Process for carbon dioxide fixation and regeneration

Abstract

A process is provided for capturing and transporting carbon dioxide in a solid or liquid mixture. In this process, a liquid base is added to carbon dioxide to produce a carbonate, the carbonate is then stored or transported to a second facility where an acid is added to the carbonate to release carbon dioxide. The carbon dioxide can then be used as needed. The liquid base or the acid may be mined, collected from an industrial waste stream (fly ash), or produced by a chemical or electrochemical process including electrolysis, electrodialysis, or salt splitting.

Description

PROCESS FOR CARBON DIOXIDE FIXATION AND REGENERATION

[0001] This application claims priority to US provisional application 63 / 669,110 filed July 9, 2024. FIELD

[0002] The field relates to the capture of carbon dioxide. The field also relates to the capture and transport of carbon dioxide. BACKGROUND

[0003] Carbon dioxide is a trace gas in the Earth’s atmosphere at current levels of about 420 parts per million or 0.04% as of 2022. Carbon dioxide (CO2) is a primary source of carbon for life on Earth through photosynthesis and is also an important heat-trapping gas, also known as a greenhouse gas. The amount of carbon dioxide in the air has increased from the extraction and burning of fossil fuels (such as coal, oil, and natural gas), from wildfires, and natural processes like volcanic eruptions. Since the onset of industrial times in the 18th century, some estimates are that human activities have raised atmospheric CO2 by 50% – meaning the amount of CO2 is now 150% of its value in 1750.

[0004] Carbon capture, utilization, and storage (CCUS) comprise of a group of technologies and processes designed to capture carbon dioxide (CO2) emissions from power plants, industrial facilities, or directly from the atmosphere, store it in long-term reservoirs or in stable solid or aqueous carbonates, or utilize the captured CO2in various applications to prevent it from entering the atmosphere and contributing to climate change. Carbon storage and carbon utilization are currently two distinct destinations for captured carbon.

[0005] Once the carbon dioxide is captured, it can be transported to storage sites or utilization facilities as a gas through pipelines or by tank trucks, ships or trains. These carbon dioxide transportation methods require extra capital expenditures (especially pipelines) and could generate extra carbon emissions. In addition, the storage of gaseous carbon dioxide requires gas tight storage systems to prevent subsequent carbon dioxide emissions.

[0006] Carbon sequestration or carbonation is one of the natural or engineered carbon storage mechanisms, in which CO2 is converted into stable carbonates, such as aqueous bicarbonate, solid calcium carbonate (CaCO3), magnesium carbonate (MgCO3), or iron carbonate (FeCO3). This can occur naturally in certain geological formations or can be induced through various methods such as mineral carbonation or biological processes. However, the generated carbonates, especially the aqueous bicarbonate, are often of little value without further process steps, and the stored carbon cannot be utilized by carbon utilization industry for valuable chemical production.

[0007] On the other hand, CO2is a versatile industrial feedstock, used, for example, as an inert gas in welding and fire extinguishers, as a pressurizing gas in air guns and oil recovery, and as a supercritical fluid solvent in decaffeination and supercritical drying. It is a byproduct of fermentation of sugars in bread, beer and wine making, and is added to carbonated beverages for effervescence. With the development of new carbon utilization technologies, such as electrochemical synthesis and synthetic biology, the value of CO2 as a chemical and biological feedstock is increasing because of the various products that can be produced by sustainable synthesis methods. The development of those technologies requires stable and easy-access CO2of high purity and affordable cost.

