (NH 4 ) 2 SO 3 It may be desirable to separate it from

[0196] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0197] (5) CaSO 3 →(s)CaO(s)+SO 2 (g)

[0198] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0199] Note: CaSO 3(s) may be dried or dehydrated, or both, before or during “(5)”.

[0200] NOTE: In some embodiments, SO 2 (g) NH 4 CH 3 React with COO(aq) (NH 4 ) 2 SO 3 (aq) is formed, followed by (NH 4 ) 2 SO 3 Ca(CH 3 COO) 2 (aq) and CaSO 3 It may be preferable to form (s) because of, for example and without limitation, one or more or any combination of the following potential advantages: In some embodiments, SO 2 It may be desirable to absorb (g) in an absorber tower. The formation of deposits may be problematic in an absorber tower due to, for example and without limitation, the deposits clogging packing or plates, or impeding gas flow, or impeding liquid flow, or forming scaling, or any combination thereof. Ca(CH 3 COO) 2 (aq) and SO 2 (g) reacts with CaSO 3 Precipitates containing (s) may form, which may be problematic in some absorber towers or gas absorption processes. NH 4 CH 3 COO(aq) and SO 2 The reaction with (g) can optionally remain in aqueous or liquid solution throughout the reaction. 4 ) 2 SO 3 is soluble in water, which may be desirable in an absorber tower. For example, SO 2(g) The SO 2 gas may be present in the absorber because it may be at a dilute concentration, or at a low partial pressure, or may form a gas mixture, or may improve the absorption efficiency, or any combination thereof. 2 (g) may be desirable to absorb. For example, in some embodiments, the process used to decompose calcium sulfite into calcium oxide and sulfur dioxide may form a gas mixture containing sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in the gas mixture may be less than 1 atm, or less than 0.9 atm, or less than 0.8 atm, or less than 0.7 atm, or less than 0.6 atm, or less than 0.5 atm, or less than 0.4 atm, or less than 0.3 atm, or less than 0.2 atm, or less than 0.1 atm, or less than 0.05 atm, or any combination thereof, and / or the volume percent concentration of sulfur dioxide in the gas mixture may be less than 100%, or less than 90%, or less than 80%, or less than 70%, or less than 60%, or less than 50%, or less than 40%, or less than 30%, or less than 20%, or less than 10%, or less than 5%, or any combination thereof. Higher rate or efficiency of absorption. Solid-liquid separation can be made easier or more straightforward or with higher yields. For example, the formation and / or separation of precipitates can be more controllable when the rate of precipitation depends on the mixing of two liquids rather than from a gas and a liquid.

[0201] Example 12: Process for the production of alkaline earth oxides or cement or clinker using ammonia intermediate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0202] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0203] Note: CO 2 (g) When CO is generated, 2 (g) High partial pressure CO 2 (g) or purity CO 2 CO generated or captured in (g) 2 It may be desirable to include (g).

[0204] (2) Mg(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 3 (s or aq) → 2NH 4 CH 3 COO(aq)+MgSO 3 (s)

[0205] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0206] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2SO 3 (aq)+2CH 3 COOH(aq)

[0207] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+(NH 4 ) 2 SO 3 (s)

[0208] Note: CH 3 COOH is (NH 4 ) 2 SO 3 In some embodiments, the water can be removed and / or (NH 4 ) 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0209] NOTE: In some embodiments, (NH 4 ) 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is (NH 4 ) 2 SO 3 Precipitation or crystallization may begin before .

[0210] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3COOH(aq), and the solid-liquid separation can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0211] (5) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0212] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0213] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0214] NOTE: In some embodiments, SO 2 (g) NH 4 CH 3 React with COO(aq) (NH 4 ) 2 SO 3 (aq) is formed, followed by (NH 4 ) 2 SO 3 Mg(CH 3 COO) 2 (aq) and MgSO 3 It may be preferable to form (s) because of, for example and without limitation, one or more or any combination of the following potential advantages: In some embodiments, SO 2 It may be desirable to absorb Mg(CH)(g) in an absorber tower. The formation of deposits may be problematic in an absorber tower due to, for example and without limitation, the deposits clogging packing or plates, or impeding gas flow, or impeding liquid flow, or forming scaling, or any combination thereof. 3 COO) 2(aq) and SO 2 (g) reacts with MgSO 3 Precipitates containing (s) may form, which may be problematic in some absorber towers or gas absorption processes. NH 4 CH 3 COO(aq) and SO 2 The reaction with (g) can optionally remain in aqueous or liquid solution throughout the reaction. 2 SO 3 is soluble in water, which may be desirable in an absorber tower. For example, SO 2 (g) The SO 2 gas may be present in the absorber because it may be at a dilute concentration, or at a low partial pressure, or may form a gas mixture, or may improve the absorption efficiency, or any combination thereof. 2 (g) may be desirable to absorb. For example, in some embodiments, the process used to decompose calcium sulfite into calcium oxide and sulfur dioxide may form a gas mixture containing sulfur dioxide. For example, in some embodiments, the partial pressure of sulfur dioxide in the gas mixture may be less than 1 atm, or less than 0.9 atm, or less than 0.8 atm, or less than 0.7 atm, or less than 0.6 atm, or less than 0.5 atm, or less than 0.4 atm, or less than 0.3 atm, or less than 0.2 atm, or less than 0.1 atm, or less than 0.05 atm, or any combination thereof, and / or the volume percent concentration of sulfur dioxide in the gas mixture may be less than 100%, or less than 90%, or less than 80%, or less than 70%, or less than 60%, or less than 50%, or less than 40%, or less than 30%, or less than 20%, or less than 10%, or less than 5%, or any combination thereof. Higher rate or efficiency of absorption. Solid-liquid separation can be made easier or more straightforward or with higher yields. For example, the formation and / or separation of precipitates can be more controllable when the rate of precipitation depends on the mixing of two liquids rather than from a gas and a liquid.

[0215] Example 13: Calcium oxide or cement or clinker production process using ammonia intermediate with recycle separation (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0216] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0217] (2) Ca(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 3 (s or aq)+CH 3 COOH(aq) → 2NH 4 CH 3 COO(aq)+CH3 COOH(aq)+CaSO 3 (s)

[0218] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0219] Note: CH 3 COOH(aq) and (NH 4 ) 2 SO 3 (NH) from membrane-based separation of (aq) 4 ) 2 SO 3 (aq) in the retentate solution. 3 Since COOH(aq) is present, CH 3 COOH(aq) may be present.

[0220] (3)2(NH 4 )CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0221] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 2CH different from COOH(aq) 3 COOH(aq)

[0222] Note: CH 3 A portion of the COOH(aq) can be separated using a separation process, such as a membrane-based process like reverse osmosis, to produce (NH 4 ) 2 SO 3 (aq). In some embodiments, CH 3COOH(aq) may have a hydration radius or molar mass small enough to permeate the membrane, while the membrane may be too small to accommodate (NH 4 ) 2 SO 3 (aq) can be blocked. In some embodiments, (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) is 2CH 3 The permeate containing COOH(aq) and (NH 4 ) 2 SO 3 (aq)+2CH 3 and a retentate containing COOH(aq).

[0223] (5) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0224] Note: "(5)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0225] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(5)”.

[0226] Example 14: Process for the production of alkaline earth oxides or cement or clinker using ammonia intermediate with recycle separation (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0227] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0228] (2) Mg(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 3 (s or aq)+CH 3 COOH(aq) → 2NH 4 CH 3 COO(aq)+CH 3 COOH(aq)+MgSO 3 (s)

[0229] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0230] Note: CH 3 COOH(aq) and (NH 4 ) 2 SO 3 (NH) from membrane-based separation of (aq) 4 ) 2 SO 3 (aq) in the retentate 3 Since COOH(aq) is present, CH 3 COOH(aq) may be present.

[0231] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 )2 SO 3 (aq)+2CH 3 COOH(aq)

[0232] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 2CH different from COOH(aq) 3 COOH(aq)

[0233] Note: CH 3 A portion of the COOH(aq) can be separated using a separation process, such as a membrane-based process like reverse osmosis, to produce (NH 4 ) 2 SO 3 (aq). In some embodiments, CH 3 COOH(aq) may have a hydration radius or molar mass small enough to permeate the membrane, while the membrane may be too small to accommodate (NH 4 ) 2 SO 3 (aq) can be blocked. In some embodiments, (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) is 2CH 3 The permeate containing COOH(aq) and (NH 4 ) 2 SO 3 (aq)+2CH 3 and a retentate containing COOH(aq).

[0234] (5) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0235] Note: "(6)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0236] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0237] Example 15: Precipitation of calcium and production of ammonia from ammonium sulfate using acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0238] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0239] (2) Ca(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 4 (aq) → 2NH 4 CH 3 COO(aq)+CaSO 4 (s)

[0240] (3) 2NH 4 CH 3COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0241] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq or l) + (NH 4 ) 2 SO 3 (s)+water

[0242] Note: CH 3 COOH is (NH 4 ) 2 SO 3 In some embodiments, the water can be removed and / or (NH 4 ) 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0243] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0244] (5)(NH 4 ) 2 SO 3 (s or aq) + Ca(OH) 2(s or aq) → [2NH 4 OH(aq) or 2NH 3 (aq)]+CaSO 3 (s)

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

[0246] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0247] Note: 2NH 3 (aq) may be separated into ammonia gas and water as required.

[0248] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0249] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0250] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0251] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0252] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0253] (8)2NH 4 OH(aq) or 2NH 3 (aq) → 2NH 3 (g or l or aq) + water

[0254] NOTE: In some embodiments, it may be desirable to generate ammonia gas or liquid ammonia. In some embodiments, it may be desirable to generate high or higher concentration aqueous ammonia or ammonium hydroxide solutions.

[0255] NOTE: In some embodiments, 2NH 4 OH(aq) or 2NH 3 It may be desirable for (aq) to comprise an aqueous solution, for example in some embodiments it may be desirable to keep aqueous ammonia or ammonium hydroxide in the aqueous phase.

[0256] Example 16: Production of ammonia from ammonium sulfate using alkaline earth precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g) Magnesium silicate(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + silicon dioxide (s) MgS(s)+2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+H 2 S(g) Magnesium (weak acid anion) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0257] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0258] (2) Mg(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 4 (aq) → 2NH 4 CH 3 COO(aq)+MgSO 4 (s or aq)

[0259] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0260] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+(NH 4 ) 2 SO 3 (s)

[0261] Note: CH 3 COOH is (NH 4 ) 2 SO 3 In some embodiments, the water can be removed and / or (NH 4 ) 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0262] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0263] (5)(NH 4 ) 2 SO 3 (s or aq) + Mg(OH) 2 (s or aq) → [2NH 4 OH(aq) or 2NH 3 (aq)]+MgSO 3 (s)

[0264] Note: Mg(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0265] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0266] Note: 2NH 3 (aq) may be separated into ammonia gas and water as required.

[0267] (6) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0268] Note: "(6)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0269] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0270] (7) MgO(s) + water (g or l or aq) → Mg(OH) 2 (s or aq)

[0271] Note: MgO(s) is MgSO3 To remove water vapor before or during the decomposition of MgO(s) from Mg(s), or MgSO 3 It can be used to accelerate the drying of (s).

[0272] (8)2NH 4 OH(aq) or 2NH 3 (aq) → 2NH 3 (g or l or aq) + water

[0273] NOTE: In some embodiments, it may be desirable to generate ammonia gas or liquid ammonia. In some embodiments, it may be desirable to generate high or higher concentration aqueous ammonia or ammonium hydroxide solutions.

[0274] NOTE: In some embodiments, 2NH 4 OH(aq) or 2NH 3 It may be desirable for (aq) to comprise an aqueous solution, for example in some embodiments it may be desirable to keep aqueous ammonia or ammonium hydroxide in the aqueous phase.

[0275] Example 17: Production of ammonia from ammonium sulfate using alkaline earth precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0276] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0277] (2) Ca(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 4 (aq) → 2NH 4 CH 3 COO(aq)+CaSO 4 (s)

[0278] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0279] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+(NH 4 ) 2 SO 3 (s)

[0280] Note: CH 3 COOH is (NH 4 ) 2 SO 3 In some embodiments, the water can be removed and / or (NH 4 ) 2 SO 3may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0281] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0282] (5)(NH 4 ) 2 SO 3 (s or aq) + Mg(OH) 2 (s or aq) → [2NH 4 OH(aq) or 2NH 3 (aq)]+MgSO 3 (s or aq)

[0283] Note: Mg(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0284] Note: MgSO 3 (s) can be separated using solid-liquid separation.

[0285] Note: 2NH 3 (aq) may be separated into ammonia gas and water as required.

[0286] (6) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0287] Note: "(6)" is MgSO, which may be kiln-fired. 3 (s) baking.

[0288] Note: MgSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0289] (7) MgO(s) + water (g or l or aq) → Mg(OH) 2 (s or aq)

[0290] Note: MgO(s) is MgSO 3 To remove water vapor before or during the decomposition of MgO(s) from Mg(s), or MgSO 3 It can be used to accelerate the drying of (s).

[0291] (8)2NH 4 OH(aq) or 2NH 3 (aq) → 2NH 3 (g or l or aq) + water

[0292] NOTE: In some embodiments, it may be desirable to generate ammonia gas or liquid ammonia. In some embodiments, it may be desirable to generate high or higher concentration aqueous ammonia or ammonium hydroxide solutions.

[0293] NOTE: In some embodiments, 2NH 4 OH(aq) or 2NH 3 It may be desirable for (aq) to comprise an aqueous solution, for example in some embodiments it may be desirable to keep aqueous ammonia or ammonium hydroxide in the aqueous phase.

[0294] Example 18: Preparation of Ammonium Carbonate or Ammonium Bicarbonate or Ammonium Carbamate or Urea Using Acid Intermediate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0295] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0296] (2) Ca(CH 3 COO) 2 (aq)+(NH 4 ) 2 SO 4 (aq) → 2NH 4 CH 3 COO(aq)+CaSO 4 (s)

[0297] (3) 2NH 4 CH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → (NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq)

[0298] (4)(NH 4 ) 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+(NH 4 )2 SO 3 (s)

[0299] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0300] Note:(NH 4 ) 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0301] (5)(NH 4 ) 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → [2NH 4 OH(aq) or 2NH 3 (aq)]+CaSO 3 (s)

[0302] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0303] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0304] (6) CaSO 3 (s) → CaO(s) + SO2 (g)

[0305] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0306] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0307] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0308] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0309] (8)2NH 4 OH(aq)+CO 2 (g) → (NH 4 ) 2 CO 3 (s or aq)+H 2 O(l or aq or g)

[0310] NOTE: In some embodiments, (NH 4 ) 2 CO 3 (s or aq) can be further reacted with carbon dioxide and / or water to form sodium bicarbonate.

[0311] NOTE: In some embodiments, the aqueous solution may include a mixture of ammonium carbonate, or ammonium bicarbonate, or ammonium carbamate, or ammonium sesquicarbonate, or free ammonia, or aqueous ammonia, or ammonium hydroxide, or any combination thereof.

[0312] Example 19: Direct Air Capture, or CO from Air 2or CO using alkaline earths, sulfur dioxide and acids 2 Collection of (1) Reaction of alkaline earth oxides, or alkaline earth hydroxides, or any combination thereof, with carbon dioxide. CaO(s)+CO 2 (g) → CaCO 3 (s), and / or Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O(g or l)

[0313] (2) CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)

[0314] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0315] (3) Ca(CH 3 COO) 2 (aq)+SO 2 (g) → CaSO 3 (s)+2CH 3 COOH(aq)

[0316] NOTE: In some embodiments, SO 2 (g) is a dilute SO 2 (g) may constitute a gas.

[0317] (4) CaSO 3 →(s)CaO(s)+SO 2 (g)

[0318] (5) CaO(s)+H 2 O(l or g) → Ca(OH) 2 (s or aq)

[0319] Example 20: Direct Air Capture, or CO from Air 2 or CO using alkaline earths, sulfur dioxide and acids 2 Collection of (1) Reaction of alkaline earth oxides, or alkaline earth hydroxides, or any combination thereof, with carbon dioxide. MgO+CO 2 (g) → MgCO 3 (s), and / or Mg(OH) 2 (s or aq)+CO 2 (g) → MgCO 3 (s)+H 2 O(g or l)

[0320] (2) MgCO 3 (s or aq) + 2CH 3 COOH(aq) → Mg(CH 3 COO) 2 (aq)+CO 2 (g)

[0321] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0322] (3) Mg(CH 3 COO) 2 (aq)+SO 2 (g) → MgSO 3 (s)+2CH 3 COOH(aq)

[0323] NOTE: In some embodiments, SO 2 (g) is a dilute SO 2 (g) may constitute a gas.

[0324] (4) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0325] (5) MgO(s)+H 2 O(l or g) → Mg(OH) 2 (s or aq)

[0326] Example 21: Direct Air Capture, or CO from Air 2 CO recovery using alkali, alkaline earth and sulfur dioxide 2 Collection of (1) 2NaOH(aq) + CO 2 (g) → Na 2 CO 3 (aq or s) + H 2 O(g or l)

[0327] (2)Na 2 CO 3 (aq or s) + SO 2 (l or aq) → Na 2 SO 3 (aq or s) + CO 2 (g)

[0328] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0329] (3)Na 2 SO 3 (aq or s) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaSO 3 (s)

[0330] (4) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0331] (5) CaO(s)+H 2 O(l or g) → Ca(OH) 2 (s or aq)

[0332] Example 22: Direct Air Capture, or CO from Air 2 or CO2 recovery using alkali, alkaline earth and sulfur dioxide 2 Collection of (1) 2NaOH(aq) + CO 2 (g) → Na 2 CO 3(aq or s) + H 2 O(g or l)

[0333] (2)Na 2 CO 3 (aq or s) + SO 2 (l or aq) → Na 2 SO 3 (aq or s) + CO 2 (g)

[0334] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0335] (3)Na 2 SO 3 (aq or s) + Mg(OH) 2 (s or aq) → 2NaOH(aq) + MgSO 3 (s)

[0336] (4) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0337] (5) MgO(s)+H 2 O(l or g) → Mg(OH) 2 (s or aq)

[0338] Example 23: Direct Air Capture, or CO from Air 2 or CO2 recovery using alkali, alkaline earth and sulfur dioxide 2 Collection of (1) 2NaOH(aq) + CO 2 (g) → Na 2 CO 3 (aq or s) + H 2 O(g or l)

[0339] (2)Na 2 CO 3 (aq or s) + 2CH 3 COOH(l or aq) → 2NaCH 3 COO(aq)+CO 2 (g)

[0340] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0341] (3) 2NaCH 3 COO(aq)+SO 2 (g) → Na 2 SO 3 (aq or s) + 2CH 3 COOH(aq)

[0342] NOTE: In some embodiments, SO 2 (g) is a dilute SO 2 (g) may constitute a gas.

[0343] (4) 2CH 3 Na from COOH 2 SO 3 Separation

[0344] (5)Na 2 SO 3 (aq or s) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaSO 3 (s)

[0345] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0346] (7) CaO(s)+H 2 O(l or g) → Ca(OH) 2 (s or aq)

[0347] Example 24: Direct Air Capture, or CO from Air 2 or CO2 recovery using alkali, alkaline earth and sulfur dioxide 2 Collection of (1) 2NaOH(aq) + CO 2 (g) → Na 2 CO 3 (aq or s) + H 2 O(g or l)

[0348] (2)Na 2 CO 3 (aq or s) + 2CH 3 COOH(l or aq) → 2NaCH 3 COO(aq)+CO 2 (g)

[0349] Note: CO in (2) 2 (g) is the captured CO 2 (g) may be included.

