Calcium sulfite
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| Names | |
|---|---|
| IUPAC name
Calcium sulfite | |
| Other names
Sulfurous acid, calcium salt (1:1) E226 | |
| Identifiers | |
| 3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.030.529 |
| E number | E226 (preservatives) |
| PubChem CID |
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| UNII | |
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| Properties | |
| CaSO3 | |
| Molar mass | 120.17 g/mol |
| Appearance | white solid |
| Melting point | 600 °C (1,112 °F; 873 K) |
| 0.0043 g/100 mL, 18C | |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions |
Calcium sulfate |
| Other cations |
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 and .[1] All forms are white solids. It is most notable as the product of flue-gas desulfurization.
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.[2]
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.[3]
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.
Scrubbing with limestone follows the following idealized reaction:
- SO2 + CaCO3 → CaSO3 + CO2
Scrubbing with hydrated lime follows the following idealized reaction:[4][5]
- SO2 + Ca(OH)2 → CaSO3 + H2O
In the laboratory calcium sulfite can be produced by reaction of aqueous solutions of calcium chloride and sodium sulfite.
- CaCl2 + Na2SO3 → CaSO3 + 2 NaCl
Structure
The structure of calcium sulfite has been examined by X-ray crystallography.[6] These studies show that sulfite anion adopts its characteristic pyramidal geometry. The Ca2+ centers have high coordination numbers, being bonded to the sulfite oxygen atoms and the water, giving calcium a coordination number of eight. 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 [[Ca<sub>3</sub>(SO<sub>3</sub>)212H<sub>2</sub>O]]2+ cations and either sulfite or sulfate as the anion.[1][7]
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See also
References
- 1 2 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: 1051–1054. doi:10.1246/cl.1984.1051.
- ↑ "USGS Gypsum Statistics and Information". USGS. Retrieved June 26, 2016.
- ↑ Ropp, Richard (2013). Encyclopedia of the Alkaline Earth Compounds. Elsevier Science Technology. pp. 145–148.
- ↑ Hudson, JL (1980). Sulfur Oxidation in Scrubber Systems. University of Virginia.
- ↑ Miller, Bruce (2004). Coal Energy Systems. Elsevier Science Technology. pp. 294–299.
- ↑ 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: 1155–6. doi:10.1246/bcsj.57.1155.