[0008] This disclosure describes economic and energy efficient processes as an alternative method for carbon dioxide storage and transportation, in which carbon dioxide would be storing and transporting in a solid or liquid form at ambient pressure and temperature, and then releasing the carbon dioxide when and if it is needed. The processes described in this disclosure improves the overall efficiency of CCUS ecosystem by connecting carbon storage with carbon utilization, enabling the utilization of low value carbon storage waste, and providing carbon utilization technologies with economic and easy-access carbon sources. SUMMARY

[0009] A process for transporting carbon dioxide is provided involving the addition of a liquid base to carbon dioxide to produce a carbonate or a bicarbonate at a first facility, transportation of the carbonate or bicarbonate at least 100 meters to a second facility and then adding an acid to the carbonate to release carbon dioxide at the second facility. The liquid base may have a concentration from about 0.04% to 100%. The stored carbonate or bicarbonate is maintained inthe carbonate or bicarbonate form and then carbon dioxide is released to be used in an industrial process at the same location or a different location. The liquid base generally has a pH between 8 and 14 and preferably the liquid base has a pH between 12 and 14 or higher. The acid may have a pH between 1 and 4 and in some cases under 1. The liquid base may be added to carbon dioxide at an ambient temperature and an ambient pressure but in some cases, it is desirable to do so at decreased or elevated pressures or temperatures. The liquid base may be selected from the group consisting of sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide, lithium hydroxide, aluminum hydroxide, beryllium hydroxide, strontium hydroxide, barium hydroxide, titanium hydroxide, manganese hydroxide, nickel hydroxide, zinc hydroxide, ruthenium hydroxide and other noble and non-noble metal hydroxides. In addition to pure base streams, industrial waste streams can be used as a source of alkalinity such as fly ash, or mined brucite. The acid may be selected from the group consisting of sulfuric acid, sulfurous acid, hyposulfurous acid, hydrosulfuric acid, chloric acid, hydrochloric acid, perchloric acid, nitric acid, acetic acid, oxalic acid, phosphoric acid, hydrobromic acid, hydrofluoric acid, chromic acid, boric acid, citric acid, formic acid, permanganic acid and silicic acid. The carbonate or bicarbonate may include calcium carbonate, calcium bicarbonate, magnesium carbonate, magnesium bicarbonate, zinc carbonate, zinc bicarbonate, lithium carbonate, lithium bicarbonate, aluminum carbonate, aluminum bicarbonate, beryllium carbonate, beryllium bicarbonate, strontium carbonate, strontium bicarbonate, barium carbonate, barium bicarbonate, titanium carbonate, titanium bicarbonate, manganese carbonate, manganese bicarbonate, nickel carbonate, nickel bicarbonate, sodium carbonate, sodium bicarbonate, potassium carbonate, and potassium bicarbonate. The process may further include collecting the carbon dioxide from air, industrial processes, or as a product of a carbon capture process. The released carbon dioxide is about 99.9% pure carbon dioxide. The released carbon dioxide is greater than 90 wt% of the carbon dioxide to which the liquid base was added. The carbonate or bicarbonate may be transported to a new location and / or stored for a desired period of time prior to the addition of acid to produce usable carbon dioxide. The liquid base or acid or both may be produced by a chemical or electrochemical process such as electrolysis, electrodialysis, or salt splitting. BRIEF DESCRIPTION OF THE DRAWINGS

[0010] FIG.1 is a schematic drawing that shows the three steps of carbon dioxide conversion, carbon dioxide storage or transportation and carbon dioxide regeneration.

[0011] FIG.2 is a schematic drawing that adds an electrolyzer or salt splitting unit to provide the base and acid to the process of converting carbon dioxide to be stored or transported and then regenerated.

[0012] FIG.3 is a schematic drawing that shows the conversion of carbon dioxide, transportation and on-site regeneration with two electrolyzers or two salt splitting units or one electrolyzer and one salt splitting unit. DETAILED DESCRIPTION

[0013] This disclosure describes a process in which CO2is separated from CO2-containing sources, including air, industrial processes, or as a product of carbon capture processes; converted into a stable carbonate for storage and transportation, and converted back to pure CO2 at a CO2 utilization site when needed. The processes described in this disclosure improve the overall efficiency of CCUS ecosystem by connecting carbon storage with carbon utilization, enabling the utilization of low value carbon storage waste, and providing carbon utilization technologies with economic and easy-access carbon sources.