[0350] (3) 2NaCH 3 COO(aq)+SO 2 (g) → Na 2 SO 3 (aq or s) + 2CH 3 COOH(aq)

[0351] NOTE: In some embodiments, SO 2 (g) is a dilute SO 2 (g) may constitute a gas.

[0352] (4) 2CH 3 Na from COOH 2 SO 3 Separation

[0353] (5)Na 2 SO 3 (aq or s) + Mg(OH) 2 (s or aq) → 2NaOH(aq) + MgSO 3 (s)

[0354] (6) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0355] (7) MgO(s)+H 2 O(l or g) → Mg(OH) 2 (s or aq)

[0356] Example 25: Separated CO 2 CO absorption or adsorption2 Recovery of CO 2 Desorption or release of and regeneration of reagents (1)CO 2 Absorption of CO 2 can be absorbed or adsorbed onto calcium oxide, or calcium hydroxide, or a calcium hydroxide suspension such as milk of lime, or any combination thereof to produce a calcium carbonate solid or suspension. Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O(l or g)

[0357] NOTE: The calcium hydroxide suspension can be transported to the absorption site and / or stored at or near the absorption site.

[0358] NOTE: The calcium carbonate solids can be separated by sedimentation, or solid-liquid separation, or any combination thereof.

[0359] NOTE: Calcium carbonate can be stored at or near the site of absorption or adsorption. It can be transported to an application where it is used. Calcium carbonate is 2 In some embodiments, the CO 2 The site of desorption or release of CO 2 In some embodiments, the CO 2 The site of desorption or release of CO 2 For example, in some embodiments, the location of absorption or adsorption of CO 2 It may be desirable for absorption or adsorption to be located at multiple distributed sites, while regeneration may occur at a larger and / or more centralized facility or site.

[0360] (2)CO 2 Desorption or release of: Calcium carbonate can react with acetic acid to produce calcium acetate and carbon dioxide. CaCO 3 (s)+2CH 3 COOH→Ca(CH 3 COO) 2 (aq)+CO 2 (g) Note: Calcium carbonate is CO 2 The substance may be stored at or near the site of desorption or release. Note: Acetic acid is CO 2 The substance may be stored at or near the site of desorption or release. ·Note: CO 2 The desorption or release of CO can be deployed in applications requiring carbon dioxide, or high purity carbon dioxide, or high pressure carbon dioxide, or recovered carbon dioxide, or any combination thereof. For example, 2 The desorption or release of CO 2 The system can be deployed in locations requiring enhanced oil recovery (EOR) through the use of sulphuric acid. NOTE: Calcium acetate may include an aqueous calcium acetate solution, or solid calcium acetate, or any combination thereof. Note: Calcium acetate is CO 2 The calcium acetate can be stored at or near the site of desorption or release of CO. The calcium acetate can be transported to an application that uses the calcium acetate. The calcium acetate can be transported to or near the site of regeneration. In some embodiments, the calcium acetate can be stored at or near the site of CO 2 The location of desorption or release of CO may be the same as the location of regeneration. 2 The location of desorption or release of CO may be different from the location of regeneration. For example, in some embodiments, 2 It may be desirable for the desorption or release of to be located at multiple distributed sites, while regeneration may occur at a larger and / or more centralized facility or site. ·Note: CO 2 Acetic acid vapor may be present in (g). In some embodiments, the acetic acid vapor may be present in, for example, but not limited to, CO 2 (g) CaCO 3 or CO containing a certain amount of acetic acid vapor. 2(g) with sodium carbonate or CO containing a certain amount of acetic acid vapor. 2 CO2(g) can be at least partially removed from CO2(g), such as by contacting (g) with an alkali carbonate, or by one or more of compression, or cooling, or condensation, or cryogenic separation, or freeze separation, or any combination thereof.

[0361] (3) Regeneration: Calcium acetate can react with sulfur dioxide to produce calcium sulfite. Calcium sulfite can be converted to calcium oxide and sulfur dioxide. Calcium oxide can react with water to form calcium hydroxide suspensions such as milk of lime. Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq) → CaSO 3 (s)+2CH 3 COOH(aq) CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0362] Note: Calcium oxide or calcium hydroxide is CO 2 The ions can be transported to a site of absorption or adsorption.

[0363] NOTE: Acetic acid is CO 2 The substance can be transported to the site of desorption or release.

[0364] Note: It may be desirable for revitalization to involve aggregated facilities, or facilities that can benefit from economies of scale, or any combination thereof.

[0365] Example 26: Separated CO 2 CO absorption or adsorption 2 Recovery of CO 2 Desorption or release of and regeneration of reagents (1)CO 2 Absorption of CO2 can be absorbed or adsorbed onto calcium oxide, or calcium hydroxide, or a calcium hydroxide suspension such as milk of lime, or any combination thereof to produce a calcium carbonate solid or suspension. Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O(l or g)

[0366] (2)CO 2 Desorption or release of: Calcium carbonate can react with aqueous sulfurous acid to produce calcium sulfite and carbon dioxide. CaCO 3 (s)+SO 2 (aq) → CaSO 3 (s)+CO 2 (g)

[0367] Note: CO 2 (g) SO 2 (g) Steam may be present. In some embodiments, SO 2 (g) is, for example and without limitation, a certain amount of SO 2 (g) CO 2 (g) CaCO 3 or by contacting with a certain amount of SO 2 (g) CO 2 (g) by contacting it with sodium carbonate or with a certain amount of SO 2 (g) CO 2 CO2(g) can be at least partially removed from CO2(g), such as by contacting (g) with an alkali carbonate, or by one or more of compression, or cooling, or condensation, or cryogenic separation, or freeze separation, or any combination thereof.

[0368] (3) Regeneration: Calcium sulfite is converted to calcium oxide and sulfur dioxide. Calcium oxide reacts with water to form calcium hydroxide suspensions such as milk of lime. CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0369] Example 27: Separated CO 2 CO absorption or adsorption 2 Recovery of CO 2 Desorption or release of and regeneration of reagents (1)CO 2 Adsorption of CO in calcium oxide or hydroxide to produce calcium carbonate solids 2 Adsorption or absorption of CaO(s)+CO 2 (g) → CaCO 3 (s) Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O(l or g)

[0370] (2)CO 2 Desorption or release of: Calcium carbonate can react with acetic acid to produce calcium acetate and carbon dioxide. CaCO 3 (s)+2CH 3 COOHCa→(CH 3 COO) 2 (aq)+CO 2 (g)

[0371] (3) Regeneration: Calcium acetate can react with sulfur dioxide to produce calcium sulfite. Calcium sulfite is converted to calcium oxide and sulfur dioxide. Calcium oxide can react with water to form calcium hydroxide. In some embodiments, calcium hydroxide can be formed by reaction of calcium oxide with water vapor. Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq) → CaSO 3 (s)+2CH 3 COOH(aq) CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0372] Example 28: Separated CO 2 CO absorption or adsorption 2 Recovery of CO 2 Desorption or release of and reagent regeneration (1)CO 2 Adsorption of CO in calcium oxide or hydroxide to produce calcium carbonate solids 2 Adsorption or absorption of. CaO(s)+CO 2 (g) → CaCO 3 (s) Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O(l or g)

[0373] (2)CO 2 Desorption or release: Calcium carbonate can react with sulfurous acid to produce calcium sulfite and carbon dioxide. CaCO 3 (s)+2CH 3 COOH→Ca(CH 3 COO) 2 (aq)+CO 2 (g)

[0374] (3) Regeneration: Calcium sulfite can be converted to calcium oxide and sulfur dioxide. Calcium oxide can react with water to form calcium hydroxide. In some embodiments, calcium hydroxide can be formed by reaction of calcium oxide with water vapor. Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq) → CaSO 3 (s)+2CH 3COOH(aq) CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0375] Example 29: Separated CO 2 CO absorption or adsorption 2 Recovery of CO 2 Desorption or release of and reagent regeneration (1)CO 2 Absorption of CO in sodium carbonate solution or in sodium hydroxide solution to produce sodium carbonate precipitate 2 If a sodium carbonate precipitate forms, it can be separated using, for example, a solid-liquid separation method. 2NaOH(aq or s)+CO 2 (g) → Na 2 CO 3 (aq or s) + H 2 O(l or aq or g)

[0376] NOTE: Sodium hydroxide solid or solution may be transported to the absorption site and / or stored at or near the absorption site.

[0377] NOTE: Sodium carbonate can be stored at or near the site of absorption or adsorption. Sodium carbonate can be transported to the application where calcium carbonate is used. Sodium carbonate is 2 In some embodiments, CO can be transported to the site of desorption or release. 2 The site of desorption or release of CO 2 In some embodiments, the CO 2 The site of desorption or release of CO 2 For example, in some embodiments, the location of absorption or adsorption of CO 2It may be desirable for absorption or adsorption to be located at multiple distributed sites, while regeneration may occur at a larger and / or more centralized facility or site.

[0378] (2)CO 2 Desorption or release: Sodium carbonate can react with acetic acid to produce sodium acetate and carbon dioxide. Na 2 CO 3 (aq or s) + 2CH 3 COOH→2NaCH 3 COO+CO 2 (g) Note: Sodium carbonate is CO 2 The substance may be stored at or near the site of desorption or release. Note: Acetic acid is CO 2 The substance may be stored at or near the site of desorption or release. ·Note: CO 2 The desorption or release of CO can be deployed in applications requiring carbon dioxide, or high purity carbon dioxide, or high pressure carbon dioxide, or recovered carbon dioxide, or any combination thereof. For example, 2 The desorption or release of CO 2 The system can be deployed in locations requiring enhanced oil recovery (EOR) through the use of sulphuric acid. NOTE: Sodium acetate may include aqueous calcium acetate, or solid sodium acetate, or any combination thereof. Note: Sodium acetate is CO 2 The sodium acetate can be stored at or near the site of desorption or release of sodium acetate. The sodium acetate can be transported to an application where the sodium acetate is used. The sodium acetate can be transported to or near the site of regeneration. In some embodiments, the sodium acetate can be stored at or near the site of desorption or release of sodium acetate. 2 The location of desorption or release of CO may be the same as the location of regeneration. 2 The location of desorption or release of CO may be different from the location of regeneration. For example, in some embodiments, 2It may be desirable for the desorption or release of to be located at multiple distributed sites, while regeneration may occur at a larger and / or more centralized facility or site. ·Note: CO 2 Acetic acid vapor may be present in (g). In some embodiments, the acetic acid vapor may be present in, for example, but not limited to, CO 2 (g) CaCO 3 or CO containing a certain amount of acetic acid vapor. 2 (g) with sodium carbonate or CO containing a certain amount of acetic acid vapor. 2 (g) by contacting the CO with an alkali carbonate, or by one or more of compression, or cooling, or condensation, or cryogenic separation, or freeze separation, or any combination thereof. 2 (g) can be at least partially removed.

[0379] (3) Regeneration: Sodium acetate can be reacted with sulfur dioxide to produce sodium sulfite and acetic acid. Sodium sulfite can be separated from the acetic acid. Sodium sulfite can be reacted with calcium hydroxide, or calcium oxide, or a calcium hydroxide suspension, or any combination thereof, to produce sodium hydroxide and calcium sulfite. Calcium sulfite solids can be separated from the sodium hydroxide solution. Calcium sulfite solids can be converted to calcium oxide and sulfur dioxide. Calcium oxide can be reacted with water to produce calcium hydroxide or a calcium hydroxide suspension. 2NaCH 3 COO+SO 2 (g or aq) → Na 2 SO 3 (aq or s) + 2CH 3 COOH(aq) Na 2 SO 3 and 2CH 3 COOH separation Na 2 SO 3 (aq or aq) + Ca(OH) 2 (s or aq) → CaSO3 (s) + 2NaOH CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq) Note: Sodium hydroxide is CO 2 The ions can be transported to a site of absorption or adsorption. Note: Acetic acid is CO 2 The substance can be transported to the site of desorption or release. · Note: It may be desirable for revitalization to involve aggregated facilities, or facilities that can benefit from economies of scale, or any combination thereof.

[0380] Example 30: Separated CO 2 CO absorption or adsorption 2 Recovery of CO 2 Desorption or release of and reagent regeneration (1)CO 2 Absorption of CO into a sodium hydroxide solution to produce a sodium carbonate solution, or a solid precipitate, or any combination thereof. 2 Absorption of. 2NaOH(aq or s)+CO 2 (g) → Na 2 CO 3 (aq or s) + H 2 O(l or aq or g)

[0381] (2)CO 2 Desorption or release: Sodium carbonate can react with aqueous sulfurous acid or aqueous sulfur dioxide to produce sodium sulfite and carbon dioxide. Na 2 CO 3 (aq or s) + SO 2 (aq) → Na 2 SO 3 (aq or s) + CO 2 (g) ·Note: CO 2 (g) SO 2(g) Steam may be present. In some embodiments, SO 2 (g) is, for example and without limitation, a certain amount of SO 2 (g) CO 2 (g) CaCO 3 or by contacting with a certain amount of SO 2 (g) CO 2 (g) by contacting it with sodium carbonate or with a certain amount of SO 2 (g) CO 2 CO2(g) can be at least partially removed from CO2(g), such as by contacting (g) with an alkali carbonate, or by one or more of compression, or cooling, or condensation, or cryogenic separation, or freeze separation, or any combination thereof.

[0382] (3) Regeneration: Sodium sulfite can be reacted with calcium hydroxide, or calcium oxide, or a calcium hydroxide suspension, or any combination thereof, to produce sodium hydroxide and calcium sulfite. The calcium sulfite solids are separated from the sodium hydroxide solution. The calcium sulfite solids are converted to calcium oxide and sulfur dioxide. Calcium oxide can be reacted with water to produce a calcium oxide or calcium hydroxide suspension. Na 2 SO 3 (aq or s) + Ca(OH) 2 (s or aq) → CaSO 3 (s) + 2NaOH (aq or s) CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0383] Example 31: CO 2 and sodium hydroxide (1)CO 2Desorption or release of: Sodium bicarbonate, which may constitute nahconite, can react with aqueous sulfurous acid or aqueous sulfur dioxide to produce sodium sulfite and carbon dioxide. 2NaHCO 3 (aq or s) + SO 2 (aq) → Na 2 SO 3 (aq or s) + H 2 O+2CO 2 (g), or 2NaHCO 3 (aq or s) + 2SO 2 (aq) → NaHSO 3 (aq or s) + 2CO 2 (g)

[0384] (2) Production of Sodium Hydroxide: Sodium sulfite can be reacted with calcium hydroxide, or calcium oxide, or a calcium hydroxide suspension, or any combination thereof, to produce sodium hydroxide and calcium sulfite. The calcium sulfite solids are separated from the sodium hydroxide solution. The calcium sulfite solids are converted to calcium oxide and sulfur dioxide. Calcium oxide can be reacted with water to produce calcium hydroxide or a calcium hydroxide suspension. Na 2 SO 3 (aq or s) + Ca(OH) 2 (s or aq) → CaSO 3 (s) + 2NaOH (aq or s) CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0385] Example 31: CO 2 and sodium hydroxide (2)CO 2 Desorption or release of: Sodium bicarbonate, which may constitute nahconite, can react with acetic acid to produce sodium acetate and carbon dioxide. 2NaHCO 3 (aq or s) + 2CH 3 COOH→2NaCH 3 COO+2CO 2 (g)

[0386] (3) Regeneration: Sodium acetate can be reacted with sulfur dioxide to produce sodium sulfite and acetic acid. Sodium sulfite is separated from the acetic acid. Sodium sulfite can be reacted with calcium hydroxide, or calcium oxide, or a calcium hydroxide suspension, or any combination thereof, to produce sodium hydroxide and calcium sulfite. Calcium sulfite solids are separated from the sodium hydroxide solution. Calcium sulfite solids are converted to calcium oxide and sulfur dioxide. Calcium oxide can be reacted with water to produce calcium hydroxide or a calcium hydroxide suspension. 2NaCH 3 COO+SO 2 (g or aq) → Na 2 SO 3 (aq or s) + 2CH 3 COOH(aq) Na 2 SO 3 and 2CH 3 COOH separation Na 2 SO 3 (aq or aq) + Ca(OH) 2 (s or aq) → CaSO 3 (s) + 2NaOH CaSO 3 (s) → CaO(s) + SO 2 (g) CaO(s)+H 2 O(g or l) → Ca(OH) 2 (s or aq)

[0387] Example 32: Preparation of lithium hydroxide from lithium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3(s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0388] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0389] (2) Ca(CH 3 COO) 2 (aq)+Li 2 SO 4 (aq) → 2LiCH 3 COO(aq)+CaSO 4 (s)

[0390] (3) 2LiCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Li 2 SO 3 (aq)+2CH 3 COOH(aq)

[0391] (4) Li 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq or l)+Li 2 SO 3(s)+water

[0392] Note: CH 3 COOH is Li 2 SO 3 In some embodiments, the water can be removed and / or the Li 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0393] Note:Li 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0394] (5) Li 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2LiOH(aq or s) + CaSO 3 (s)

[0395] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0396] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0397] (6) CaSO 3 →(s)CaO(s)+SO 2 (g)

[0398] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3(s) baking.

[0399] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0400] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0401] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0402] (8) 2LiOH(aq or s) → 2LiOH(s) + Water

[0403] NOTE: In some embodiments, water can be removed and / or LiOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0404] NOTE: In some embodiments, it may be desirable for LiOH to constitute a concentrated aqueous solution.

[0405] Example 33: Production of sodium hydroxide from sodium chloride using calcium precipitation, acid intermediates and process for the production of sodium sulfate and calcium chloride from calcium sulfate and sodium chloride (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0406] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0407] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0408] NOTE: In some embodiments, Na 2 SO 4 (s or aq) can be transferred from step (10).

[0409] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0410] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq or l)+Na 2 SO3 (s)+water

[0411] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, the water can be removed and / or the Na 2 SO 3 may be separated or precipitated, for example, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0412] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH (aq or l) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0413] (5)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0414] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0415] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0416] (6) CaSO 3 →(s)CaO(s)+SO 2 (g)

[0417] Note: "(6)" indicates CaSO4, which may be kiln-fired.3 (s) baking.

[0418] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0419] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0420] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0421] (8) 2NaOH(aq or s) → 2NaOH(s) + Water

[0422] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0423] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0424] (9) CaSO 4 (s or aq)+(NH 4 ) 2 CO 3 (aq) → CaCO 3 (s or aq)+(NH 4 ) 2 SO 4 (aq)

[0425] Note: CaSO 4 (s or aq) can be transferred from step “(2)”.

[0426] Note: CaCO 3 (s) is separated into (NH 4 ) 2 SO 4 It can be separated from a solution containing (aq).

[0427] (10)(NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) → 2NH 4 Cl(aq)+Na 2 SO 4 (s or aq)

[0428] NOTE: In some embodiments, the lower the temperature, e.g., below about 32 °C, or the closer the temperature of the solution is to 0 °C, the greater the NH 4 Na compared to Cl 2 SO 4 As the solubility of Na in water becomes increasingly low, 2 SO 4 A portion of (s) can be precipitated by cooling precipitation.

[0429] NOTE: In some embodiments, Na 2 SO 4 is obtained by distillation, or crystallization, or cooling precipitation, or any combination thereof, from 2NH 4 In some embodiments, Na 2 SO 4 (s), or water, or 2NH 4 Cl(aq) or 2NH 4 Cl(s), or any combination thereof may be produced or formed.

