Calcium sulfite
Calcium sulfite, or calcium sulphite, is a chemical compound, the calcium salt of sulfite with the formula CaSO·x(HO). Two crystalline forms are known, the hemihydrate and the tetrahydrate, respectively CaSO·½(HO) and CaSO·4(HO). 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 SO, 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 SO from flue gases is by treating the effluent with Ca(OH) hydrated lime or CaCO limestone. Scrubbing with limestone follows the following idealized reaction: Scrubbing with hydrated lime follows the following idealized reaction: The resulting calcium sulfite oxidizes in air to give gypsum: 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. 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. Gypsum. There is a possibility to use calcium sulfite to produce gypsum by oxidizing (adding O) it in water mixture with the manganese (Mn) cation or sulfuric acid catalyzers. Structure. The structure of calcium sulfite has been examined by X-ray crystallography. These studies show that sulfite anion adopts its characteristic pyramidal geometry. The Ca 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 Ca(SO)2(SO)12HO and Ca(SO)2(SO)12HO. 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(SO)(HO)] cations and either sulfite or sulfate as the anion. Natural occurrence. Calcium sulfite(III) hemihydrate occurs in the nature as the rare mineral hannebachite.