[0014] Moreover, the processes described in this disclosure decouple carbon capture sites from access to pipeline, allowing access to more sites with advantageous power economies. CCUS will require the use of power assets that do not compete with current grid improvements. Adding access to green power, the ideal sites have curtailed power-availability with depreciated assets. Building pipelines to these sites is prohibitively expensive because of the difficulty in obtaining rights of way, and the multiple government permitting agencies that are required for approval.

[0015] One design of this process is shown in FIG.1. The three parts of the process are shown in FIG.1. In a system 20 for processing carbon dioxide, a supply of carbon dioxide 24 is added to the carbon dioxide converter 26. A liquid base 22 is added to the carbon dioxide and reacts with the liquid base to produce carbonate or bicarbonate. A base (AOH) is used to convert CO2 gas and fix the carbon dioxide in the form of a stable carbonate (A2CO3) or bicarbonate (AHCO3) form (CO2conversion step). The base may be selected from sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide, lithium hydroxide, aluminum hydroxide, beryllium hydroxide, strontium hydroxide, barium hydroxide, titanium hydroxide, manganesehydroxide, nickel hydroxide, zinc hydroxide, ruthenium hydroxide and other noble or non-noble metal hydroxides. The formation of the carbonate by addition of CO2 to the base can be achieved at about 0 to about 200ºC and atmospheric pressure to about 34474 kPa. The base is only required to be above 7, but a higher pH will decrease the reaction time. The carbonate or bicarbonate can be stored at a desired location for a desired length of time, and then transported by means of vehicle, ship, train or any economical methods (CO2storage or transportation step). The carbonate or bicarbonate may be selected from sodium carbonate, sodium bicarbonate, potassium carbonate, potassium bicarbonate, calcium carbonate, calcium bicarbonate, magnesium carbonate, magnesium bicarbonate, zinc carbonate, zinc bicarbonate, lithium carbonate, lithium bicarbonate, aluminum carbonate, aluminum bicarbonate, beryllium carbonate, beryllium bicarbonate, strontium carbonate, strontium bicarbonate, barium carbonate, barium bicarbonate, titanium carbonate, titanium bicarbonate, manganese carbonate, manganese bicarbonate, nickel carbonate, and nickel bicarbonate.

[0016] After the carbon dioxide has reacted with the liquid base to produce carbonate or bicarbonate it is discharged from the carbon dioxide converter 26 in line 32. The carbonate or bicarbonate in line 32 is transported or stored. In an embodiment, the carbonate or bicarbonate is stored in a storage facility 34. The carbonate or bicarbonate may be stored in a solid form or in an aqueous solution form almost indefinitely.

[0017] Eventually carbonate or bicarbonate is sent in line 35 to carbon dioxide regeneration reactor 60. An acid 50 is added to carbonate or bicarbonate from storage facility 34 that is sent to the regeneration reactor 60 to produce carbon dioxide which is removed in line 38 perhaps for an industrial use. A salt 45 is shown being removed.

[0018] When needed, pure CO2can be released by dissolving A2CO3or AHCO3with an acid (HX) (the CO2 regeneration step). The acid may be selected from sulfuric acid, sulfurous acid, hyposulfurous acid, hydrosulfuric acid, chloric acid, hydrochloric acid, perchloric acid, nitric acid, formic acid, acetic acid, oxalic acid, phosphoric acid, hydrobromic acid, hydrofluoric acid, chromic acid, boric acid, citric acid, permanganic acid and silicic acid. To disengage CO2 from the carbonate, the acid must be below pH= about 7. A lower concentration acid will require greater volume.

[0019] The CO2 regeneration step can be done at a range of conditions to facilitate integration into carbon utilization technologies. For example, water gas shift reactions occur from 1000- 6000 kPa, and temperatures are 200-480˚C. In this case, it would be advantageous to allow the autogenous pressure of the disengagement to reach the process pressure. This could be done in batch or continuous modes. This process can also be applied to lower pressure cases, near or sub atmospheric pressures.