[0430] (11) One or more of the following or any combination thereof: 2NH 4 Cl(s) → 2NH 3 (g) + 2HCl(g) 2NH 3 (g) + 2HCl(g) + CaCO 3 (s) → CaCl 2 (s)+H 2 O(g)+CO 2(g)+2NH 3 (g) ·CaCO 3 (s)+2NH 4 Cl(s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g)

[0431] Note: CaCO 3 (s) can be transferred from step (9).

[0432] NOTE: One or more of the above reactions or any combination thereof may require heat input.

[0433] NOTE: In some embodiments, heat can be recovered from one or more of the reactions or any combination thereof. For example, calcium carbonate and hydrogen chloride can be exothermic.

[0434] NOTE: In some embodiments, 2NH is synthesized from aqueous solution in the presence of calcium carbonate. 4 Cl(s) can be precipitated or crystallized to form a dispersed mixture of, for example, calcium carbonate and ammonium chloride.

[0435] NOTE: Calcium chloride may constitute an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may constitute a waste product.

[0436] (12)2NH 3 (g)+H 2 O(g)+CO 2 (g) → (NH 4 ) 2 CO 3 (s or aq)

[0437] Note:(NH 4 ) 2 CO 3 (s or aq) can be transferred to step “(9)”.

[0438] Note: 2NH 3 (g) or H 2 O(g) or CO 2 (g), or any combination thereof, can be recycled or recirculated within the process. In some embodiments, losses may occur and / or 2NH 3 , or H 2 O or CO 2 , or any combination thereof may be added.

[0439] Example 34: Ammonium Sulfate, Sodium Chloride and Calcium - Process for the Production of Sodium Sulfate, Ammonia and Calcium Chloride from Weak Acid (1)(NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) → 2NH 4 Cl(aq)+Na 2 SO 4 (s or aq)

[0440] NOTE: In some embodiments, the lower the temperature, e.g., below about 32 °C, or the closer the temperature of the solution is to 0 °C, the greater the NH 4 Na compared to Cl 2 SO 4 As the solubility of Na in water becomes increasingly low, 2 SO 4 A portion of (s) can be precipitated by cooling precipitation.

[0441] NOTE: In some embodiments, Na 2 SO 4 is obtained by distillation, or crystallization, or cooling precipitation, or any combination thereof, from 2NH 4 In some embodiments, Na 2 SO 4 (s), or water, or 2NH 4 Cl(aq) or 2NH 4 Cl(s), or any combination thereof may be produced or formed.

[0442] (2) One or more of the following or any combination thereof: 2NH 4 Cl(s) → 2NH 3 (g) + 2HCl(g) 2NH 3 (g) + 2HCl(g) + CaCO 3 (s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g) ·CaCO 3 (s)+2NH 4 Cl(s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g) 2NH 3 (g) + 2HCl(g) + Ca(WA)(s) → CaCl 2 (s)+H 2 O(g) + WA(s or g or l) + 2NH 3 (g) Ca(WA)(s)+2NH 4 Cl(s) → CaCl 2 (s)+H 2 O(g) + WA(s or g or l) + 2NH 3 (g)

[0443] NOTE: One or more of the above reactions or any combination thereof may require heat input.

[0444] NOTE: In some embodiments, heat can be recovered from one or more of the reactions or any combination thereof. For example, calcium carbonate and hydrogen chloride can be exothermic.

[0445] NOTE: In some embodiments, 2NH 4 Cl(s) can be precipitated or crystallized from an aqueous solution in the presence of a calcium-weak acid to form a dispersed mixture of, for example, calcium-weak acid and ammonium chloride.

[0446] NOTE: Calcium chloride may constitute an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may constitute a waste product.

[0447] NOTE: In some embodiments, the carbon dioxide produced may include recovered carbon dioxide. For example, ammonia and / or water may be separated from the carbon dioxide using aqueous solutions and / or high pressure and / or high temperature.

[0448] Example 35: Process for producing sodium sulfate and calcium chloride from sodium chloride and calcium sulfate using ammonia and carbon dioxide intermediates (1) CaSO 4 (s or aq)+(NH 4 ) 2 CO 3 (aq) → CaCO 3 (s or aq)+(NH 4 ) 2 SO 4 (aq)

[0449] Note: CaSO 4 (s or aq) may constitute the input. For example, CaSO 4 (s) may be a product or by-product from the process, e.g., CaSO 4 (s) may be mined, e.g., CaSO 4 (s) may constitute phosphogypsum.

[0450] Note: CaCO 3 (s) is separated into (NH 4 ) 2 SO 4 It can be separated from a solution containing (aq).

[0451] (2)(NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) → 2NH 4 Cl(aq)+Na 2 SO 4 (s or aq)

[0452] NOTE: In some embodiments, the lower the temperature, e.g., below about 32 °C, or the closer the temperature of the solution is to 0 °C, the greater the NH 4 Na compared to Cl 2 SO 4 As the solubility of Na in water becomes increasingly low, 2 SO 4 A portion of (s) can be precipitated by cooling precipitation.

[0453] NOTE: In some embodiments, Na 2 SO 4 is separated from 2NH by distillation, or crystallization, or cooling precipitation, or the separation methods described herein, or any combination thereof. 4 In some embodiments, Na 2 SO 4 (s), or water, or 2NH 4 Cl(aq) or 2NH 4 Cl(s), or any combination thereof may be produced or formed.

[0454] (3) One or more of the following or any combination thereof: 2NH 4 Cl(s) → 2NH 3 (g) + 2HCl(g) 2NH 3 (g) + 2HCl(g) + CaCO 3 (s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g) ·CaCO 3 (s)+2NH 4 Cl(s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g)

[0455] Note: CaCO 3 (s) can be transferred from step (1).

[0456] NOTE: One or more of the above reactions or any combination thereof may require heat input.

[0457] NOTE: In some embodiments, heat can be recovered from one or more of the reactions or any combination thereof. For example, calcium carbonate and hydrogen chloride can be exothermic.

[0458] NOTE: In some embodiments, 2NH is synthesized from aqueous solution in the presence of calcium carbonate. 4 Cl(s) can be precipitated or crystallized to form a dispersed mixture of, for example, calcium carbonate and ammonium chloride.

[0459] NOTE: Calcium chloride may constitute an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may constitute a waste product.

[0460] (4) 2NH 3 (g)+H 2 O(g)+CO 2 (g) → (NH 4 ) 2 CO 3 (s or aq)

[0461] Note:(NH 4 ) 2 CO 3 (s or aq) can be transferred to step “(1)”.

[0462] Note: 2NH 3 (g) or H 2 O(g) or CO 2 (g), or any combination thereof, can be recycled or recirculated within the process. In some embodiments, losses may occur and / or 2NH 3 , or H 2 O or CO 2 , or any combination thereof may be added.

[0463] Example 36: Process for producing sodium sulfate and calcium chloride from sodium chloride and calcium sulfate with carbon dioxide recovery (1) 2NH 3 (aq)+H 2 O(g)+CO 2 (g) → (NH 4 ) 2 CO 3 (s or aq)

[0464] Note: CO 2 (g) CO 2 (g) may comprise a gas containing CO 2 (g) may comprise a gas containing a dilute concentration of carbon dioxide, including, but not limited to, flue gas, exhaust gas, sour gas, air, or other CO2 gases described herein. 2 Source, or other CO in the art 2 The source may include, for example, a source of

[0465] (2) CaSO 4 (s or aq)+(NH 4 ) 2 CO 3 (aq) → CaCO 3 (s or aq)+(NH 4 ) 2 SO 4 (aq)

[0466] Note: CaSO 4 (s or aq) may constitute the input. For example, CaSO 4 (s) may be a product or by-product from the process, e.g., CaSO 4 (s) may be mined, e.g., CaSO 4 (s) may constitute phosphogypsum.

[0467] Note: CaCO 3 (s) is separated into (NH 4 ) 2 SO 4It can be separated from a solution containing (aq).

[0468] (3)(NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) → 2NH 4 Cl(aq)+Na 2 SO 4 (s or aq)

[0469] NOTE: In some embodiments, the lower the temperature, e.g., below about 32 °C, or the closer the temperature of the solution is to 0 °C, the greater the NH 4 Na compared to Cl 2 SO 4 As the solubility of Na in water becomes increasingly low, 2 SO 4 A portion of (s) can be precipitated by cooling precipitation.

[0470] NOTE: In some embodiments, Na 2 SO 4 is separated from 2NH by distillation, or crystallization, or cooling precipitation, or the separation methods described herein, or any combination thereof. 4 In some embodiments, Na 2 SO 4 (s), or water, or 2NH 4 Cl(aq) or 2NH 4 Cl(s), or any combination thereof may be produced or formed.

[0471] (4) One or more of the following or any combination thereof: 2NH 4 Cl(s) → 2NH 3 (g) + 2HCl(g) 2NH 3 (g) + 2HCl(g) + CaCO 3 (s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g) ·CaCO 3 (s)+2NH4 Cl(s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g)

[0472] Note: CaCO 3 (s) can be transferred from step (1).

[0473] NOTE: One or more of the above reactions or any combination thereof may require heat input.

[0474] NOTE: In some embodiments, heat can be recovered from one or more of the reactions or any combination thereof. For example, calcium carbonate and hydrogen chloride can be exothermic.

[0475] NOTE: In some embodiments, 2NH is synthesized from aqueous solution in the presence of calcium carbonate. 4 Cl(s) can be precipitated or crystallized to form a dispersed mixture of, for example, calcium carbonate and ammonium chloride.

[0476] NOTE: Calcium chloride may constitute an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may constitute a waste product.

[0477] (5) 2NH 3 (g)+H 2 O(g)+CO 2 (g) → 2NH 3 (aq)+CO 2 (g)

[0478] Note: 2NH 3 (aq) can be transferred to step “(1)”.

[0479] NOTE: When performed in the presence of liquid water, at pressures 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 at temperatures 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, ammonia can move mostly to the water phase and carbon dioxide can remain mostly in the gas phase.

[0480] NOTE: In some embodiments, CO 2 may be further purified to remove residual ammonia. For example, CO 2 (g) can be cooled, so that at least a portion of the residual ammonia can be removed by the formation of an ammonia-carbon dioxide derivative salt, such as ammonium carbamate, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof. For example, CO2 containing residual ammonia can be 2 (g) can be cooled and / or contacted with water to remove at least a portion of the residual ammonia by formation of aqueous ammonia, or an ammonia-carbonate derivative salt, such as ammonium carbamate, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof.

[0481] Example 37: Process for producing sodium sulfate, calcium chloride and urea from sodium chloride, calcium sulfate, ammonia and carbon dioxide (1) 2NH 3 (g or aq) + water + CO 2 (g) → (NH 4 ) 2 CO 3 (s or aq)

[0482] Note: CO 2 (g) CO 2 (g) may comprise a gas containing CO2 (g) may comprise a gas containing a dilute concentration of carbon dioxide, including, but not limited to, flue gas, exhaust gas, sour gas, air, or other CO2 gases described herein. 2 Source, or other CO in the art 2 The source may include, for example, a source of

[0483] (2) CaSO 4 (s or aq)+(NH 4 ) 2 CO 3 (aq) → CaCO 3 (s or aq)+(NH 4 ) 2 SO 4 (aq)

[0484] Note: CaSO 4 (s or aq) may constitute the input. For example, CaSO 4 (s) may be a product or by-product from the process, e.g., CaSO 4 (s) may be mined, e.g., CaSO 4 (s) may constitute phosphogypsum.

[0485] Note: CaCO 3 (s) is separated into (NH 4 ) 2 SO 4 It can be separated from a solution containing (aq).

[0486] (3)(NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) → 2NH 4 Cl(aq)+Na 2 SO 4 (s or aq)

[0487] NOTE: In some embodiments, the lower the temperature, e.g., below about 32 °C, or the closer the temperature of the solution is to 0 °C, the greater the NH 4 Na compared to Cl 2 SO 4As the solubility of Na in water becomes increasingly low, 2 SO 4 A portion of (s) can be precipitated by cooling precipitation.

[0488] NOTE: In some embodiments, Na 2 SO 4 is separated from 2NH by distillation, or crystallization, or cooling precipitation, or the separation methods described herein, or any combination thereof. 4 In some embodiments, Na 2 SO 4 (s), or water, or 2NH 4 Cl(aq) or 2NH 4 Cl(s), or any combination thereof may be produced or formed.

[0489] (4) One or more of the following or any combination thereof: 2NH 4 Cl(s) → 2NH 3 (g) + 2HCl(g) 2NH 3 (g) + 2HCl(g) + CaCO 3 (s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g) ·CaCO 3 (s)+2NH 4 Cl(s) → CaCl 2 (s)+H 2 O(g)+CO 2 (g)+2NH 3 (g)

[0490] Note: CaCO 3 (s) can be transferred from step (1).

[0491] NOTE: One or more of the above reactions or any combination thereof may require heat input.

[0492] NOTE: In some embodiments, heat can be recovered from one or more of the reactions or any combination thereof. For example, calcium carbonate and hydrogen chloride can be exothermic.

[0493] NOTE: In some embodiments, 2NH is synthesized from aqueous solution in the presence of calcium carbonate. 4 Cl(s) can be precipitated or crystallized to form a dispersed mixture of, for example, calcium carbonate and ammonium chloride.

[0494] NOTE: Calcium chloride may constitute an output. In some embodiments, calcium chloride may be sold or utilized. In some embodiments, calcium chloride may constitute a waste product.

[0495] (5) 2NH 3 (g)+H 2 O(g)+CO 2 (g) → 2NH 3 (aq)+CO 2 (g)

[0496] NOTE: When performed in the presence of liquid water, at pressures 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 at temperatures 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, ammonia can move mostly to the water phase and carbon dioxide can remain mostly in the gas phase.

[0497] (6) 2NH 3 (aq) → 2NH 3 (g)+water

[0498] (7)2NH 3 (g) + CO 2 (g) → 2(NH 2 ) 2 CO(s)+H 2O(g or l)

[0499] NOTE: This process can produce urea and / or water.

[0500] NOTE: It may be desirable to further dry the ammonia or carbon dioxide or both before use in the production of urea.

[0501] Example 38: Preparation of sodium hydroxide from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0502] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0503] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO4 (s)

[0504] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0505] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq, isolated)+Na 2 SO 3 (aq, isolated)

[0506] NOTE: The aqueous solution containing sodium sulfite and acetic acid can be separated into another aqueous solution containing acetic acid and another aqueous solution containing sodium sulfite using, for example, electrodialysis, or reverse electrodialysis, or selective electrodialysis.

[0507] NOTE: For example, in some embodiments, electrodialysis selective for mono- or di- or tri- or tetravalent cations, or mono- or di- or tri- or tetravalent anions, or any combination thereof, may be used.

[0508] NOTE: An aqueous solution containing acetic acid can be used as the aqueous acetic acid in step “(1).”

[0509] (5)Na 2 SO 3 (aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaSO 3 (s)

[0510] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0511] Note: CaSO 3(s) can be separated using solid-liquid separation.

[0512] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0513] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0514] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0515] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0516] Note: CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0517] (8) 2NaOH(aq) → 2NaOH(aq or s) + Water

[0518] NOTE: In some embodiments, it may be desirable for the NaOH to constitute an aqueous solution or a concentrated aqueous solution. In some embodiments, the NaOH(aq) may be concentrated or further concentrated using one or more of the separation or water removal methods or any combination thereof.

[0519] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0520] NOTE: Water or distillate from the concentration or further concentration may be used in the process. For example, the water or distillate from the concentration or further concentration may be used for one or more or any combination thereof, including, but not limited to, dissolving sodium sulfate, or absorbing acetic acid vapor, or diluting or mixing with an aqueous solution comprising sodium acetate, or diluting or mixing with an aqueous solution comprising sodium sulfite and acetic acid, or any combination thereof.

[0521] Example 39: Preparation of Sodium Hydroxide and Calcium Oxide from Sodium Sulfate and Calcium Carbonate Using Calcium Precipitation and Acid Intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0522] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0523] (2) Ca(CH 3 COO) 2 (aq)+Na2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0524] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0525] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0526] (5) CaCO 3 (s or aq)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq)

[0527] NOTE: In some embodiments, high CO 2 For example, in some embodiments, the reaction may be carried out under partial pressures and / or elevated temperatures, such as above 1 bar, or 2 bar, or 3 bar, or 4 bar, or 5 bar, or any combination thereof. 2 Partial pressures and / or temperatures greater than 0°C, or 20°C, or 40°C, or 50°C, or 60°C, or 70°C, or 80°C, or 90°C, or 95°C, or 100°C can be used.

[0528] Note: CO 2 can be a source such as, but not limited to, one or more of the following: decomposition of sodium bicarbonate, or captured carbon dioxide, or a combination thereof, or any combination thereof.

[0529] (6)Na 2 SO 3 (s)+water→Na 2 SO 3 (aq)

[0530] (7)Na 2 SO 3 (aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s)

[0531] (8) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0532] (9)2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[0533] (10)Na 2 CO 3 (aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaCO 3 (s)

[0534] (11) 2NaOH(aq) → 2NaOH(aq or s) + Water

[0535] (12)CaCO 3 (s) → CaO(s) + CO 2 (g)

[0536] NOTE: In some embodiments, calcium carbonate may be decomposed to calcium oxide in a manner that produces high purity or recovered carbon dioxide. For example, in some embodiments, calcium carbonate may be calcined or decomposed by indirect calcination or indirect heating, resulting in the production of high purity or recovered carbon dioxide.

[0537] NOTE: The captured carbon dioxide can be sequestered or used in one or more applications or any combination thereof.

[0538] (13)CaO(s)+water→Ca(OH) 2 (s or aq)

[0539] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0540] NOTE: In some embodiments, calcium carbonate and sodium hydroxide can be produced by directly reacting calcium oxide with an aqueous solution containing sodium carbonate. For example, in some embodiments, step "(10)" can be combined with step "(13)".

[0541] Example 40: Preparation of sodium carbonate or sodium bicarbonate from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2(aq) + weak acid (s, g, l, or aq)

[0542] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0543] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0544] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0545] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0546] (5) CaCO 3 (s or aq)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq)

[0547] NOTE: In some embodiments, high CO 2 For example, in some embodiments, the reaction may be carried out under partial pressures and / or elevated temperatures, such as above 1 bar, or 2 bar, or 3 bar, or 4 bar, or 5 bar, or any combination thereof. 2Partial pressures and / or temperatures greater than 0°C, or 20°C, or 40°C, or 50°C, or 60°C, or 70°C, or 80°C, or 90°C, or 95°C, or 100°C can be used.

[0548] Note: CO 2 can be a source such as, but not limited to, one or more of the following: decomposition of sodium bicarbonate, or captured carbon dioxide, or a combination thereof, or any combination thereof.

[0549] (6)Na 2 SO 3 (s)+water→Na 2 SO 3 (aq)

[0550] (7)Na 2 SO 3 (aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s)

[0551] (8) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0552] (9)2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[0553] (10)Na 2 CO 3 (aq) → Na 2 CO 3 (s)+water

[0554] Example 41: Precipitation of calcium, acid intermediate and production of sodium hydroxide from sodium sulfate using calcium carbonate intermediate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0555] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0556] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0557] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0558] (4)Na 2 SO 3 (aq)+2CH3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0559] (5) CaCO 3 (s or aq)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq)

[0560] NOTE: In some embodiments, high CO 2 For example, in some embodiments, the reaction may be carried out under partial pressures and / or elevated temperatures, such as above 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 11 bar, or 12 bar, or 13 bar, or 14 bar, or 15 bar, or any combination thereof. 2 Partial pressures and / or temperatures greater than 0°C, or 20°C, or 40°C, or 50°C, or 60°C, or 70°C, or 80°C, or 90°C, or 95°C, or 100°C can be used.

