Chemistry:Calcium sulfite
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| Names | |
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| IUPAC name
Calcium sulfite
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| Other names
Sulfurous acid, calcium salt (1:1)
E226 | |
| Identifiers | |
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3D model (JSmol)
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PubChem CID
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| Properties | |
| CaSO3 | |
| Molar mass | 120.17 g/mol |
| Appearance | White solid |
| Melting point | 600 °C (1,112 °F; 873 K) |
| 4.3 mg/100 mL (18 °C) | |
Solubility product (Ksp)
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3.1×10−7[1] |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Calcium sulfate |
Other cations
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Sodium sulfite |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Calcium sulfite, or calcium sulphite, is a chemical compound, the calcium salt of sulfite with the formula CaSO3·x(H2O). Two crystalline forms are known, the hemihydrate and the tetrahydrate, respectively CaSO3·½(H2O) and CaSO3·4(H2O).[2] All forms are white solids. It is most notable as the product of flue-gas desulfurization.
Production
It is produced on a large scale by flue gas desulfurization (FGD). When coal or other fossil fuel is burned, the byproduct is known as flue gas. Flue gas often contains SO2, whose emission is often regulated to prevent acid rain. Sulfur dioxide is scrubbed before the remaining gases are emitted through the chimney stack. An economical way of scrubbing SO2 from flue gases is by treating the effluent with Ca(OH)2 hydrated lime or CaCO3 limestone.[3]
Scrubbing with limestone follows the following idealized reaction:
- SO
2 + CaCO
3 → CaSO
3 + CO
2
Scrubbing with hydrated lime follows the following idealized reaction:[4][5]
- SO
2 + Ca(OH)
2 → CaSO
3 + H
2O
The resulting calcium sulfite oxidizes in air to give gypsum:
- CaSO
3 + 1⁄2 O
2 → CaSO
4
The gypsum, if sufficiently pure, is marketable as a building material.
Uses
Drywall
Calcium sulfite is generated as the intermediate in the production of gypsum, which is the main component of drywall. A typical US home contains 7 metric tons of such drywall gypsum board.[6]
Food additive
As a food additive it is used as a preservative under the E number E226. Along with other antioxidant sulfites, it is commonly used in preserving wine, cider, fruit juice, canned fruit and vegetables. Sulfites are strong reducers in solution, they act as oxygen scavenger antioxidants to preserve food, but labeling is required as some individuals might be hypersensitive.
Wood pulp production
Chemical wood pulping is the removal of cellulose from wood by dissolving the lignin that binds the cellulose together. Calcium sulfite can be used in the production of wood pulp through the sulfite process, as an alternative to the Kraft process that uses hydroxides and sulfides instead of sulfites. Calcium sulfite was used, but has been largely replaced by magnesium and sodium sulfites and bisulfites to attack the lignin.[citation needed]
Gypsum
There is a possibility to use calcium sulfite to produce gypsum by oxidizing (adding O2) it in water mixture with the manganese (Mn2+) cation or sulfuric acid catalyzers.[7][8]
Structure
Structure of the [Ca3(SO3)2(H2O)12]2+ cage in calcium sulfite tetrahydrate.
Structure of anhydrous CaSO3.
2aq12.png)
X-ray crystallography shows that anhydrous calcium sulfite has a complicated polymeric structure.[9] The tetrahydrate crystallizes as a solid solution of Ca3(SO3)2(SO4).12H2O and Ca3(SO3)2(SO3).12H2O. The mixed sulfite-sulfate represents an intermediate in the oxidation of the sulfite to the sulfate, as is practiced in the production of gypsum. This solid solution consists of [Ca3(SO3)2(H2O)12]2+ cations and either sulfite or sulfate as the anion.[2][10] These crystallographic studies confirm that sulfite anion adopts a pyramidal geometry.
Natural occurrence
Calcium sulfite(III) hemihydrate occurs in the nature as the rare mineral hannebachite.[11][12]
See also
References
- ↑ John Rumble (June 18, 2018) (in English). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
- ↑ 2.0 2.1 Abraham Cohen; Mendel Zangen (1984). "Studies On Alkaline Earth Sulfites. Structure and Stability of the New Compound Ca3(SO3)2SO4.12H2O and Its Solid Solution In Calcium Sulfite Tetrahydrate". Chemistry Letters 13 (7): 1051–1054. doi:10.1246/cl.1984.1051.
- ↑ Wirsching, Franz (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a04_555.
- ↑ Hudson, JL (1980). Sulfur Oxidation in Scrubber Systems. University of Virginia.
- ↑ Miller, Bruce (2004). Coal Energy Systems. Elsevier Science Technology. pp. 294–299.
- ↑ "USGS Gypsum Statistics and Information". http://minerals.usgs.gov/minerals/pubs/commodity/gypsum/.
- ↑ Li, Yuran; Zhou, Jinting; Zhu, Tingyu; Jing, Pengfei (2014-02-01). "Calcium Sulfite Oxidation and Crystal Growth in the Process of Calcium Carbide Residue to Produce Gypsum" (in en). Waste and Biomass Valorization 5 (1): 125–131. doi:10.1007/s12649-013-9206-2. ISSN 1877-2641.
- ↑ "How can we convert calcium sulfite into calcium sulfate after..." (in en). https://www.researchgate.net/post/How_can_we_convert_calcium_sulfite_into_calcium_sulfate_after_a_flue_gas_desulfurization_scrubber.
- ↑ Yasue, Tamotsu; Arai, Yasuo (1986). "Crystal Structure of Calcium Sulfite". Gypsum & Lime (Jap. Language) 203: 235–44.
- ↑ Matsuno, Takashi; Takayanagi, Hiroaki; Furuhata, Kimio; Koishi, Masumi; Ogura, Haruo (1984). "The Crystal Structure of Calcium Sulfite Hemihydrate". Bulletin of the Chemical Society of Japan 57 (4): 1155–6. doi:10.1246/bcsj.57.1155.
- ↑ "Hannebachite". https://www.mindat.org/min-1997.html.
- ↑ "List of Minerals". 21 March 2011. https://www.ima-mineralogy.org/Minlist.htm.
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