[0020] FIG.2 shows a system 100 that uses an electrolyzer or salt splitting unit 125 to produce hydrogen 137, oxygen 139 and a base 140 to be sent to react with carbon dioxide gas 102 at pressures ranging from about 0 to about 8963 kPa and temperatures from ambient to 250ºC. The electrolyzer or salt splitting unit 125 is used to split a neutral salt solution (AX) with a concentration between about 0.01 to about 10 M, generating a base effluent stream (AOH) with a concentration between about 0.01 to 10 M, an acid effluent stream (HX) with a concentration between about 0.01 to 10 M, and green hydrogen at a pressure between about 34.47 and about 8963 kPa as a valuable co-product. The generated base (AOH) is used to adsorb CO2gas at pressures ranging from about 0 to about 9000 kPa, and temperatures from ambient to about 250ºC and convert it into a stable form of solid or liquid carbonate (A2CO3) or bicarbonate (AHCO3) in a CO2conversion step. The electrolyzer or salt splitting unit 125 may be operated between about 0 and about 120˚C and between about 0 and about 9000 kPa differential pressure. The base is shown in reactor 106 supplied by line 140. The base and carbon dioxide react to produce a carbonate or bicarbonate at about ambient temperature and about 21 kPa. The carbonate or bicarbonate is then transported to vessel 110 in line 109 to be stored or transported to carbon dioxide regeneration section 150 in line 112 at ambient conditions. The solid or liquid carbonate or bicarbonate can be stored temporarily or transported to another desired location for storage or use by means of vehicles, ships, low pressure pipeline, or any economical methods (CO2 storage or transportation step). For example, the solid carbonate or liquid bicarbonate may be transported in line 112 to the regeneration section 150. The regeneration section 150 may be at least 100 m, 10 km or 100 km or 1000 km away from the system 100 in which the carbon dioxide reacts with the base.

[0021] In this embodiment, when needed, pure carbon dioxide can be released by dissolving the carbonate or bicarbonate with the acid (HX) in line 135 generated by the electrolyzer or saltsplitting unit (carbon dioxide regeneration step). The electrolyzer 125 produces the acid stream in line 135 that is sent to the carbon dioxide regeneration section 150. In a reactor 130 in the regeneration section 150, a carbonate or bicarbonate 130 is reacted with the acid stream 135 to produce carbon dioxide which is shown exiting in line 140 at pressures ranging from about 0 to about 8963 kPa and temperatures from about ambient temperature to about 250ºC.

[0022] The carbon dioxide regeneration step can be done at a range of conditions, e.g. at a temperature between about 0 and about 100˚C and a pressure between about a vacuum and about 15200 kPa to facilitate integration into carbon utilization technologies. Also, in reactor 130 in the regeneration section 150, a near neutral salt is also generated after the carbonate or bicarbonate reacted with the acid 135. Line 134 transports the spent salt solution and water for filtration and conditioning in 120 before reuse. This salt product can then be sent back to the CO2 conversion section 100 and fed into the electrolyzer or salt splitting unit 125 to produce more hydrogen 137, oxygen 139, base stream 140, and acid stream 135 to continue the process.