[0561] Note: CO 2 can be a source such as, but not limited to, one or more of the following: decomposition of sodium bicarbonate, or captured carbon dioxide, or a combination thereof, or any combination thereof.

[0562] (6)Na 2 SO 3 (s)+water→Na 2 SO 3 (aq)

[0563] (7)Na 2 SO 3 (aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO3 (s)

[0564] (8) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0565] NOTE: CaO(s) may be transferred to step “(9)” or step “(11)”.

[0566] Note: 2 (g) can be transferred to step “(3)”.

[0567] (9)CaO(s)+water→Ca(OH) 2 (s or aq)

[0568] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0569] NOTE: In some embodiments, calcium carbonate and sodium hydroxide can be produced by directly reacting an aqueous solution containing sodium carbonate with calcium oxide. In some embodiments, calcium carbonate and sodium hydroxide can be produced by directly reacting an aqueous solution containing sodium carbonate with calcium oxide, which may include combining step "(9)" and step "(11)".

[0570] (10)2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[0571] Note: CO 2 can be transferred to step (5).

[0572] (11)Na 2 CO 3 (aq) + Ca(OH) 2(s or aq) → 2NaOH(aq) + CaCO 3 (s)

[0573] NOTE: Aqueous solutions containing sodium hydroxide(s) can be separated from calcium carbonate by solid-liquid separation.

[0574] Note: Calcium carbonate can be transferred to "(5)".

[0575] (12) 2NaOH(aq) → 2NaOH(aq or s) + Water

[0576] NOTE: The solution comprising sodium hydroxide may be further concentrated, or at least a portion of the water may be removed from the solution comprising sodium hydroxide, or any combination thereof.

[0577] NOTE: In some embodiments, at least a portion of the water removed or recovered from the solution comprising aqueous sodium hydroxide can be transferred to step “(6).”

[0578] Example 42: Production of sodium hydroxide from sodium sulfate and calcium carbonate using calcium precipitation and carbon dioxide intermediate (1) CaCO 3 (s or aq)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq)

[0579] NOTE: In some embodiments, high CO 2 For example, in some embodiments, the reaction may be carried out under partial pressures and / or elevated temperatures, such as above 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 11 bar, or 12 bar, or 13 bar, or 14 bar, or 15 bar, or any combination thereof. 2Partial pressures and / or temperatures greater than 0°C, or 20°C, or 40°C, or 50°C, or 60°C, or 70°C, or 80°C, or 90°C, or 95°C, or 100°C can be used.

[0580] Note: CO 2 can be a source such as, but not limited to, one or more of the following: decomposition of sodium bicarbonate, or captured carbon dioxide, or a combination thereof, or any combination thereof.

[0581] (2)Na 2 SO 4 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 4 (s)

[0582] (3) 2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[0583] Note: CO 2 can be transferred to step (1).

[0584] (4)Na 2 CO 3 (aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaCO 3 (s)

[0585] NOTE: Aqueous solutions containing sodium hydroxide can be separated from calcium carbonate by solid-liquid separation.

[0586] Note: Calcium carbonate can be transferred to "(5)".

[0587] (5) 2NaOH(aq) → 2NaOH(aq or s) + Water

[0588] NOTE: The solution comprising sodium hydroxide may be further concentrated, or at least a portion of the water may be removed from the solution comprising sodium hydroxide, or any combination thereof.

[0589] NOTE: In some embodiments, at least a portion of the water removed or recovered from the solution comprising aqueous sodium hydroxide can be transferred to step “(1)” or step “(2).”

[0590] (6) CaCO 3 (s) → CaO(s) + CO 2 (g)

[0591] NOTE: In some embodiments, calcium carbonate may be decomposed to calcium oxide in a manner that produces high purity or recovered carbon dioxide. For example, in some embodiments, calcium carbonate may be calcined or decomposed by indirect calcination or indirect heating, resulting in the production of high purity or recovered carbon dioxide.

[0592] NOTE: The captured carbon dioxide can be sequestered or used in one or more applications or any combination thereof.

[0593] (7)CaO(s)+water→Ca(OH) 2 (s or aq)

[0594] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0595] NOTE: In some embodiments, calcium carbonate and sodium hydroxide can be produced by directly reacting calcium oxide with an aqueous solution containing sodium carbonate. For example, in some embodiments, step "(4)" can be combined with step "(7)".

[0596] Example 43: Preparation of sodium carbonate or sodium bicarbonate from sodium sulfate and calcium carbonate (1) CaCO 3 (s or aq)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq)

[0597] NOTE: In some embodiments, high CO 2 For example, in some embodiments, the reaction may be carried out under partial pressures and / or elevated temperatures, such as above 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 11 bar, or 12 bar, or 13 bar, or 14 bar, or 15 bar, or any combination thereof. 2 Partial pressures and / or temperatures greater than 0°C, or 20°C, or 40°C, or 50°C, or 60°C, or 70°C, or 80°C, or 90°C, or 95°C, or 100°C can be used.

[0598] Note: CO 2 can be a source such as, but not limited to, one or more of the following: decomposition of sodium bicarbonate, or captured carbon dioxide, or a combination thereof, or any combination thereof.

[0599] (2)Na 2 SO 4 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 4 (s)

[0600] NOTE: In some embodiments, NaHCO 3 (aq) or NaHCO 3 (s) may constitute a product that can be sold or used.

[0601] Note: 2NaHCO 3 (aq) is separated into CaSO by solid-liquid separation. 4 (s) can be separated from at least a portion of

[0602] (3) 2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[0603] Note: CO 2 can be transferred to step (1).

[0604] Example 44: Process for producing sodium hydroxide and calcium sulfate from sodium sulfate and weak acid calcium (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0605] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0606] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0607] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0608] (2) Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq)+H 2 O(l or aq) → CaSO 3 (s)+2CH 3 COOH(aq)

[0609] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0610] NOTE: In some embodiments, the 2CH 3 Residual aqueous magnesium sulfite may be present in "2CHCOOH(aq)" that was transferred from reaction to reaction "(1)". In some embodiments, the residual aqueous magnesium sulfite may be present in "2CH 3 In some embodiments, aqueous magnesium sulfite may be added to the "2CH" COOH(aq) that was transferred from reaction "(2)" to reaction "(1)". 3 This is because, for example, magnesium sulfite added or accumulated beyond the solubility limit of magnesium sulfite in solution may remain in Ca(CH 3 COO) 2 (aq) or Mg(CH 3 COO) 2 (aq) and SO 2 (g or aq) or may precipitate or co-precipitate during reaction with sulfite or bisulfite.

[0611] NOTE: In some embodiments, the 2CH 3Residual aqueous magnesium sulfite may be present in the "COOH(aq)". In some embodiments, a portion of the residual aqueous magnesium sulfite may be concentrated and / or separated using, but not limited to, one or more of heating, or cooling, or reverse osmosis, or a 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, where the pore size or characteristics of the membrane may allow for the permeation of at least a portion of the acetic acid and the rejection of at least a portion of the magnesium sulfite, and / or the resulting concentrated magnesium sulfite solution may be cooled to produce at least a portion of a magnesium sulfite precipitate.

[0612] (3) CaSO 3 (s)+SO 2 (g or aq)+H 2 O(aq) + water → Ca(HSO 3 ) 2 (aq)

[0613] (4)Na 2 SO 4 (s or aq) + Ca(HSO 3 ) 2 (aq) → 2NaHSO 3 (aq)+CaSO 4 (s)

[0614] Note: "(4)" is CaSO 4 (s) to reduce the solubility or dissolution of CaSO 4 To reduce the possibility of (aq) formation, it may be carried out at elevated temperatures.

[0615] (5) One or more of the following or any combination thereof: 2NaHSO 3 (aq) → Na 2 SO 3 (s or aq) + SO 2 (g)+H 2 O(g or l) 2NaHSO3 (aq) → Na 2 S 2 O 5 (s)+H 2 O+water ·Na 2 S 2 O 5 (s) → Na 2 SO 3 (s)+SO 2 (g)

[0616] (6)SO 2 (g or aq) + water → SO 2 (aq)

[0617] (7)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq) + CaSO 3 (s)

[0618] (8) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0619] (9) CaO(s)+H 2 O+water→Ca(OH) 2 (s or aq)

[0620] Example 45: Preparation of sodium hydroxide from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0621] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0622] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0623] (3) 2NaCH 3 COO(aq) + citric acid(aq) → sodium citrate(aq) + 2CH 3 COOH(aq)

[0624] NOTE: In some embodiments, other carboxylic acids besides citric acid may be used, such as carboxylic acids that form soluble sodium salts and relatively less soluble calcium salts.

[0625] (4) Sodium citrate (aq) + 2CH 3 COOH(aq) → Sodium citrate(s) + 2CH 3 COOH(aq)

[0626] NOTE: "(4)" may include separating sodium citrate from acetic acid. For example, sodium citrate may be separated from an aqueous solution containing acetic acid or from acetic acid by distillation.

[0627] (5) Sodium citrate (aq) + Ca(OH) 2(s or aq) → Calcium citrate (s) + 2NaOH (aq)

[0628] NOTE: The aqueous solution containing sodium hydroxide can be separated from the solid containing calcium citrate by solid-liquid separation.

[0629] (6) 2NaOH(aq) → 2NaOH(aq or s) + Water

[0630] NOTE: In some embodiments, the 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 processing. In some embodiments, the aqueous solution comprising sodium hydroxide may constitute a product and / or may be ready for sale or use.

[0631] (7) Calcium citrate(s) + SO 2 (aq) → Citric acid(aq) + CaSO 3 (s)

[0632] (8) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0633] (9)SO 2 (g)+water→SO 2 (aq)

[0634] (10) CaO(s)+H 2 O+water→Ca(OH) 2 (s or aq)

[0635] NOTE: In some embodiments, CaO(s) can be reacted with water. In some embodiments, CaO(s) can be reacted with sodium citrate to produce calcium citrate and sodium hydroxide. In some embodiments, for example, step "(5)" and step "(10)" can be combined.

[0636] Example 46: Process for the production of calcium oxide or cement or clinker using ascorbic acid intermediate (1) Reaction of calcium, or magnesium, or other alkaline earth-weak acid anion-containing materials with ascorbic acid, which may include, but is not limited to, one or more of the following or any combination thereof: ·CaCO 3 (s or aq) + ascorbic acid (aq) → calcium ascorbate (aq) + CO 2 (g) Calcium silicate(s) + ascorbic acid(aq) → calcium ascorbate(aq) + silicon dioxide(s) CaS(s) + ascorbic acid(aq) → calcium ascorbate(aq) + H 2 S(g) Calcium (weak acid anion) + ascorbic acid (aq) → calcium ascorbate (aq) + weak acid (s, or g, or l, or aq)

[0637] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0638] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0639] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0640] (2) Calcium ascorbate (aq) + SO 2 (g or aq)+H 2 O(l or aq) → CaSO 3 (s) + ascorbic acid (aq)

[0641] Note: CaSO 3(s) can be separated using solid-liquid separation.

[0642] NOTE: In some embodiments, the 2CH 3 Residual aqueous magnesium sulfite may be present in "2CHCOOH(aq)" that was transferred from reaction to reaction "(1)". In some embodiments, the residual aqueous magnesium sulfite may be present in "2CH 3 In some embodiments, aqueous magnesium sulfite may be added to the "2CH" COOH(aq) that was transferred from reaction "(2)" to reaction "(1)". 3 This is because, for example, magnesium sulfite added or accumulated beyond the solubility limit of magnesium sulfite in solution may remain in Ca(CH 3 COO) 2 (aq) or Mg(CH 3 COO) 2 (aq) and SO 2 (g or aq) or may precipitate or co-precipitate during reaction with sulfite or bisulfite.

[0643] NOTE: In some embodiments, the 2CH 3 Residual aqueous magnesium sulfite may be present in the "COOH(aq)". In some embodiments, a portion of the residual aqueous magnesium sulfite may be concentrated and / or separated using, but not limited to, one or more of heating, or cooling, or reverse osmosis, or a 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, where the pore size or characteristics of the membrane may allow for the permeation of at least a portion of the acetic acid and the rejection of at least a portion of the magnesium sulfite, and / or the resulting concentrated magnesium sulfite solution may be cooled to produce at least a portion of a magnesium sulfite precipitate.

[0644] Note: In some embodiments, the use of ascorbic acid may be desirable because it may be non-volatile, or may contain only minimal or no vapor phase, or any combination thereof. This may mean that the ascorbic acid may remain substantially in the aqueous phase, or may not substantially evaporate into residual gas, or any combination thereof. In some embodiments, other acids having stronger acid strength than "WA" or "weak acids" and weaker acidity than sulfurous acid, or other acids that form water-soluble calcium or magnesium or alkaline earth salts, or other acids that are non-volatile or have a lower vapor pressure or higher boiling point than water, or any combination thereof, may be used instead of or in addition to ascorbic acid.

[0645] (3) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0646] Note: "(3)" indicates CaSO, which may be kiln-fired. 3 (s) baking.

[0647] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(3)”.

[0648] Example 47: Preparation of sodium hydroxide from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2(aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0649] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0650] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0651] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0652] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → Na 2 SO 3 (s)+2CH 3 COOH(aq)

[0653] (5)Na 2 SO 3 (s)+H 2 O(g) → 2NaOH(s or l) + SO 2 (g)

[0654] NOTE: In some embodiments, the reaction can be carried out at elevated temperatures, or temperatures greater than 100° C., or 200° C., or 300° C., or 400° C., or 500° C., or 600° C., or any combination thereof.

[0655] Example 48: Preparation of sodium carbonate from sodium sulfate using calcium precipitation and acid intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0656] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0657] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0658] (3) 2NaCH3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0659] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → Na 2 SO 3 (s)+2CH 3 COOH(aq)

[0660] (5)Na 2 SO 3 (s)+CO 2 (g) → Na 2 CO 3 (s or l) + SO 2 (g)

[0661] NOTE: In some embodiments, the reaction can be carried out at elevated temperatures, or temperatures greater than 100° C., or 200° C., or 300° C., or 400° C., or 500° C., or 600° C., or any combination thereof.

[0662] Example 49: Direct Air Capture Process Using Alkaline Intermediate (1) One or more of the following or any combination thereof: CaO(s or aq)+CO 2 (g or aq) → CaCO 3 (s or aq) Ca(OH) 2 (s or aq)+CO 2 (g or aq) → CaCO 3 (s or aq)+H 2 O(aq)

[0663] Note: CO 2 (g) When CO is generated, 2 (g) High partial pressure CO 2 (g) or purity CO 2CO generated or captured in (g) 2 It may be desirable to include (g).

[0664] (2) CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)

[0665] Note: CO 2 (g) High partial pressure CO 2 (g) or purity CO 2 CO generated or captured in (g) 2 It may be desirable to include (g).

[0666] (3) Ca(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq) → 2NaCH 3 COO(aq)+CaSO 3 (s)

[0667] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0668] (4) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0669] (5)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0670] (6) CaSO 3(s) → CaO(s) + SO 2 (g)

[0671] (7)CaO(s)+water→Ca(OH) 2 (s or aq)

[0672] Example 50: Manufacturing process of precipitated calcium carbonate (1) Reaction of materials containing calcium, or magnesium, or other alkaline earth-weak acid anions with acetic acid, which may include, but is not limited to, one or more of the following or any combination thereof: ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0673] (2) Ca(CH 3 COO) 2 (aq)+SO 2 (g or aq)+H 2 O(l or aq) → CaSO 3 (s)+2CH 3 COOH(aq)

[0674] (3) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0675] (4) One or more of the following or any combination thereof: CaO+CO 2 →CaCO 3 (s) ·CaO(s)+water→Ca(OH) 2 (s or aq) Ca(OH) 2 (s or aq)+CO 2 →CaCO 3 (s or aq)

[0676] Example 51: Sodium hydroxide production from sodium bicarbonate using calcium precipitation and acid intermediates and precipitated calcium carbonate production (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0677] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0678] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0679] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0680] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0681] (2) Ca(CH 3 COO) 2 (aq)+2NaHCO 3 (aq or s) → 2NaCH 3 COO(aq) + CaCO 3 (s)+CO 2 (g)

[0682] NOTE: In some embodiments, NaHCO 3 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0683] NOTE: In some embodiments, NaHCO 3 (aq or s) may comprise a mineral, or may comprise nahconite, or any combination thereof.

[0684] NOTE: In some embodiments, NaHCO 3 (s) is Ca(CH 3 COO) 2 (aq) by dissolving in water or an aqueous solution before mixing with NaHCO 3 (aq) can be formed.

[0685] Note: CO 2 (g) is the recovered CO 2 (g) may be constituted.

[0686] NOTE: Some embodiments may form dissolved calcium bicarbonate, which in some embodiments may be decomposed into calcium carbonate and carbon dioxide by heating the solution, or by applying a vacuum to the solution, or any combination thereof.

[0687] Note: CaCO 3 (s) may constitute precipitated calcium carbonate.

[0688] Note: CaCO 3 (s) can be separated by solid-liquid separation.

[0689] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0690] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0691] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0692] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0693] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0694] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0695] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0696] (5)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0697] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0698] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0699] (6) CaSO 3 (s) → CaO(s) + SO 2 (g)

[0700] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0701] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0702] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0703] NOTE: In some embodiments, CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0704] NOTE: In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide. In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide, which may include combining step "(5)" and step "(7)".

[0705] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0706] (8) 2NaOH(aq or s) → 2NaOH(aq or s) + Water

[0707] NOTE: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution containing a higher mass percent concentration of NaOH.

[0708] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0709] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0710] Example 52: Precipitation of calcium and production of sodium hydroxide from sodium carbonate using acid intermediates and production of precipitated calcium carbonate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[0711] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0712] Note: CO 2 (g) is the recovered CO 2may be configured.

[0713] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0714] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0715] (2) Ca(CH 3 COO) 2 (aq)+Na 2 CO 3 (aq or s) → 2NaCH 3 COO(aq) + CaCO 3 (s)

[0716] NOTE: In some embodiments, Na 2 CO 3 (aq or s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0717] NOTE: In some embodiments, Na 2 CO 3 (aq or s) may comprise minerals, or may comprise decomposed nahconite, or any combination thereof.

[0718] NOTE: In some embodiments, Na 2 CO 3 (aq or s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution to form NaHCO 3 (aq or s) can be formed.

[0719] NOTE: Some embodiments may form dissolved calcium bicarbonate, which in some embodiments may be decomposed into calcium carbonate and carbon dioxide by heating the solution, or by applying a vacuum to the solution, or any combination thereof.

[0720] Note: CaCO 3 (s) may constitute precipitated calcium carbonate.

[0721] Note: CaCO 3 (s) can be separated by solid-liquid separation.

[0722] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0723] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0724] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0725] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0726] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0727] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0728] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0729] (5)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0730] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0731] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0732] (6) CaSO 3 →(s)CaO(s)+SO 2 (g)

[0733] Note: "(6)" indicates CaSO4, which may be kiln-fired. 3 (s) baking.

[0734] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(6)”.

[0735] (7) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0736] NOTE: In some embodiments, CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0737] NOTE: In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide. In some embodiments, an aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide, which may include combining step "(5)" and step "(7)".

[0738] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0739] (8) 2NaOH(aq or s) → 2NaOH(aq or s) + Water

[0740] NOTE: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution containing a higher mass percent concentration of NaOH.

[0741] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0742] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0743] Example 53: Process for the production of sodium hydroxide using sulfur dioxide and carbon dioxide intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[0744] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0745] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0746] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0747] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0748] NOTE: In some embodiments, the acetic acid in step “(1)” can include aqueous acetic acid generated or regenerated in step “(4).”