[0023] Yet another design of this process is shown in Figure 3. FIG.3 shows a system with two electrolyzers or salt splitting units 220 and 236. An electrolyzer or salt splitting unit 220 is used to split a neutral salt solution (AX), generating a base effluent stream (AOH), an acid effluent stream (HX) as a valuable co-product, and green hydrogen as a second valuable co-product. A salt solution in line 218 is sent to electrolyzer or salt splitting unit 220 which produces a hydrogen stream 222, an oxygen stream 224 and an acid stream 226. A stream of base 228 is produced and shown entering reactor 214 to react with the carbon dioxide from line 210 in reactor 214 to produce a carbonate or bicarbonate at pressures ranging from about 0 to about 9000 kPa and temperatures from ambient to about 250ºC. The generated base (AOH) is used to adsorb CO2 gas with a concentration between about 0.04% to about 100% at pressures ranging from about 0 to about 9000 kPa, and temperatures from about ambient to about 250ºC and convert it into the stable form of carbonate (A2CO3) or bicarbonate (AHCO3) of a concentration between about 0.01 and about 10 M (CO2 conversion step). The carbonate or bicarbonate is transported to a vessel 230 in line 232 where it may remain, be stored or be transported. A2CO3or AHCO3can be transported in or from the vessel 230 to another desired location by means of vehicles, ships, low pressure pipeline, or any economical methods (CO2 storage or transportation step) in line 234 and / or to a reactor 246 in a carbon dioxide regeneration section 250 to bereacted with an acid provided in line 242 to produce carbon dioxide which is then sent in stream 248 to be used in an industrial facility. On the CO2 utilization site, another electrolyzer or salt splitting unit 236 is used to split a neutral salt solution (BY), generating an acid effluent stream (HY), a base effluent stream (BOH) as a valuable co-product, and green hydrogen as a second valuable co-product. Also shown is neutral salt solution 234 which is sent to the electrolyzer 236 to produce a hydrogen stream 238 and an oxygen stream 240 at pressures ranging from about 0 to about 9000 kPa, and temperatures from ambient to about 250˚C. An amount of base 252 is also produced which may be used elsewhere in the facility. When needed, pure CO2 can be released by dissolving ACO3or AHCO3with the acid (HY) (CO2regeneration step). The CO2regeneration step can be done at a range of conditions to facilitate integration into carbon utilization technologies. Example 1

[0024] One example of this process is exemplified in Example 1. At the carbon capture site, the electrolyzer used in this process employs a feed solution containing 0.3 Molar sodium sulfate. Under operational conditions, the electrolyzer is configured to produce multiple key outputs: hydrogen, oxygen, sodium hydroxide, and sulfuric acid. Specifically, the system is designed such that 1.5 tonnes of sodium sulfate feed results in the production of 20 kilograms of hydrogen, 163 kilograms of oxygen, and one tonne of sulfuric acid. Concurrently, the system generates 0.8 tonnes of sodium hydroxide.

[0025] The sodium hydroxide produced is subsequently reacted with 0.9 tonnes of carbon dioxide at a starting concentration of 85 %, leading to the formation of approximately 22 tonnes of 1 M sodium bicarbonate per day. The bicarbonate products are then ready for transportation to a utilization site via truck, train, rail, or via a conventional carbon dioxide pipeline but without compression, as preferred. This transportation flexibility is crucial for adapting to various geographic and economic contexts.

[0026] At the utilization site, the electrolyzer used in this process is engineered to produce a pure base stream for commercial sale. The acidic stream, a byproduct of the electrolysis reaction, is further utilized by mixing it with sodium (or calcium) bicarbonate solutions to regenerate a pure carbon dioxide stream. This approach ensures the full utilization of all byproducts, therebyenhancing the sustainability and efficiency of the system. Each electrolyzer within the system operates at a scale facilitated by a 68-kilowatt power input. Example 2

[0027] Another example of this process is described in Example 2. At the carbon capture site, a salt splitting unit used in this process employs a feed solution containing 0.6 Molar lithium sulfate. Under operational conditions, the salt splitting unit is configured to produce multiple key outputs: hydrogen, oxygen, sulfuric acid, and lithium hydroxide. Specifically, the system is designed such that 1.1 tonnes of lithium sulfate feed results in the production of 20 kilograms of hydrogen, 163 kilograms of oxygen, 6 tonnes of 2 Molar sulfuric acid solution, and 0.5 ton of lithium hydroxide in a 2 Molar solution. The salt splitting unit within the system operates at a scale facilitated by a 68-kilowatt power input.