[0749] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0750] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0751] Note: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0752] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[0753] NOTE: In some embodiments, Ca(CH 3 COO) 2 (aq) is Ca(CH) from step (1). 3 COO) 2 It may contain (aq).

[0754] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0755] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0756] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH from step (2). 3 May contain COO(aq).

[0757] NOTE: In some embodiments, SO 2 is CaSO in step (9) 3 SO from the calcination or decomposition of (s) 2 (g) may be included.

[0758] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0759] Note: CH 3COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0760] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0761] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0762] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0763] (5) Reaction of weak alkaline earth acids, such as alkaline earth carbonates, with carbon dioxide and / or water to form alkaline earth bicarbonates. ·CaCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq) MgCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Mg(HCO 3 ) 2 (aq)

[0764] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be 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 any combination thereof.

[0765] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) is CaCO from step (10) 3 (s) or MgCO 3 It may include (s).

[0766] NOTE: In some embodiments, CO 2 (g or aq) is CO from step (1), or step (8), or any combination thereof. 2 may include.

[0767] (6) Reaction of alkali sulfite with alkaline earth hydrogen carbonate to form alkali hydrogen carbonate and alkaline earth sulfite. ·Na 2 SO 3 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s) ·Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[0768] NOTE: In some embodiments, Na 2 SO 3 (s) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may be dissolved in water prior to mixing with the aqueous solution containing (aq) or may form an aqueous solution.

[0769] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[0770] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[0771] NOTE: In some embodiments, Na 2 SO 3 (s or aq) is Na from step (4) 2 SO 3 may include.

[0772] NOTE: In some embodiments, Ca(HCO 3 ) 2 (aq) or Mg(HCO3 ) 2 (aq) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may contain (aq).

[0773] (7) 2NaHCO 3 (aq) → 2NaHCO 3 (s)+water

[0774] NOTE: In some embodiments, NaHCO 3 may be sold as a product and / or used as a carbon sequestration medium.

[0775] Note: In some embodiments, step “(7)” can be combined with step “(8).”

[0776] NOTE: In some embodiments, 2NaHCO 3 (aq) is a compound that is dissolved in water and / or in a pressurized or pressurized environment. 2 CO 3 (aq) and CO 2 (g) and water, which results in NaHCO 3 The need to crystallize or precipitate (s) can be avoided or prevented.

[0777] NOTE: In some embodiments, 2NaHCO 3 (aq) is the NaHCO from step (6) 3 It may contain (aq).

[0778] NOTE: In some embodiments, residual dissolved MgSO 3 Alternatively, at least a portion of the magnesium sulfite, if present, may be separated or precipitated during this process.

[0779] NOTE: Water can be separated from sodium bicarbonate or sodium carbonate using the systems and methods for water separation described herein.

[0780] NOTE: In some embodiments, steps 8 and 9 may be combined in a single step, for example, sodium bicarbonate in the aqueous phase may be decomposed into aqueous sodium carbonate and carbon dioxide, which may include recovered carbon dioxide. In some embodiments, the aqueous sodium carbonate can 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. In some embodiments, the aqueous sodium carbonate can be separated from water to produce solid sodium carbonate, and / or the solid sodium carbonate can be dissolved in water, and / or the sodium carbonate can 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.

[0781] (8)2NaHCO 3 (s) → Na 2 CO 3 (s)+CO 2 (g)+H 2 O(g or l)

[0782] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0783] NOTE: In some embodiments, Na 2 CO 3 may be sold as a product and / or used as a carbon sequestration medium.

[0784] Note: In some embodiments, step “(7)” can be combined with step “(8).”

[0785] NOTE: In some embodiments, 2NaHCO 3(aq) is a compound that is dissolved in water and / or in a pressurized or pressurized environment. 2 CO 3 (aq) and CO 2 (g) and water, which results in NaHCO 3 The need to crystallize or precipitate (s) can be avoided or prevented.

[0786] NOTE: In some embodiments, 2NaHCO 3 (s) is NaHCO from step (6) or step (7) 3 may include.

[0787] (9) Calcination or decomposition of alkaline earth sulfites to alkaline earth oxides and sulfur dioxide. ·CaSO 3 (s) → CaO(s) + SO 2 (g) MgSO 3 (s) → MgO(s) + SO 2 (g)

[0788] Note: CaSO kilns may be used. 3 (s) or MgSO 3 (s) baking.

[0789] Note: CaSO 3 (s) or MgSO 3 (s) may be dried or dehydrated or both before or during firing.

[0790] Note: CaSO 3 (s) or MgSO 3 (s) is the CaSO 3 (s) or MgSO 3 It may include (s).

[0791] (10) Reaction of alkaline earth oxides or hydroxides with alkali carbonates to produce alkaline earth carbonates and alkali hydroxides. CaO(s or aq) + Na 2 CO 3(s or aq) + water → 2NaOH(aq) + CaCO 3 (s) MgO(s or aq) + Na 2 CO 3 (s or aq) + water → 2NaOH(aq) + MgCO 3 (s)

[0792] Note: In some embodiments, CaO+Na 2 CO 3 (s or aq) + water or MgO + Na 2 CO 3 (s or aq) + water can be carried out in multiple steps. For example, in some embodiments, CaO or MgO is reacted with water to produce 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 a solid-liquid suspension containing milk of lime or milk of magnesia, or calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na 2 CO 3 may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, Ca(OH) 2 (s or aq), or milk of lime, or Mg(OH) 2 or a solution or solid-liquid mixture or suspension containing milk of magnesia, 2 CO 3 (aq) to form a solution comprising aqueous sodium hydroxide and a solid comprising calcium or magnesium carbonate.

[0793] NOTE: In some embodiments, at least a portion of the calcium carbonate or magnesium carbonate can be separated from at least a portion of the sodium hydroxide using, for example, solid-liquid separation.

[0794] NOTE: The CaO(s) or MgO(s) may include CaO(s) or MgO(s) from step “(9).”

[0795] Note: Na 2 CO 3 (s or aq) is Na from step (7) or step (8) 2 CO 3 It may contain (s or aq).

[0796] NOTE: In some embodiments, CaCO 3 or MgCO 3 can be moved to step 5.

[0797] Example 54: Process for the production of sodium hydroxide using sulfur dioxide and carbon dioxide intermediates (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) → 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[0798] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0799] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0800] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0801] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0802] NOTE: In some embodiments, the acetic acid in step “(1)” can include aqueous acetic acid generated or regenerated in step “(4).”

[0803] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0804] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0805] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0806] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[0807] NOTE: In some embodiments, Ca(CH 3 COO) 2 (aq) is Ca(CH) from step (1). 3 COO) 2 It may contain (aq).

[0808] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0809] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0810] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH from step (2). 3 May contain COO(aq).

[0811] NOTE: In some embodiments, SO 2 is CaSO in step (9) 3 SO from the calcination or decomposition of (s) 2 (g) may be included.

[0812] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0813] Note: CH 3COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0814] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0815] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0816] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0817] (5) Reaction of weak alkaline earth acids, such as alkaline earth carbonates, with carbon dioxide and / or water to form alkaline earth bicarbonates. ·CaCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq) MgCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Mg(HCO 3 ) 2 (aq)

[0818] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be 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 any combination thereof.

[0819] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) is CaCO from step (9) 3 (s) or MgCO 3 It may include (s).

[0820] NOTE: In some embodiments, CO 2 (g or aq) is CO from step (1), or step (8), or any combination thereof. 2 may include.

[0821] (6) Reaction of alkali sulfite with alkaline earth hydrogen carbonate to form alkali hydrogen carbonate and alkaline earth sulfite. ·Na 2 SO 3 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s) ·Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[0822] NOTE: In some embodiments, Na 2 SO 3 (s) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may be dissolved in water prior to mixing with the aqueous solution containing (aq) or may form an aqueous solution.

[0823] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[0824] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[0825] NOTE: In some embodiments, Na 2 SO 3 (s or aq) is Na from step (4) 2 SO 3 may include.

[0826] NOTE: In some embodiments, Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 )2 (aq) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may contain (aq).

[0827] (7) 2NaHCO 3 (aq or s) → Na 2 CO 3 (aq or s) + CO 2 (g)+H 2 O(g or l)

[0828] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0829] NOTE: In some embodiments, Na 2 CO 3 may be sold as a product and / or used as a carbon sequestration medium.

[0830] NOTE: In some embodiments, NaHCO 3 2NaHCO 3 (s) and / or 2NaHCO 3 (s) is Na 2 CO 3 (s), CO 2 and H 2 O(g or l).

[0831] NOTE: In some embodiments, Na 2 CO 3 (s) can be dissolved in water, for example, prior to reaction with, for example, calcium hydroxide or magnesium hydroxide in step 8.

[0832] NOTE: In some embodiments, 2NaHCO 3 (aq) is a compound that is dissolved in water and / or in a pressurized or pressurized environment. 2 CO 3 (aq) and CO 2 (g) and water, which results in NaHCO3 (s) and / or may avoid or prevent the need to crystallize or precipitate, e.g., CO 2 The evaporation of water during desorption can be minimized or reduced.

[0833] NOTE: In some embodiments, 2NaHCO 3 (aq) is the NaHCO from step (6) 3 may include.

[0834] (8) Calcination or decomposition of alkaline earth sulfites to alkaline earth oxides and sulfur dioxide. ·CaSO 3 →(s)CaO(s)+SO 2 (g) MgSO 3 (s) → +SO 2 (g)

[0835] Note: CaSO kilns may be used. 3 (s) or MgSO 3 (s) baking.

[0836] Note: CaSO 3 (s) or MgSO 3 (s) may be dried or dehydrated or both before or during firing.

[0837] Note: CaSO 3 (s) or MgSO 3 (s) is the CaSO 3 (s) or MgSO 3 It may include (s).

[0838] (9) Reaction of alkaline earth oxides or hydroxides with alkali carbonates to produce alkaline earth carbonates and alkali hydroxides. CaO(s or aq) + Na 2 CO 3 (s or aq) + water → 2NaOH(aq) + CaCO 3 (s) MgO(s or aq) + Na2 CO 3 (s or aq) + water → 2NaOH(aq) + MgCO 3 (s)

[0839] Note: In some embodiments, CaO+Na 2 CO 3 (s or aq) + water or MgO + Na 2 CO 3 (s or aq) + water can be carried out in multiple steps. For example, in some embodiments, CaO or MgO is reacted with water to produce 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 a solid-liquid suspension containing milk of lime or milk of magnesia, or calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na 2 CO 3 may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, Ca(OH) 2 (s or aq), or milk of lime, or Mg(OH) 2 or a solution or solid-liquid mixture or suspension containing milk of magnesia, 2 CO 3 (aq) to form a solution comprising aqueous sodium hydroxide and a solid comprising calcium or magnesium carbonate.

[0840] NOTE: In some embodiments, at least a portion of the calcium carbonate or magnesium carbonate can be separated from at least a portion of the sodium hydroxide using, for example, solid-liquid separation.

[0841] NOTE: The CaO(s) or MgO(s) may include CaO(s) or MgO(s) from step “(8).”

[0842] Note: Na 2 CO 3(aq) is Na from step (6) or step (7) 2 CO 3 It may contain (aq).

[0843] NOTE: In some embodiments, CaCO 3 or MgCO 3 can be moved to step 5.

[0844] NOTE: In some embodiments, NaOH(aq) may be concentrated or at least a portion of the water may be removed. The separated or recovered water may be transferred to step "5" or used as a solvent or input in step "5", for example. In some embodiments, NaOH(aq) may be concentrated to a concentrate, or a 33 wt% solution, or a 50 wt% solution, or solid NaOH, or any combination thereof, using one or more of the water separation systems and / or methods, or any combination thereof.

[0845] Example 55: Process for producing sodium bicarbonate and / or calcium oxide or calcium carbonate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[0846] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0847] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0848] NOTE: In some embodiments, CO 2 (g) may be used internally or in other processes. For example, in some embodiments, CO 2 (g) can be used in step (5).

[0849] NOTE: In some embodiments, CO 2 (g) may be utilized, or sequestered, or sold, or may constitute a product. For example, CO 2 (g) CO 2 Quarantine site or CO 2 It may be utilized for EOR or external uses, or sequestered, or sold.

[0850] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0851] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0852] NOTE: In some embodiments, the acetic acid in step “(1)” can include aqueous acetic acid generated or regenerated in step “(4).”

[0853] (2) Ca(CH3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0854] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0855] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0856] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[0857] NOTE: In some embodiments, Ca(CH 3 COO) 2 (aq) is Ca(CH) from step (1). 3 COO) 2 It may contain (aq).

[0858] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0859] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0860] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH from step (2). 3 May contain COO(aq).

[0861] NOTE: In some embodiments, SO 2 is CaSO in step (7) 3 SO from the calcination or decomposition of (s) 2 (g) may be included.

[0862] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0863] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0864] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0865] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0866] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0867] (5) Reaction of weak alkaline earth acids, such as alkaline earth carbonates, with carbon dioxide and / or water to form alkaline earth bicarbonates. ·CaCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq) MgCO 3 (s)+CO 2 (g or aq)+H2 O(aq) → Mg(HCO 3 ) 2 (aq)

[0868] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be 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 any combination thereof.

[0869] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) is CaCO from step (8) 3 (s) or MgCO 3 It may include (s).

[0870] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) may constitute inputs such as limestone or dolomite.

[0871] NOTE: In some embodiments, CO 2 (g or aq) is CO from step (1) 2 may include.

[0872] NOTE: In some embodiments, CO 2 (g or aq) is the CO from the emission source 2 , another CO 2 Source or captured CO 2 or any combination thereof. For example, in some embodiments, 2 (g or aq) refers to, but is not limited to, CO from blue hydrogen or blue ammonia facilities, or ammonia facilities, or ethanol plants, or carbon capture plants. 2 or any combination thereof.

[0873] (6) Reaction of alkali sulfite with alkaline earth hydrogen carbonate to form alkali hydrogen carbonate and alkaline earth sulfite. ·Na 2 SO 3 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s) ·Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[0874] NOTE: In some embodiments, Na 2 SO 3 (s) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may be dissolved in water or may form an aqueous solution prior to or during mixing with the aqueous solution containing (aq).

[0875] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[0876] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[0877] NOTE: In some embodiments, NaHCO 3 may be concentrated and / or crystallized into a solid, such as, for example, solid sodium bicarbonate or solid sodium carbonate.

[0878] (7) Decomposition of alkaline earth sulfites into alkaline earth oxides and sulfur dioxide ·CaSO 3 (s) → CaO(s) + SO 2(g) MgSO 3 (s) → +SO 2 (g)

[0879] Note: CaSO kilns may be used. 3 (s) or MgSO 3 (s) baking.

[0880] Note: CaSO 3 (s) or MgSO 3 (s) may be dried or dehydrated or both before or during firing.

[0881] Note: CaSO 3 (s) or MgSO 3 (s) is the CaSO 3 (s) or MgSO 3 It may include (s).

[0882] NOTE: CaO or MgO may constitute a value product if desired. For example, CaO or MgO may constitute an ultra-low carbon footprint CaO or MgO product. In some embodiments, calcium oxide, or calcium hydroxide, or magnesium oxide, or magnesium hydroxide, or any combination thereof may constitute 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 constitute a product or may be sold or may be sold from exemplary embodiments of the present invention.

[0883] (8) Reaction of alkaline earth oxides or hydroxides with carbon dioxide to form alkaline earth carbonates. CaO(s)+CO 2 (g) → CaCO 3 (s) MgO+CO 2 (g) → MgCO 3 (s) CaO(s)+H 2 O → Ca(OH)2 (s or aq) MgO(s)+H 2 O → Mg(OH) 2 (s or aq) Ca(OH) 2 (s or aq)+CO 2 (g) → CaCO 3 (s)+H 2 O Mg(OH) 2 (s or aq)+CO 2 (g) → MgCO 3 (s)+H 2 O

[0884] NOTE: In some embodiments, CaO(s) or MgO(s) reacts 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 containing calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH) 2 or Mg(OH) 2 reacts with carbonates such as sodium carbonate or sodium bicarbonate to produce CaCO 3 or MgCO 3 or CO 2 Reacts with CaCO 3 or MgCO 3 For example, the sodium carbonate or sodium bicarbonate may form CO 2 In the absorption solution or CO 2 The absorbent solution used may include sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassium bicarbonate, or an alkali carbonate, or an alkali bicarbonate, or any combination thereof.

[0885] NOTE: In some embodiments, CO 2 (g) is a point source of CO 2 CO in or from the emission source2 For example, CO 2 (g) Flue gas or dilute CO 2 , or high purity CO 2 or captured CO 2 may include.

[0886] NOTE: In some embodiments, CO 2 (g) CO in or derived from air 2 For example, CO 2 (g) At least a certain amount of CO is generated even at very low concentrations. 2 For example, calcium oxide can be used to create air that can contain very low or very dilute concentrations of CO, if desired. 2 For example, CO 2 (g) may include carbonates such as sodium or potassium carbonate, which may include carbonates derived from the reaction of carbon dioxide in the air with sodium or potassium or other alkali salts, such as sodium or potassium hydroxide, to form alkali carbonates, and / or may include carbonates derived from the reaction of calcium oxide or hydroxide with alkali carbonates to regenerate or form alkali hydroxides or alkali oxides or other alkali salts that can be used to absorb carbon dioxide from the air to regenerate or reform the alkali carbonates.

[0887] NOTE: In some embodiments, CaCO 3 or MgCO 3 may constitute a valuable resource. In some embodiments, CaCO 3 or MgCO 3 may constitute precipitated calcium carbonate. In some embodiments, CaCO 3 or MgCO 3 may constitute a carbon sequestration medium.

[0888] NOTE: In some embodiments, for example and without limitation, Example 53, or Example 54, or Example 55, or Example 61, or Example 62, or any combination thereof, may include separate and / or simultaneous processes. For example, in some embodiments, the CO generated in step "(1)" of Example 53 or Example 54 may be used. 2 may constitute input to Example 55.

[0889] Example 56: Process for the production of calcium carbonate from Ca(WA) using ammonium chloride intermediate (1) Reaction of ammonium chloride with materials containing calcium, magnesium, or other alkaline earth weak acid anions Ca(WA)(s)+2NH 4 Cl(s or g or aq) → CaCl 2 (s or aq)+2NH 3 (g or aq)+H 2 O(g or aq)

[0890] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid phase or in a mixed solid-gas phase. For example, 2NH 4 Heating Cl(s) and Ca(WA)(s) produces NH 4 Cl to NH 3 (g) and HCl(g), which reacts with Ca(WA)(s) to produce, for example, CaCl 2 It may form (s) and / or (WA) and / or water.

[0891] NOTE: In some embodiments, the WA may include, for example, but not limited to, one or more of silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide, or any combination thereof.

[0892] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid-liquid or solid-aqueous phase. For example, 2NH 4Cl(aq) and Ca(WA)(s) can be mixed and / or reacted to produce, for example, CaCl 2 (aq) and 2NH 3 (aq or g) can be formed.

[0893] (2) CaCl 2 (s)+water→CaCl 2 (aq)

[0894] NOTE: In some embodiments, CaCl from step 1 is added. 2 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[0895] (3) Ammonia or a weak base can be dissolved in water or an aqueous solution to form aqueous ammonia, and / or ammonia can be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate. CaCl 2 (aq)+2NH 3 (g) → CaCl 2 (aq)+2NH 3 (aq) 2NH 3 (g)+water→NH 3 (aq) 2NH 3 (g or aq)+CO 2 (g)+H 2 O(l or aq) → (NH 4 ) 2 CO 3 (aq) 2NH 3 (g or aq) + 2CO 2 (g)+2H 2 O(l or aq) → 2NH 4 HCO 3 (aq) ·(NH 4 ) 2 CO 3 (aq)+CO 2 (g)+H 2 O(l or aq) → 2NH 4 HCO 3 (aq)

[0896] NOTE: In some embodiments, the NH from step 1 3 may contain gas and / or CaCl 2 It can be dissolved in (aq).