[0028] The lithium hydroxide produced is subsequently reacted with 0.45 tonnes of carbon dioxide at a starting concentration of 5%, leading to the formation of approximately 0.8 tonnes of lithium carbonate solids per day. The carbonate and sulfuric acid products are then ready for storage or transportation to a utilization site via truck, train, or rail, as preferred. This transportation flexibility is crucial for adapting to various geographic and economic contexts.

[0029] At the utilization site, the sulfuric acid solution is utilized by mixing it with the carbonate solid to regenerate a pure carbon dioxide stream. Concurrently, 6.4 tonnes of 1.9 molar lithium sulfate solution is produced and can be transported back to the carbon capture site and fed into the salt splitting unit or sale as concentrated lithium solution as preferred. This approach ensures the full utilization of all byproducts, thereby enhancing the sustainability and efficiency of the system. Example 3

[0030] Another example of this process is described in Example 3. At the carbon capture site, 7 kilograms of calcium hydroxide and 55 tonnes of calcium chloride are added into 100 tonnes of seawater to make a solution of around pH 11. Twenty-two tonnes of carbon dioxide at a starting concentration of 12% is reacted with the alkalic water, leading to the formation of approximately 51 tonnes of calcium carbonate and magnesium carbonate solid per day. Concurrently, theprocess softens and regenerates seawater. The carbonates are then ready for transportation to a utilization site via truck, train, or rail, as preferred. This transport flexibility is crucial for adapting to various geographic and economic contexts. At the utilization site, the carbonate solids are mixed with 37 tonnes of chloric acid to regenerate a pure carbon dioxide stream. Concurrently, 165 tonnes of solutions containing 56 tonnes of calcium chloride (5 M) are produced and can be used at the carbon capture site to convert more carbon dioxide. This approach ensures the full utilization of all byproducts, thereby enhancing the sustainability and efficiency of the system. Example 4

[0031] Another example of this process is described in Example 4. At the carbon capture site, a salt splitting unit used in this process is fed with 1,800 Liters per day of processed mining waste containing 1 Molar sodium sulfate to the anode chambers and 9,000 Liters per day of another processed mining waste containing 0.5 Molar of sodium sulfate to the cathode chambers. Under operational conditions, the salt splitting unit is configured to produce multiple key outputs: oxygen and sulfuric acid of pH 1.4 from the anode chamber, and hydrogen and sodium hydroxide of pH 12.5 from the cathode chamber. Specifically, the system is designed such that in the anode chambers 1,800 Liters per day of processed mining waste containing 1 Molar sodium sulfate results in the production of 400 Liters per day of oxygen and 1,800 Liters of sulfuric acid of pH 1.4. In the cathode chambers, 9,000 Liters per day of processed mining waste containing 0.5 Molar of sodium sulfate results in the production of 3,190 Liters per day of hydrogen and 9,000 Liters per day of sodium hydroxide of pH 12.5. The salt splitting unit within the system operates at a scale facilitated by a 1-megawatt power input.

[0032] The sodium hydroxide that is produced is subsequently reacted with 12 tonnes per day of carbon dioxide at a starting concentration of 15%, leading to the formation of approximately 13.9 tonnes of sodium bicarbonate solids per day. The bicarbonate and sulfuric acid products are then ready for storage or transportation to a utilization site via truck, train, or rail, as preferred. This transportation flexibility is crucial for adapting to various geographic and economic contexts.

[0033] At the utilization site, the sulfuric acid solution is utilized by mixing it with the carbonate solid to regenerate a pure carbon dioxide stream. Concurrently, 20.2 tonnes sodium sulfate in solution is produced and can be transported back to the carbon capture site and fed into the saltsplitting unit or sale as pure sodium sulfate solution as preferred. This approach ensures the full utilization of all byproducts, thereby enhancing the sustainability and efficiency of the system.