[0897] NOTE: In some embodiments, NH 3 can be dissolved in water and / or CaCl 2 Apart from CO 2 It can react with.

[0898] (4) Calcium chloride can react with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate. CaCl 2 (aq)+2NH 3 (aq)+CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 3 (aq) + 2CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g) CaCl 2 (aq)+(NH 4 ) 2 CO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 4 HCO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g)

[0899] NOTE: In some embodiments, excess CO2 is present or CO 2 In some embodiments, when the excess CO 2 can be transferred to an input or reactant for step 4 and / or an input or reactant for step 3.

[0900] NOTE: In some embodiments, CaCl 2 (aq)+NH 3 The (aq) solution can be generated in step 1 and / or transferred to step 4, optionally steps 2 and 3 can be skipped.

[0901] NOTE: In some embodiments, CO 2 (g) is a recovered CO2 from another embodiment described herein. 2 For example, in some embodiments, CO 2 (g) CO from the reaction of calcium carbonate with acetic acid 2 may include.

[0902] NOTE: In some embodiments, CaCO 3 (s) may be transferred to or constitute input into one or more of the embodiments described herein or any combination thereof. For example, CaCO 3 (s) may be an input to a process to produce sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[0903] NOTE: In some embodiments, CO 2 (g) CO from emission sources, or point sources, or air, or external sources, or any combination thereof 2 may include.

[0904] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 1.

[0905] NOTE: In some embodiments, 2NH 4Cl(aq) can be transferred to step 5.

[0906] (5) 2NH 4 Cl(aq) → 2NH 4 Cl(s)+water

[0907] NOTE: In some embodiments, 2NH 4 Cl(s) can be transferred to step 1.

[0908] NOTE: In some embodiments, water may be transferred to step 3 and / or step 4.

[0909] NOTE: In some embodiments, this exemplary embodiment may 2 Conversion of CO 2 To further enhance the removal potential of CO or CO leaving the process 2 This embodiment may be integrated with other embodiments described herein to allow for the production of chemicals without the need for the output of Ca(WA) or to allow for the use of other Ca(WA) inputs or less reactive Ca(WA) inputs, or any combination thereof. For example, in some embodiments, CaCO 3 may be transferred from this embodiment to the second embodiment, and then the CO captured from the second embodiment may be 2 For example, in some embodiments, CO transferred between this embodiment and the second embodiment 2 may constitute an intermediate in the manufacture of chemicals such as, but not limited to, one or more of sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof, or any combination thereof. For example, in some embodiments, CO in the production of CaCO 2 CaCO may be from an emission source or from the air and / or may be manufactured. 3can be transferred from this embodiment to a second embodiment, such as an embodiment for producing sodium carbonate or sodium bicarbonate, thereby reducing the net CO 2 Conversion or CO 2 The chances of removal can be increased.

[0910] Example 57: Process for the production of alkali hydroxide using carbon dioxide and / or sulfur dioxide intermediates (1) Reaction of ammonium chloride with materials containing calcium, magnesium, or other alkaline earth weak acid anions Ca(WA)(s)+2NH 4 Cl(s or g or aq) → CaCl 2 (s or aq)+2NH 3 (g or aq)+H 2 O(g or aq)

[0911] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid phase or in a mixed solid-gas phase. For example, 2NH 4 Heating Cl(s) and Ca(WA)(s) produces NH 4 Cl to NH 3 (g) and HCl(g), which reacts with Ca(WA)(s) to produce, for example, CaCl 2 It may form (s) and / or (WA) and / or water.

[0912] NOTE: In some embodiments, the WA may include, for example, but not limited to, one or more of silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide, or any combination thereof.

[0913] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid-liquid or solid-aqueous phase. For example, 2NH 4 Cl(aq) and Ca(WA)(s) can be mixed and / or reacted to produce, for example, CaCl 2 (aq) and 2NH 3(aq or g) can be formed.

[0914] (2) CaCl 2 (s)+water→CaCl 2 (aq)

[0915] NOTE: In some embodiments, CaCl from step 1 is added. 2 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[0916] (3) Ammonia or a weak base can be dissolved in water or an aqueous solution to form aqueous ammonia, and / or ammonia can be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate. CaCl 2 (aq)+2NH 3 (g) → CaCl 2 (aq)+2NH 3 (aq) 2NH 3 (g)+water→NH 3 (aq) 2NH 3 (g or aq)+CO 2 (g)+H 2 O(l or aq) → (NH 4 ) 2 CO 3 (aq) 2NH 3 (g or aq) + 2CO 2 (g)+2H 2 O(l or aq) → 2NH 4 HCO 3 (aq) ·(NH 4 ) 2 CO 3 (aq)+CO 2 (g)+H 2 O(l or aq) → 2NH 4 HCO 3 (aq)

[0917] NOTE: In some embodiments, the NH from step 1 3 may contain gas and / or CaCl2 It can be dissolved in (aq).

[0918] NOTE: In some embodiments, NH 3 can be dissolved in water and / or CaCl 2 Apart from CO 2 It can react with.

[0919] (4) Calcium chloride can react with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate. CaCl 2 (aq)+2NH 3 (aq)+CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 3 (aq) + 2CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g) CaCl 2 (aq)+(NH 4 ) 2 CO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 4 HCO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g)

[0920] NOTE: In some embodiments, excess CO 2 is present or CO 2 In some embodiments, when the excess CO 2can be transferred to an input or reactant for step 4 and / or an input or reactant for step 3.

[0921] NOTE: In some embodiments, CaCl 2 (aq)+NH 3 The (aq) solution can be generated in step 1 and / or transferred to step 4, optionally steps 2 and 3 can be skipped.

[0922] NOTE: In some embodiments, CO 2 (g) is a recovered CO2 from another embodiment described herein. 2 For example, in some embodiments, CO 2 (g) CO from the reaction of calcium carbonate with acetic acid 2 may include.

[0923] NOTE: In some embodiments, CaCO 3 (s) may be transferred to or constitute input into one or more of the embodiments described herein or any combination thereof. For example, CaCO 3 (s) may be an input to a process to produce sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[0924] NOTE: In some embodiments, CO 2 (g) CO from emission sources, or point sources, or air, or external sources, or any combination thereof 2 may include.

[0925] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 1.

[0926] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 5.

[0927] (5) 2NH 4Cl(aq) → 2NH 4 Cl(s)+water

[0928] NOTE: In some embodiments, 2NH 4 Cl(s) can be transferred to step 1.

[0929] NOTE: In some embodiments, water may be transferred to step 3 and / or step 4.

[0930] (6) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(l or aq) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(l or aq) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g)+H 2 O(l or aq) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(l or aq)

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

[0932] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0933] NOTE: In some embodiments, CO 2 can be moved to step 4.

[0934] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0935] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0936] (7)Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0937] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0938] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0939] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) is provided or supplied as Na 2 SO 4 (aq) may be formed.

[0940] (8)2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0941] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0942] (9)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[0943] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0944] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[0945] NOTE: In some embodiments, Na 2 SO3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (9). In some embodiments, magnesium sulfite solids may be separated during step "(9)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[0946] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0947] (10)Na 2 SO 3 (s or aq) + Ca(OH) 2 (s or aq) → 2NaOH(aq or s) + CaSO 3 (s)

[0948] Note: Ca(OH) 2 (s or aq) may constitute a solid-liquid suspension such as milk of lime.

[0949] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[0950] (11)CaSO 3 (s) → CaO(s) + SO 2 (g)

[0951] Note: "(11)" is CaSO, which may be kiln-fired.3 (s) baking.

[0952] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(11)”.

[0953] (12) CaO(s) + water (g or l or aq) → Ca(OH) 2 (s or aq)

[0954] NOTE: In some embodiments, CaO(s) is CaSO 3 To remove water vapor before or during the decomposition of CaO(s) into CaO(s), or CaSO 3 It can be used to accelerate the drying of (s).

[0955] NOTE: In some embodiments, the aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide. In some embodiments, the aqueous solution containing sodium sulfite can be reacted directly with calcium oxide to produce calcium sulfite and sodium hydroxide, which may include combining step "(10)" and step "(12)".

[0956] NOTE: In some embodiments, calcium oxide can be reacted with water to produce an aqueous solution containing calcium hydroxide, or a solid-liquid suspension, or milk of lime, or a solid, or any combination thereof.

[0957] (13) 2NaOH(aq or s) → 2NaOH(aq or s) + Water

[0958] NOTE: In some embodiments, NaOH(aq) may be concentrated into an aqueous solution containing a higher mass percent concentration of NaOH.

[0959] NOTE: In some embodiments, water can be removed and / or NaOH can be separated or precipitated, such as, but not limited to, by evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0960] NOTE: In some embodiments, it may be desirable for NaOH to constitute a concentrated aqueous solution.

[0961] Example 58: Process for the production of alkali hydroxide using carbon dioxide, alkali carbonate and / or sulfur dioxide intermediates (1) Reaction of ammonium chloride with materials containing calcium, magnesium, or other alkaline earth weak acid anions Ca(WA)(s)+2NH 4 Cl(s or g or aq) → CaCl 2 (s or aq)+2NH 3 (g or aq)+H 2 O(g or aq)

[0962] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid phase or in a mixed solid-gas phase. For example, 2NH 4 Heating Cl(s) and Ca(WA)(s) produces NH 4 Cl to NH 3 (g) and HCl(g), which reacts with Ca(WA)(s) to produce, for example, CaCl 2 It may form (s) and / or (WA) and / or water.

[0963] NOTE: In some embodiments, the WA may include, for example, but not limited to, one or more of silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide, or any combination thereof.

[0964] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid-liquid or solid-aqueous phase. For example, 2NH 4 Cl(aq) and Ca(WA)(s) can be mixed and / or reacted to produce, for example, CaCl 2 (aq) and 2NH 3 (aq or g) can be formed.

[0965] (2) CaCl 2 (s)+water→CaCl 2 (aq)

[0966] NOTE: In some embodiments, CaCl from step 1 is added. 2 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[0967] (3) Ammonia or a weak base can be dissolved in water or an aqueous solution to form aqueous ammonia, and / or ammonia can be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate. CaCl 2 (aq)+2NH 3 (g) → CaCl 2 (aq)+2NH 3 (aq) 2NH 3 (g)+water→NH 3 (aq) 2NH 3 (g or aq)+CO 2 (g)+H 2 O(l or aq) → (NH 4 ) 2 CO 3 (aq) 2NH 3 (g or aq) + 2CO 2 (g)+2H 2 O(l or aq) → 2NH 4 HCO 3 (aq) ·(NH 4 ) 2 CO 3 (aq)+CO 2 (g)+H2 O(l or aq) → 2NH 4 HCO 3 (aq)

[0968] NOTE: In some embodiments, the NH from step 1 3 may contain gas and / or CaCl 2 It can be dissolved in (aq).

[0969] NOTE: In some embodiments, NH 3 can be dissolved in water and / or CaCl 2 Apart from CO 2 It can react with.

[0970] (4) Calcium chloride can react with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate. CaCl 2 (aq)+2NH 3 (aq)+CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 3 (aq) + 2CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g) CaCl 2 (aq)+(NH 4 ) 2 CO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 4 HCO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g)

[0971] NOTE: In some embodiments, excess CO 2 is present or CO 2 In some embodiments, when the excess CO 2 can be transferred to an input or reactant for step 4 and / or an input or reactant for step 3.

[0972] NOTE: In some embodiments, CaCl 2 (aq)+NH 3 The (aq) solution can be generated in step 1 and / or transferred to step 4, optionally steps 2 and 3 can be skipped.

[0973] NOTE: In some embodiments, CO 2 (g) is a recovered CO2 from another embodiment described herein. 2 For example, in some embodiments, CO 2 (g) CO from the reaction of calcium carbonate with acetic acid 2 may include.

[0974] NOTE: In some embodiments, CaCO 3 (s) may be transferred to or constitute input into one or more of the embodiments described herein or any combination thereof. For example, CaCO 3 (s) may be an input to a process to produce sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[0975] NOTE: In some embodiments, CO 2 (g) CO from emission sources, or point sources, or air, or external sources, or any combination thereof 2 may include.

[0976] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 1.

[0977] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 5.

[0978] (5) 2NH 4 Cl(aq) → 2NH 4 Cl(s)+water

[0979] NOTE: In some embodiments, 2NH 4 Cl(s) can be transferred to step 1.

[0980] NOTE: In some embodiments, water may be transferred to step 3 and / or step 4.

[0981] (6) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[0982] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[0983] Note: CO 2 (g) is the recovered CO 2 may be configured.

[0984] NOTE: In some embodiments, CO 2 can be moved to step 4.

[0985] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[0986] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[0987] NOTE: In some embodiments, the acetic acid in step “(6)” can include aqueous acetic acid generated or regenerated in step “(9).”

[0988] (7)Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[0989] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[0990] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2(aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[0991] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[0992] NOTE: In some embodiments, Ca(CH 3 COO) 2 (aq) is Ca(CH) from step (6). 3 COO) 2 It may contain (aq).

[0993] (8)2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[0994] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[0995] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH 3 May contain COO(aq).

[0996] NOTE: In some embodiments, SO 2 is CaSO in step (14) 2 SO from the calcination or decomposition of (s) 3 (g) may be included.

[0997] (9)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH3 COOH(aq)+Na 2 SO 3 (s)

[0998] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[0999] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to obtain Na. 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[1000] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (9). In some embodiments, magnesium sulfite solids may be separated during step "(9)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[1001] Note: Na2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1002] (10) Reaction of alkaline earth weak acids, such as alkaline earth carbonates, with carbon dioxide and / or water to form alkaline earth bicarbonates. ·CaCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq) MgCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Mg(HCO 3 ) 2 (aq)

[1003] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be 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 any combination thereof.

[1004] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) is CaCO from step (14) 3 (s) or MgCO 3 It may include (s).

[1005] NOTE: In some embodiments, CO 2(g or aq) is CO from step (6), or step (13), or any combination thereof. 2 may include.

[1006] (11) Reaction of alkali sulfite with alkaline earth hydrogen carbonate to form alkali hydrogen carbonate and alkaline earth sulfite. ·Na 2 SO 3 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s) ·Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[1007] NOTE: In some embodiments, Na 2 SO 3 (s) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may be dissolved in water prior to mixing with the aqueous solution containing (aq) or may form an aqueous solution.

[1008] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[1009] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[1010] NOTE: In some embodiments, Na 2 SO 3 (s or aq) is Na from step (4) 2 SO 3 may include.

[1011] NOTE: In some embodiments, Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 (aq) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may contain (aq).

[1012] (12)2NaHCO 3 (aq) → Na 2 CO 3 (aq)+CO 2 (g)+H 2 O(g or l)

[1013] Note: CO 2 (g) is the recovered CO 2 may be configured.

[1014] NOTE: In some embodiments, Na 2 CO 3 may be sold as a product and / or used as a carbon sequestration medium.

[1015] NOTE: In some embodiments, 2NaHCO 3 (aq) is a compound that is dissolved in water and / or in a pressurized or pressurized environment. 2 CO 3 (aq) and CO 2 (g) and water, which results in NaHCO 3 (s) and / or may avoid or prevent the need to crystallize or precipitate, e.g., CO 2 The evaporation of water during desorption can be minimized or reduced.

[1016] NOTE: In some embodiments, 2NaHCO 3 (aq) is the NaHCO from step (11) 3 may include.

[1017] (13) Calcination or decomposition of alkaline earth sulfites to alkaline earth oxides and sulfur dioxide. ·CaSO 3 (s) → CaO(s) + SO 2 (g) MgSO 3 (s) → MgO(s) + SO 2 (g)

[1018] Note: CaSO kilns may be used. 3 (s) or MgSO 3 (s) baking.

[1019] Note: CaSO 3 (s) or MgSO 3 (s) may be dried or dehydrated or both before or during firing.

[1020] Note: CaSO 3 (s) or MgSO 3 (s) is CaSO from step (11) 3 (s) or MgSO 3 It may include (s).

[1021] (14) Reaction of alkaline earth oxides or hydroxides with alkali carbonates to produce alkaline earth carbonates and alkali hydroxides. CaO(s or aq) + Na 2 CO 3 (s or aq) + water → NaOH(aq) + CaCO 3 (s) MgO(s or aq) + Na 2 CO 3 (s or aq) + water → NaOH(aq) + MgCO 3 (s)

[1022] Note: In some embodiments, CaO+Na 2 CO 3 (s or aq) + water or MgO + Na 2 CO 3(s or aq) + water can be carried out in multiple steps. For example, in some embodiments, CaO or MgO is reacted with water to produce 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 a solid-liquid suspension containing milk of lime or milk of magnesia, or calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na 2 CO 3 may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, Ca(OH) 2 (s or aq), or milk of lime, or Mg(OH) 2 or a solution or solid-liquid mixture or suspension containing milk of magnesia, 2 CO 3 (aq) to form a solution comprising aqueous sodium hydroxide and a solid comprising calcium or magnesium carbonate.

[1023] NOTE: In some embodiments, at least a portion of the calcium carbonate or magnesium carbonate can be separated from at least a portion of the sodium hydroxide using, for example, solid-liquid separation.

[1024] NOTE: The CaO(s) or MgO(s) may include CaO(s) or MgO(s) from step “(13).”

[1025] Note: Na 2 CO 3 (aq) is Na from step (11) or step (12) 2 CO 3 It may contain (aq).

[1026] NOTE: In some embodiments, CaCO 3 or MgCO 3 may be transferred to step 10.

[1027] NOTE: In some embodiments, NaOH(aq) may be concentrated or at least a portion of the water may be removed. The separated or recovered water may be transferred to step "10" or used as a solvent or input in step "10", for example. In some embodiments, NaOH(aq) may be concentrated to a concentrate, or a 33 wt% solution, or a 50 wt% solution, or solid NaOH, or any combination thereof, using one or more of the water separation systems and / or methods, or any combination thereof.

[1028] Example 59: Process for producing alkaline earth oxides or alkaline earth hydroxides using carbon dioxide, sulfur dioxide and / or alkaline intermediates (1) Reaction of ammonium chloride with materials containing calcium, magnesium, or other alkaline earth weak acid anions Ca(WA)(s)+2NH 4 Cl(s or g or aq) → CaCl 2 (s or aq)+2NH 3 (g or aq)+H 2 O(g or aq)

[1029] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid phase or in a mixed solid-gas phase. For example, 2NH 4 Heating Cl(s) and Ca(WA)(s) produces NH 4 Cl to NH 3 (g) and HCl(g), which reacts with Ca(WA)(s) to produce, for example, CaCl 2 It may form (s) and / or (WA) and / or water.

[1030] NOTE: In some embodiments, the WA may include, for example, but not limited to, one or more of silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide, or any combination thereof.

[1031] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid-liquid or solid-aqueous phase. For example, 2NH 4 Cl(aq) and Ca(WA)(s) can be mixed and / or reacted to produce, for example, CaCl 2 (aq) and 2NH 3 (aq or g) can be formed.

[1032] (2) CaCl 2 (s)+water→CaCl 2 (aq)

[1033] NOTE: In some embodiments, CaCl from step 1 is added. 2 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[1034] (3) Ammonia or a weak base can be dissolved in water or an aqueous solution to form aqueous ammonia, and / or ammonia can be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate. CaCl 2 (aq)+2NH 3 (g) → CaCl 2 (aq)+2NH 3 (aq) 2NH 3 (g)+water→NH 3 (aq) 2NH 3 (g or aq)+CO 2 (g)+H 2 O(l or aq) → (NH 4 ) 2 CO 3 (aq) 2NH 3 (g or aq) + 2CO 2 (g)+2H 2 O(l or aq) → 2NH 4 HCO 3 (aq) ·(NH 4 ) 2 CO 3 (aq)+CO 2 (g)+H2 O(l or aq) → 2NH 4 HCO 3 (aq)

[1035] NOTE: In some embodiments, the NH from step 1 3 may contain gas and / or CaCl 2 It can be dissolved in (aq).

[1036] NOTE: In some embodiments, NH 3 can be dissolved in water and / or CaCl 2 Apart from CO 2 It can react with.

[1037] (4) Calcium chloride can react with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate. CaCl 2 (aq)+2NH 3 (aq)+CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 3 (aq) + 2CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g) CaCl 2 (aq)+(NH 4 ) 2 CO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 4 HCO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g)

[1038] NOTE: In some embodiments, excess CO 2 is present or CO 2 In some embodiments, when the excess CO 2 can be transferred to an input or reactant for step 4 and / or an input or reactant for step 3.

[1039] NOTE: In some embodiments, CaCl 2 (aq)+NH 3 The (aq) solution can be generated in step 1 and / or transferred to step 4, optionally steps 2 and 3 can be skipped.

[1040] NOTE: In some embodiments, CO 2 (g) is a recovered CO2 from another embodiment described herein. 2 For example, in some embodiments, CO 2 (g) CO from the reaction of calcium carbonate with acetic acid 2 may include.

[1041] NOTE: In some embodiments, CaCO 3 (s) may be transferred to or constitute input into one or more of the embodiments described herein or any combination thereof. For example, CaCO 3 (s) may be an input to a process to produce sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[1042] NOTE: In some embodiments, CO 2 (g) CO from emission sources, or point sources, or air, or external sources, or any combination thereof 2 may include.

[1043] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 1.

[1044] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 5.

[1045] (5) 2NH 4 Cl(aq) → 2NH 4 Cl(s)+water

[1046] NOTE: In some embodiments, 2NH 4 Cl(s) can be transferred to step 1.

[1047] NOTE: In some embodiments, water may be transferred to step 3 and / or step 4.

[1048] (6) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, g, l, or aq)

[1049] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[1050] Note: CO 2 (g) When CO is generated,2 (g) High partial pressure CO 2 (g) or purity CO 2 CO generated or captured in (g) 2 It may be desirable to include (g).

[1051] Note: CaCO 3 can be from step "4".

[1052] Note: CO 2 can be transferred to step "3" or step "4".

[1053] (7)Ca(CH 3 COO) 2 (aq)+Na 2 SO 3 (s or aq) → 2NaCH 3 COO(aq)+CaSO 3 (s)

[1054] Note: CaSO 3 (s) can be separated using solid-liquid separation.

[1055] NOTE: In some embodiments, Na 2 SO 3 (s or aq) may comprise a solid containing sodium sulfite, which may be added to or dissolved in a solution containing calcium acetate.

[1056] NOTE: In some embodiments, Na 2 SO 3 (s or aq) may comprise an aqueous solution containing sodium sulfite and acetic acid.

[1057] (8)2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[1058] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[1059] (9)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq or l)+Na 2 SO 3 (s)

[1060] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1061] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to give Na 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[1062] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (9). In some embodiments, magnesium sulfite solids may be separated during step "(9)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[1063] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1064] NOTE: In some embodiments, the feed solution containing sodium sulfite and acetic acid can be distilled off, where a portion of the acetic acid and water vapor evaporates and / or condenses to form a separate acetic acid solution, and / or a remaining solution containing aqueous acetic acid and a higher concentration of sodium sulfite than the sodium sulfite concentration in the feed solution.

[1065] (10)CaSO 3 (s) → CaO(s) + SO 2 (g)

[1066] Note: "(10)" is CaSO, which may be kiln-fired. 3 (s) baking.

[1067] Note: CaSO 3 (s) may be dried or dehydrated, or both, before or during “(10)”.

[1068] Example 60: Process for producing alkali carbonate or alkali hydrogen carbonate using carbon dioxide, alkali carbonate and / or sulfur dioxide intermediates (1) Reaction of ammonium chloride with materials containing calcium, magnesium, or other alkaline earth weak acid anions Ca(WA)(s)+2NH 4 Cl(s or g or aq) → CaCl 2 (s or aq)+2NH 3 (g or aq)+H 2 O(g or aq)

[1069] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid phase or in a mixed solid-gas phase. For example, 2NH 4 Heating Cl(s) and Ca(WA)(s) produces NH 4 Cl to NH 3 (g) and HCl(g), which reacts with Ca(WA)(s) to produce, for example, CaCl 2 It may form (s) and / or (WA) and / or water.

[1070] NOTE: In some embodiments, the WA may include, for example, but not limited to, one or more of silicon oxide, or iron oxide, or aluminum oxide, or hydroxide, or oxide, or any combination thereof.

[1071] NOTE: In some embodiments, the reaction of Ca(WA) with ammonium chloride can be carried out in the solid-liquid or solid-aqueous phase. For example, 2NH 4 Cl(aq) and Ca(WA)(s) can be mixed and / or reacted to produce, for example, CaCl 2 (aq) and 2NH 3 (aq or g) can be formed.

[1072] (2) CaCl 2 (s)+water→CaCl 2 (aq)

[1073] NOTE: In some embodiments, CaCl from step 1 is added. 2 may comprise a solid and / or may be dissolved in water to form an aqueous solution.

[1074] (3) Ammonia or a weak base can be dissolved in water or an aqueous solution to form aqueous ammonia, and / or ammonia can be dissolved in water and / or reacted with carbon dioxide to form ammonium carbonate or ammonium bicarbonate. CaCl 2 (aq)+2NH 3 (g) → CaCl 2 (aq)+2NH 3 (aq) 2NH 3 (g)+water→NH 3 (aq) 2NH 3 (g or aq)+CO 2 (g)+H 2 O(l or aq) → (NH 4 ) 2 CO 3 (aq) 2NH 3 (g or aq) + 2CO 2(g)+2H 2 O(l or aq) → 2NH 4 HCO 3 (aq) ·(NH 4 ) 2 CO 3 (aq)+CO 2 (g)+H 2 O(l or aq) → 2NH 4 HCO 3 (aq)

[1075] NOTE: In some embodiments, the NH from step 1 3 may contain gas and / or CaCl 2 It can be dissolved in (aq).

[1076] NOTE: In some embodiments, NH 3 can be dissolved in water and / or CaCl 2 Apart from CO 2 It can react with.

[1077] (4) Calcium chloride can react with ammonia, or carbon dioxide, or ammonium carbonate, or ammonium bicarbonate, or any combination thereof to form ammonium chloride and calcium carbonate. CaCl 2 (aq)+2NH 3 (aq)+CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s) CaCl 2 (aq)+2NH 3 (aq) + 2CO 2 (g)+H 2 O→2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g) CaCl 2 (aq)+(NH 4 ) 2 CO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3(s) CaCl 2 (aq)+2NH 4 HCO 3 (aq) → 2NH 4 Cl(aq)+CaCO 3 (s)+CO 2 (g)

[1078] NOTE: In some embodiments, excess CO 2 is present or CO 2 In some embodiments, when the excess CO 2 can be transferred to an input or reactant for step 4 and / or an input or reactant for step 3.

[1079] NOTE: In some embodiments, CaCl 2 (aq)+NH 3 The (aq) solution can be generated in step 1 and / or transferred to step 4, optionally steps 2 and 3 can be skipped.

[1080] NOTE: In some embodiments, CO 2 (g) is a recovered CO2 from another embodiment described herein. 2 For example, in some embodiments, CO 2 (g) CO from the reaction of calcium carbonate with acetic acid 2 may include.

[1081] NOTE: In some embodiments, CaCO 3 (s) may be transferred to or constitute input into one or more of the embodiments described herein or any combination thereof. For example, CaCO 3 (s) may be an input to a process to produce sodium hydroxide, or calcium oxide, or calcium hydroxide, or sodium bicarbonate, or sodium carbonate, or any combination thereof.

[1082] NOTE: In some embodiments, CO 2(g) CO from emission sources, or point sources, or air, or external sources, or any combination thereof 2 may include.

[1083] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 1.

[1084] NOTE: In some embodiments, 2NH 4 Cl(aq) can be transferred to step 5.

[1085] (5) 2NH 4 Cl(aq) → 2NH 4 Cl(s)+water

[1086] NOTE: In some embodiments, 2NH 4 Cl(s) can be transferred to step 1.

[1087] NOTE: In some embodiments, water may be transferred to step 3 and / or step 4.

[1088] (6) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[1089] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[1090] Note: CaCO 3 can be from step "4".

[1091] Note: CO 2 (g) is the recovered CO 2 may be configured.

[1092] NOTE: In some embodiments, CO 2 (g) may be used internally or in other processes. For example, in some embodiments, CO 2 (g) can be used in step (10).

[1093] NOTE: In some embodiments, CO 2 (g) may be utilized, or sequestered, or sold, or may constitute a product. For example, CO 2 (g) CO 2 Quarantine site or CO 2 It may be utilized for EOR or external uses, or sequestered, or sold.

[1094] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[1095] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[1096] NOTE: In some embodiments, the acetic acid in step “(6)” can include aqueous acetic acid generated or regenerated in step “(9).”

[1097] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[1098] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[1099] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[1100] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[1101] NOTE: In some embodiments, Ca(CH 3 COO) 2 (aq) is Ca(CH) from step (6). 3 COO) 2 It may contain (aq).

[1102] (8)2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[1103] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[1104] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH 3 May contain COO(aq).

[1105] NOTE: In some embodiments, SO 2 is CaSO in step (12) 2 SO from the calcination or decomposition of (s) 3 (g) may be included.

[1106] (9)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[1107] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1108] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to give Na 2 SO 3In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[1109] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3 Precipitation or crystallization may begin prior to (9). In some embodiments, magnesium sulfite solids may be separated during step "(9)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[1110] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1111] (10) Reaction of alkaline earth weak acids, such as alkaline earth carbonates, with carbon dioxide and / or water to form alkaline earth bicarbonates. ·CaCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Ca(HCO 3 ) 2 (aq) MgCO 3 (s)+CO 2 (g or aq)+H2 O(aq) → Mg(HCO 3 ) 2 (aq)

[1112] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be 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 any combination thereof.

[1113] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) is CaCO from step (13) 3 (s) or MgCO 3 It may include (s).

[1114] NOTE: In some embodiments, CaCO 3 (s) or MgCO 3 (s) may constitute inputs such as limestone or dolomite.

[1115] NOTE: In some embodiments, CO 2 (g or aq) is CO from step (6) 2 may include.

[1116] NOTE: In some embodiments, CO 2 (g or aq) is the CO from the emission source 2 , another CO 2 Source or captured CO 2 or any combination thereof. For example, in some embodiments, 2 (g or aq) refers to, but is not limited to, CO from blue hydrogen or blue ammonia facilities, or ammonia facilities, or ethanol plants, or carbon capture plants. 2 or any combination thereof.

[1117] (11) Reaction of alkali sulfite with alkaline earth hydrogen carbonate to form alkali hydrogen carbonate and alkaline earth sulfite. ·Na 2 SO 3 (s or aq) + Ca(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+CaSO 3 (s) ·Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[1118] NOTE: In some embodiments, Na 2 SO 3 (s) is Ca(HCO 3 ) 2 (aq) or Mg(HCO 3 ) 2 It may be dissolved in water or may form an aqueous solution prior to or during mixing with the aqueous solution containing (aq).

[1119] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[1120] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[1121] NOTE: In some embodiments, NaHCO 3 may be concentrated and / or crystallized into a solid, such as, for example, solid sodium bicarbonate or solid sodium carbonate.

[1122] (12) Decomposition of alkaline earth sulfites to alkaline earth oxides and sulfur dioxide ·CaSO 3 (s) → CaO(s) + SO2 (g) MgSO 3 (s) → MgO(s) + SO 2 (g)

[1123] Note: CaSO kilns may be used. 3 (s) or MgSO 3 (s) baking.

[1124] Note: CaSO 3 (s) or MgSO 3 (s) may be dried or dehydrated or both before or during firing.

[1125] Note: CaSO 3 (s) or MgSO 3 (s) is CaSO from step (11) 3 (s) or MgSO 3 It may include (s).

[1126] Note: CaO or MgO may constitute a value product if desired. For example, CaO or MgO may constitute a very low carbon footprint CaO or MgO product.

[1127] (13) Reaction of alkaline earth oxides or hydroxides with carbon dioxide to form alkaline earth carbonates. CaO(s)+CO 2 (g) → CaCO 3 (s) MgO(s)+CO 2 (g) → MgCO 3 (s)

[1128] NOTE: In some embodiments, CaO(s) or MgO(s) reacts 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 containing calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH) 2 or Mg(OH) 2 reacts with carbonates such as sodium carbonate or sodium bicarbonate to produce CaCO 3 or MgCO 3 or CO 2 Reacts with CaCO 3 Or MgCO 3 For example, the sodium carbonate or sodium bicarbonate may form CO 2 In the absorption solution or CO 2 The absorbent solution used may include sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassium bicarbonate, or an alkali carbonate, or an alkali bicarbonate, or any combination thereof.

[1129] NOTE: In some embodiments, CO 2 (g) is a point source of CO 2 CO in or from the emission source 2 For example, CO 2 (g) Flue gas or dilute CO 2 , or high purity CO 2 or captured CO 2 may include.

[1130] NOTE: In some embodiments, CO 2 (g) CO in or derived from air 2 For example, CO 2 (g) At least a certain amount of CO is generated even at very low concentrations. 2 For example, calcium oxide can be used to create air that can contain very low or very dilute concentrations of CO, if desired. 2 For example, CO 2(g) may include carbonates such as sodium or potassium carbonate, which may include carbonates derived from the reaction of carbon dioxide in the air with sodium or potassium or other alkali salts, such as sodium or potassium hydroxide, to form alkali carbonates, and / or may include carbonates derived from the reaction of calcium oxide or hydroxide with alkali carbonates to regenerate or form alkali hydroxides or alkali oxides or other alkali salts that can be used to absorb carbon dioxide from the air to regenerate or reform the alkali carbonates.

[1131] NOTE: In some embodiments, CaCO 3 or MgCO 3 may constitute a valuable resource. In some embodiments, CaCO 3 or MgCO 3 may constitute a carbon sequestration medium.

[1132] Example 61: Process for the production of sodium hydroxide using sulfur dioxide, carbon dioxide, carboxylic acid and magnesium intermediate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3COOH(aq) → Ca(CH 3 COO) 2 (aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[1133] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[1134] Note: CO 2 (g) is the recovered CO 2 may be configured.

[1135] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[1136] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[1137] NOTE: In some embodiments, the acetic acid in step “(1)” can include aqueous acetic acid generated or regenerated in step “(4).”

[1138] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[1139] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[1140] (4)Na 2SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[1141] (5) MgCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Mg(HCO 3 ) 2 (aq)

[1142] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be greater than 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.

[1143] NOTE: In some embodiments, MgCO 3 (s) is MgO or Mg(OH) 2 and CO 2 MgCO from reaction with 3 It may include (s).

[1144] NOTE: In some embodiments, CO 2 (g or aq) is CO from step (1), or step (9), or any combination thereof. 2 For example, in some embodiments, MgO or Mg(OH) 2 and CO 2 The reaction with CO results from the calcination or decomposition of calcium carbonate. 2 and / or the calcium carbonate calciner may be capable of producing lean or flue gas carbon dioxide, since the carbon dioxide in the lean or flue gas carbon dioxide may be recovered by reaction with magnesium oxide and / or magnesium hydroxide.

[1145] (6)Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[1146] NOTE: In some embodiments, Na 2 SO 3 (s) is Mg(HCO 3 ) 2 It may be dissolved in water prior to mixing with the aqueous solution containing (aq) or may form an aqueous solution.

[1147] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[1148] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[1149] NOTE: In some embodiments, Na 2 SO 3 (s or aq) is Na from step (4) 2 SO 3 may include.

[1150] NOTE: In some embodiments, Mg(HCO 3 ) 2 (aq) is Mg(HCO) from step (5). 3 ) 2 It may contain (aq).

[1151] NOTE: In some embodiments, residual MgSO 3 In a solution containing sodium bicarbonate, for example, MgSO 3 (aq). In some embodiments, residual MgSO 3It may be desirable to separate at least a portion of the nitrile from at least a portion of the sodium bicarbonate. For example, in some embodiments, the separation may include, but is not limited to, one or more of electrodialysis, or selective electrodialysis, or monoselective electrodialysis (MSED), or diselective electrodialysis (DSED), or concentration, or cryoprecipitation, or reverse osmosis, or a membrane-based process, or nanofiltration, or any combination thereof, and the like.

[1152] (7) MgSO 3 (s) → MgO(s) + SO 2 (g)

[1153] NOTE: The thermal decomposition of magnesium sulfite can be carried out with less energy and / or at lower temperatures than the thermal decomposition of calcium sulfite.

[1154] NOTE: The sulfur dioxide formed can be used, for example, in the reaction of alkali acetates or alkali carboxylates with sulfur dioxide.

[1155] (8) Reaction of magnesium oxide or magnesium hydroxide with carbon dioxide to form magnesium carbonate. MgO(s)+CO 2 (g) → MgCO 3 (s) MgO(s)+H 2 O(l or g or s) → Mg(OH) 2 (s or aq) Mg(OH) 2 (s or aq)+CO 2 (g) → MgCO 3 (s)+H 2 O(l or g or s)

[1156] NOTE: In some embodiments, CO 2 (g) CO from the decomposition of calcium carbonate 2 (g) may be included.

[1157] NOTE: In some embodiments, CO 2 (g) CO from an emission source, point source, or air2 (g) may be included.

[1158] Note: MgCO 3 (s) is MgCO 3 (s)+CO 2 +H 2 During the reaction of O with MgCO 3 It may include (s).

[1159] (9)2NaHCO 3 (aq) → 2NaHCO 3 (s)+water

[1160] NOTE: In some embodiments, NaHCO 3 (s) may be formed by a process or cycle including concentration and cooling precipitation, or a precipitation or crystallization process, or any combination thereof.

[1161] NOTE: In some embodiments, NaHCO 3 may be sold as a product and / or used as a carbon sequestration medium.

[1162] NOTE: In some embodiments, 2NaHCO 3 (aq) is a compound that is dissolved in water and / or in a pressurized or pressurized environment. 2 CO 3 (aq) and CO 2 (g) and water, which results in NaHCO 3 The need to crystallize or precipitate (s) can be avoided or prevented.

[1163] NOTE: In some embodiments, residual dissolved MgSO 3 Or at least a portion of the magnesium sulfite (if present) may be separated and / or precipitated.

[1164] NOTE: Water can be separated from sodium bicarbonate or sodium carbonate using systems and methods for water separation, systems and methods for salt precipitation or crystallization, or any combination thereof.

[1165] (10)2NaHCO 3 (s) → Na 2 CO 3 (s)+CO 2 (g)+H 2 O(g or l)

[1166] Note: CO 2 (g) is the recovered CO 2 may be configured.

[1167] NOTE: In some embodiments, Na 2 CO 3 may be sold as a product and / or used as a carbon sequestration medium.