Claims

Claims 1. A process for transporting carbon dioxide comprising adding a liquid base to carbon dioxide to produce a carbonate at a first facility, transporting said carbonate at least one mile to a second facility and then adding an acid to the carbonate to release carbon dioxide at the second facility.

2. The process of claim 1 wherein said liquid base is produced from an aqueous neutral salt solution by a chemical or electrochemical process including by an electrolyzer, a salt splitting unit, or an electrodialysis unit.

3. The process of claim 1 wherein said acid is produced from an aqueous neutral salt solution by a chemical or electrochemical process including electrolyzer, salt splitting unit, or electrodialysis.

4. The process of claim 1 wherein said liquid base has a concentration from about 0.04% to 100%.

5. The process of claim 1 wherein said carbonate is stored and then said carbon dioxide is released to be used in an industrial process at a same location as a facility where said liquid base is added to said carbon dioxide.

6. The process of claim 1 wherein said liquid base has a pH between about 8 and 14.

7. The process of claim 1 wherein said liquid base has a pH between about 12 and 14 or higher.

8. The process of claim 1 wherein said acid has a pH between about 1 and 4.

9. The process of claim 1 wherein said acid has a pH under 1.

10. The process of claim 1 wherein said liquid base is added to carbon dioxide at a temperature between about 0 and 100˚C and a pressure between about a vacuum and 15200 kPa.

11. The process of claim 1 wherein said acid is added to said carbonate at a temperature between about 0 and 100˚C and a pressure between vacuum and 15200 kPa.

12. The process of claim 1 wherein said liquid base is selected from the group consisting of sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide, lithium hydroxide, aluminum hydroxide, beryllium hydroxide, strontium hydroxide, barium hydroxide, titanium hydroxide, manganese hydroxide, nickel hydroxide, zinchydroxide, ruthenium hydroxide and other noble or non-noble metal hydroxides, or a mixture of hydroxides resulting from an industrial process.

13. The process of claim 1 wherein said acid is selected from the group consisting of sulfuric acid, sulfurous acid, hyposulfurous acid, hydro sulfuric acid, chloric acid, hydrochloric acid, perchloric acid, nitric acid, acetic acid, oxalic acid, phosphoric acid, hydrobromic acid, hydrofluoric acid, chromic acid, boric acid, citric acid, formic acid, permanganic acid and silicic acid.

14. The process of claim 1 wherein said carbonate and said bicarbonate is selected from the group consisting of calcium carbonate, calcium bicarbonate, magnesium carbonate, magnesium bicarbonate, zinc carbonate, zinc bicarbonate, lithium carbonate, lithium bicarbonate, aluminum carbonate, aluminum bicarbonate, beryllium carbonate, beryllium bicarbonate, strontium carbonate, strontium bicarbonate, barium carbonate, barium bicarbonate, titanium carbonate, titanium bicarbonate, manganese carbonate, manganese bicarbonate, nickel carbonate, nickel bicarbonate, sodium carbonate, sodium bicarbonate, potassium carbonate, and potassium bicarbonate.

15. The process of claim 1 further comprising collecting said carbon dioxide from air, industrial processes, or as a product of a carbon capture process.

16. The process of claim 1 wherein said released carbon dioxide is about 99.9% pure carbon dioxide.

17. The process of claim 1 wherein said released carbon dioxide is greater than 90 wt% of said carbon dioxide to which a liquid base was added.

18. The process of claim 1 wherein a salt is produced when said acid is added to said carbonate.

19. A process for storing carbon dioxide comprising adding a liquid base to carbon dioxide to produce a carbonate or a bicarbonate, then storing said carbonate or bicarbonate and then adding an acid to the carbonate or bicarbonate to release carbon dioxide.

20. The process of claim 1 wherein said carbonate is transported before said addition of said acid.

21. A process for fixation and release of carbon dioxide comprising adding a liquid base to carbon dioxide to produce a carbonate and then adding an acid to the carbonate to release carbon dioxide.

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