[1168] NOTE: In some embodiments, Na 2 CO 3 (s) may be dissolved in water or an aqueous solution and / or may be Ca(OH) 2 and Na 2 CO 3 Na in reaction with (s) 3 CO 2 (s) may be constituted.

[1169] (11) Calcination or decomposition of alkaline earth carbonates to form alkaline earth oxides and carbon dioxide. ·CaCO 3 (s) → CaO(s) + CO 2 (g) MgCO 3 (s) → MgO(s) + CO 2 (g)

[1170] NOTE: In some embodiments, it may be desirable to decompose the calcium or magnesium carbonate in a form in which the carbon dioxide is highly pure, or in which the carbon dioxide is recovered, or in which the carbon dioxide is diluted and then recovered, or any combination thereof.

[1171] NOTE: In some embodiments, carbon dioxide from the decomposition of calcium carbonate or magnesium carbonate may constitute the carbon dioxide in the reaction of magnesium oxide or magnesium hydroxide with carbon dioxide.

[1172] (12) Reaction of alkaline earth oxides or hydroxides with alkali carbonates to form alkaline earth carbonates and alkali hydroxides. CaO(s or aq) + Na 2 CO 3 (s or aq) + water → 2NaOH(aq) + CaCO 3 (s) MgO(s or aq) + Na 2 CO 3 (s or aq) + water → 2NaOH(aq) + MgCO 3 (s) Ca(OH) 2 (s or aq)+Na 2 CO 3 (s or aq) → 2NaOH(aq) + CaCO 3 (s) MgO(s or aq) + Na 2 CO 3 (s or aq) + water → 2NaOH(aq) + MgCO 3 (s)

[1173] Note: In some embodiments, CaO+Na 2 CO 3 (s or aq) + water or MgO + Na 2 CO 3 (s or aq) + water can be carried out in multiple steps. For example, in some embodiments, CaO or MgO is reacted with water to produce Ca(OH) 2 (s), 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 a solid-liquid suspension containing milk of lime or milk of magnesia, or calcium hydroxide or magnesium hydroxide. For example, in some embodiments, Na 2 CO3 may comprise an aqueous solution or may be dissolved in water to form an aqueous solution. For example, in some embodiments, Ca(OH) 2 (s or aq), or milk of lime, or Mg(OH) 2 or a solution or solid-liquid mixture or suspension containing milk of magnesia, 2 CO 3 (aq) to form a solution comprising aqueous sodium hydroxide and a solid comprising calcium or magnesium carbonate.

[1174] NOTE: In some embodiments, at least a portion of the calcium carbonate or magnesium carbonate can be separated from at least a portion of the sodium hydroxide using, for example, solid-liquid separation.

[1175] Example 62: Process for producing sodium bicarbonate or sodium carbonate and / or calcium oxide or calcium carbonate (1) Reaction of acetic acid with materials containing calcium, magnesium, or other alkaline earth weak acid anions ·CaCO 3 (s or aq) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+CO 2 (g)+H 2 O(aq or l) Calcium silicate(s) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq) + silicon dioxide (s) + H 2 O(aq or l) ·CaS(s)+2CH 3 COOH(aq) → Ca(CH 3 COO) 2 (aq)+H 2 S(g) Calcium (weak acid anion) + 2CH 3 COOH(aq) → Ca(CH 3 COO) 2(aq) + weak acid (s, or g, or l, or aq) + H 2 O(aq or l)

[1176] NOTE: Residual or undissolved solids, such as silicon dioxide or other undissolved solids, can be separated from the liquid solution using solid-liquid separation.

[1177] Note: CO 2 (g) is the recovered CO 2 may be configured.

[1178] NOTE: In some embodiments, CO 2 (g) may be used internally or in other processes.

[1179] NOTE: In some embodiments, CO 2 (g) may be utilized, or sequestered, or sold, or may constitute a product. For example, CO 2 (g) CO 2 Quarantine site or CO 2 It may be utilized for EOR or external uses, or sequestered, or sold.

[1180] NOTE: In some embodiments, some chemicals that contain calcium may contain an amount of magnesium. In some embodiments, for example, an input chemical or input material may contain a mixture of calcium and magnesium.

[1181] NOTE: In some embodiments, acetic acid vapor and / or water vapor are added to CO 2 (g) may be separated or recovered.

[1182] (2) Ca(CH 3 COO) 2 (aq)+Na 2 SO 4 (s or aq) → 2NaCH 3 COO(aq)+CaSO 4 (s)

[1183] NOTE: In some embodiments, Na 2 SO4 (s) is Ca(CH 3 COO) 2 It may be added directly to or dissolved in (aq).

[1184] NOTE: In some embodiments, Na 2 SO 4 (s) is Ca(CH 3 COO) 2 (aq) is dissolved in water or an aqueous solution before mixing with Na 2 SO 4 (aq) can be formed.

[1185] NOTE: In some embodiments, water can be added to the process to make up for water that may exit the process, for example, if NaOH(aq) is the output, or another aqueous solution is the output, or any combination thereof. 2 SO 4 Na in the form of (aq) 2 SO 4 Or it can be added to the process by an aqueous solution containing sodium sulfate, Na 2 SO 4 At least a portion of the water in (aq) may constitute water added to the process. In some embodiments, Na 2 SO 4 (aq) can be provided or supplied as an aqueous solution. For example, in some embodiments, Na 2 SO 4 (aq) is Na 2 SO 4 (aq) to the process. In some embodiments, Na 2 SO 4 (aq) is solid or Na 2 SO 4 (s) and then dissolved in water to form Na 2 SO 4 (aq) can be formed.

[1186] NOTE: In some embodiments, Ca(CH3 COO) 2 (aq) is Ca(CH) from step (1). 3 COO) 2 It may contain (aq).

[1187] (3) 2NaCH 3 COO(aq)+SO 2 (g or aq)+H 2 O(l or aq) → Na 2 SO 3 (aq)+2CH 3 COOH(aq)

[1188] NOTE: In some embodiments, SO 2 (g) is SO 2 (g) may contain other gases. In some embodiments, 2NaCH 3 COO(aq)+SO 2 The reaction of (g) may result in at least some acetic acid vapor in the residual gas during or after the reaction. In some embodiments, the NaCH 3 The COO(aq) may be pre-contacted with or absorb at least a portion of the acetic acid vapor from the residual gas. In some embodiments, the reactor or absorber may be a reactor or absorber that is capable of absorbing at least a portion of the acetic acid vapor from the residual gas. 3 COO(aq) to SO 2 (g) before or during the reaction with NaCH 3 The COO(aq) may be configured to absorb acetic acid vapor. In some embodiments, acetic acid vapor may be removed from the residual gas using, for example, but not limited to, alkaline earth carbonate, or alkaline earth-weak acid, or alkaline earth carbonate-water slurry, or alkaline earth oxide, or one or more of alkaline earth, or any combination thereof.

[1189] NOTE: In some embodiments, NaCH 3 COO(aq) is NaCH from step (2). 3 May contain COO(aq).

[1190] NOTE: In some embodiments, SO 2 is CaSO in step (7) 3 SO from the calcination or decomposition of (s) 2 (g) may be included.

[1191] (4)Na 2 SO 3 (aq)+2CH 3 COOH(aq) → 2CH 3 COOH(aq)+Na 2 SO 3 (s)

[1192] Note: CH 3 COOH is Na 2 SO 3 In some embodiments, Na 2 SO 3 may be separated or precipitated from the solution by, for example, but not limited to, evaporation, or distillation, or crystallization, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1193] NOTE: In some embodiments, the CH 3 The COOH and / or water can be removed by, for example, evaporation, or distillation, or crystallization, or any combination thereof, to give Na 2 SO 3 In some embodiments, CH 3 The COOH may be distilled off with the water vapor and / or condensed with the water vapor, resulting in CH 3 A distillate or condensate containing COOH(aq) can be obtained.

[1194] NOTE: In some embodiments, Na 2 SO 3 (aq)+2CH 3 Magnesium sulfite(aq) may be present in COOH(aq). In some embodiments, when present, magnesium sulfite is Na 2 SO 3Precipitation or crystallization may begin prior to (4). In some embodiments, magnesium sulfite solids may be separated during step "(4)". In some embodiments, the separated magnesium sulfite may be decomposed to magnesium oxide, or may be decomposed separately from calcium sulfite, or may be decomposed together with calcium sulfite, or any combination thereof.

[1195] Note: Na 2 SO 3 (s) is separated into CH by solid-liquid separation. 3 The COOH(aq) can be separated by solid-liquid separation, which can include, but is not limited to, a filter, or a centrifuge, or a decanter, or a separation system or method described herein, or a separation system or method described in the art, or any combination thereof.

[1196] (5) MgCO 3 (s)+CO 2 (g or aq)+H 2 O(aq) → Mg(HCO 3 ) 2 (aq)

[1197] NOTE: Pressurized CO 2 Under atmospheric conditions or concentrated carbon dioxide or CO 2 (aq). For example, CO 2 The partial pressure may for example be greater than 0.5 bar, or 1 bar, or 2 bar, or 3 bar, or 4 bar, or 5 bar, 6 bar, or 7 bar, or 8 bar, or 9 bar, or 10 bar, or any combination thereof.

[1198] NOTE: In some embodiments, MgCO 3 (s) is MgO or Mg(OH) 2 and CO 2 MgCO from reaction with 3 It may include (s).

[1199] NOTE: In some embodiments, CO 2(g or aq) is CO from step (1), or step (9), or any combination thereof. 2 For example, in some embodiments, MgO or Mg(OH) 2 and CO 2 The reaction with CO results from the calcination or decomposition of calcium carbonate. 2 and / or the calcium carbonate calciner may be capable of producing lean or flue gas carbon dioxide, since the carbon dioxide in the lean or flue gas carbon dioxide may be recovered by reaction with magnesium oxide and / or magnesium hydroxide.

[1200] (6)Na 2 SO 3 (s or aq)+Mg(HCO 3 ) 2 (aq) → 2NaHCO 3 (aq)+MgSO 3 (s)

[1201] NOTE: In some embodiments, Na 2 SO 3 (s) is Mg(HCO 3 ) 2 It may be dissolved in water prior to mixing with the aqueous solution containing (aq) or may form an aqueous solution.

[1202] Note: CaSO 3 (s) or MgSO 3 At least a portion of (s) can be separated by solid-liquid separation.

[1203] NOTE: In some embodiments, NaHCO 3 may be sold as a product or used as a carbon sequestration medium.

[1204] NOTE: In some embodiments, Na 2 SO 3 (s or aq) is Na from step (4) 2 SO 3 may include.

[1205] NOTE: In some embodiments, Mg(HCO 3 ) 2 (aq) is Mg(HCO) from step (5). 3 ) 2 It may contain (aq).

[1206] NOTE: In some embodiments, residual MgSO 3 In a solution containing sodium bicarbonate, for example, MgSO 3 (aq). In some embodiments, residual MgSO 3 It may be desirable to separate at least a portion of the nitrile from at least a portion of the sodium bicarbonate. For example, in some embodiments, the separation may include, but is not limited to, one or more of electrodialysis, or selective electrodialysis, or monoselective electrodialysis (MSED), or diselective electrodialysis (DSED), or concentration, or cryoprecipitation, or reverse osmosis, or a membrane-based process, or nanofiltration, or any combination thereof, and the like.

[1207] (7) MgSO 3 (s) → MgO(s) + SO 2 (g)

[1208] NOTE: The thermal decomposition of magnesium sulfite can be carried out with less energy and / or at lower temperatures than the thermal decomposition of calcium sulfite.

[1209] NOTE: The sulfur dioxide formed can be used, for example, in the reaction of alkali acetates or alkali carboxylates with sulfur dioxide.

[1210] (8) Reaction of magnesium oxide or magnesium hydroxide with carbon dioxide to form magnesium carbonate. MgO(s)+CO 2 (g) → MgCO 3 (s) MgO(s)+H 2 O(l or g or s) → Mg(OH) 2 (s or aq) Mg(OH) 2 (s or aq)+CO2 (g) → MgCO 3 (s)+H 2 O(l or g or s)

[1211] NOTE: In some embodiments, CO 2 (g) CO from the decomposition of calcium carbonate 2 (g) may be included.

[1212] NOTE: In some embodiments, CO 2 (g) CO from emission sources, or point sources, or the air, or any combination thereof 2 (g) may be included.

[1213] Note: MgCO 3 (s) is MgCO 3 (s)+CO 2 +H 2 During the reaction of O with MgCO 3 It may include (s).

[1214] NOTE: In some embodiments, carbon dioxide from the decomposition of calcium carbonate or magnesium carbonate may constitute the carbon dioxide in the reaction of magnesium oxide or magnesium hydroxide with carbon dioxide.

[1215] NOTE: In some embodiments, CaO(s) or MgO(s) reacts 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 containing calcium hydroxide and / or magnesium hydroxide. In some embodiments, Ca(OH) 2 or Mg(OH) 2 reacts with carbonates such as sodium carbonate or sodium bicarbonate to produce CaCO 3 or MgCO 3 or CO 2 Reacts with CaCO3 or MgCO 3 For example, the sodium carbonate or sodium bicarbonate may form CO 2 In the absorption solution or CO 2 The absorbent solution used may include sodium carbonate, or sodium bicarbonate, or potassium carbonate, or potassium bicarbonate, or an alkali carbonate, or an alkali bicarbonate, or any combination thereof.

[1216] NOTE: In some embodiments, CO 2 (g) is a point source of CO 2 CO in or from the emission source 2 For example, CO 2 (g) Flue gas or dilute CO 2 , or high purity CO 2 or captured CO 2 may include.

[1217] NOTE: In some embodiments, CO 2 (g) CO in or derived from air 2 For example, CO 2 (g) At least a certain amount of CO is generated even at very low concentrations. 2 For example, calcium oxide can be used to create air that can contain very low or very dilute concentrations of CO, if desired. 2 For example, CO 2 (g) may include carbonates such as sodium or potassium carbonate, which may include carbonates derived from the reaction of carbon dioxide in the air with sodium or potassium or other alkali salts, such as sodium or potassium hydroxide, to form alkali carbonates, and / or may include carbonates derived from the reaction of calcium oxide or hydroxide with alkali carbonates to regenerate or form alkali hydroxides or alkali oxides or other alkali salts that can be used to absorb carbon dioxide from the air to regenerate or reform the alkali carbonates.

[1218] NOTE: In some embodiments, CaCO3 or MgCO 3 may constitute a valuable resource. In some embodiments, CaCO 3 or MgCO 3 may constitute precipitated calcium carbonate. In some embodiments, CaCO 3 or MgCO 3 may constitute a carbon sequestration medium.

[1219] Exemplary Description: Alkaline Earth Oxide Generation System and Method explanation Some embodiments of the present invention may relate to systems and methods for producing alkaline earth oxides, or alkaline earth hydroxides, or cements, or clinkers. Some embodiments of the present invention may relate to the manufacture of alkaline earth oxides, or alkaline earth hydroxides, or cements, or clinkers, which may include calcium, magnesium, or other alkaline earth containing chemicals or materials.

[1220] Some embodiments may include using an input material that includes an alkaline earth weak acid material to produce an alkaline earth oxide, or an alkaline earth hydroxide, or a cement, or a clinker. For example, in some embodiments, the alkaline earth weak acid material may include a carbonate, which may include, but is not limited to, one or more of 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 include a silicate-based material, which may include, but is not limited to, one or more of calcium silicate, or magnesium silicate, or orthosilicate, or fluorosilicate, or metasilicate, or pyrosilicate, or aluminosilicate, or silicon oxide, or silicon-based material, or any combination thereof. In some embodiments, the alkaline earth weak acid material may include a sulfide-based material, which may include, but is not limited to, one or more of calcium sulfide, or magnesium sulfide, or any combination thereof. For example, in some embodiments, the alkaline earth weak acid material may include a metal oxide or metal oxide derivative anion material, which may include, but is not limited to, one or more of aluminates, or ferrates, or ferrites, or zincates, or mangana...

Claims

1. A material containing calcium carbonate is reacted with a solution containing aqueous carboxylic acid to form a gas containing carbon dioxide and a solution containing aqueous calcium carboxylic acid. The aforementioned solution containing aqueous calcium carboxylate is reacted with sodium sulfate to form a solution containing aqueous sodium carboxylate and a solid containing calcium sulfate. The solution containing aqueous sodium carboxylate is reacted with sulfur dioxide to form sodium sulfite and aqueous carboxylic acid, The separation of the sodium sulfite from the aqueous carboxylic acid, The process involves reacting sodium sulfite to form a solid containing calcium sulfite, The calcium sulfite is decomposed to form calcium oxide and sulfur dioxide. A method that includes this.

2. The method according to claim 1, wherein the reaction of sodium sulfite to form a solid containing calcium sulfite includes reacting the sodium sulfite with calcium hydroxide to form an aqueous solution containing sodium hydroxide and a solid containing calcium sulfite.

3. Reacting sodium sulfite to form a solid containing calcium sulfite is, First, calcium carbonate is reacted with carbon dioxide and water to form a solution containing aqueous calcium bicarbonate, and then, The aforementioned solution containing aqueous calcium bicarbonate is reacted with sodium sulfite to form a solution containing aqueous sodium bicarbonate and a solid containing calcium sulfite. The method according to claim 1, including the method described in claim 1.

4. The decomposition of the aforementioned sodium bicarbonate to form sodium carbonate and carbon dioxide, The calcium oxide is reacted with water to form calcium hydroxide, The sodium carbonate is reacted with the calcium hydroxide to form an aqueous solution containing sodium hydroxide and a solid containing calcium carbonate. The method according to claim 3, further comprising:

5. The method according to claim 3, further comprising decomposing the sodium bicarbonate to form sodium carbonate and carbon dioxide.

6. The method according to claim 5, further comprising reacting the sodium carbonate with calcium hydroxide to form an aqueous solution containing sodium hydroxide and a solid containing calcium carbonate.

7. The method according to any one of claims 1 to 3, further comprising reacting calcium oxide with water to form calcium hydroxide.

8. The method according to any one of claims 1 to 3, wherein the aqueous carboxylic acid is selected from formic acid, acetic acid, propanoic acid, or any mixture thereof.

9. The method according to any one of claims 1 to 3, wherein the reaction of the solution containing aqueous sodium carboxylate with sulfur dioxide is carried out in an absorption tower comprising a first step and a second step.

10. The method according to any one of claims 1 to 3, wherein at least a portion of the calcium oxide is reacted with carbon dioxide to form calcium carbonate.

11. A material containing calcium carbonate is reacted with a solution containing aqueous carboxylic acid to form a gas containing carbon dioxide and a solution containing aqueous calcium carboxylic acid. The aforementioned solution containing aqueous calcium carboxylate is reacted with sodium sulfite to form a solution containing aqueous sodium carboxylate and a solid containing calcium sulfite. Decomposing the aforementioned calcium sulfite to form calcium oxide and sulfur dioxide, The aforementioned solution containing aqueous sodium carboxylate is reacted with sulfur dioxide to form sodium sulfite and carboxylic acid. To separate at least a portion of the sodium sulfite from the aqueous carboxylic acid. A method that includes this.

12. The method according to claim 11, further comprising reacting calcium oxide with water to form calcium hydroxide.

13. The method according to claim 11 or 12, further comprising recovering at least a portion of the carbon dioxide.

14. The method according to claim 11 or 12, wherein the carboxylic acid is selected from formic acid, acetic acid, or propanoic acid, and the carboxylate salt is selected from formate, acetate, or propanoate.

15. The method according to claim 11 or 12, wherein the reaction of the solution containing aqueous sodium carboxylate with sulfur dioxide is carried out in an absorption tower comprising a first step and a second step.

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