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How do you get calcium sulfate?

How do you get calcium sulfate?

The main sources of calcium sulfate are naturally occurring gypsum and anhydrite, which occur at many locations worldwide as evaporites. These may be extracted by open-cast quarrying or by deep mining. World production of natural gypsum is around 127 million tonnes per annum.

What is the chemical equation for calcium sulphate?

Calcium sulfate

PubChem CID 24497
Molecular Formula CaSO4 or CaO4S
Synonyms CALCIUM SULFATE 7778-18-9 Drierite calcium sulphate Anhydrous gypsum More…
Molecular Weight 136.14
Component Compounds CID 1118 (Sulfuric acid) CID 5460341 (Calcium)

What elements are in calcium sulfate?


  • OTHER NAMES: Anhydrous gypsum; also see Overview for synonyms of hydrates.
  • ELEMENTS: Calcium, sulfur, oxygen.
  • COMPOUND TYPE: Salt (inorganic)
  • STATE: Solid.
  • MOLECULAR WEIGHT: 136.14 g/mol.
  • MELTING POINT: 1460°C (2660°F)
  • BOILING POINT: Not applicable.

How do you use calcium sulfate?

Calcium sulfate is a food additive used as an anticaking agent, dough conditioner and strengthener, flour treatment agent, pH regulator, thickenner and yeast food. It is a white or white-yellow fine odorless powder. Due to its high calcium content (16-20%), calcium sulfate can also be used in flour fortification.

What is the difference between calcium carbonate and calcium sulfate?

Carbonate, as a strong base, will trans- form sequentially into HCO3 (aq) and H2CO3(aq), which will liberate gaseous CO2. Sulfate ion is a weak base; therefore it does not protonate significantly and the solubility of calcium sulfate increases only slightly in acidic solution.

What is the common name for calcium sulphate?

Calcium sulfate, CaSO4, is a naturally occurring calcium salt. It is commonly known in its dihydrate form, CaSO4∙2H2O, a white or colourless powder called gypsum. As uncalcined gypsum, the sulfate is employed as a soil conditioner.

Is calcium sulfate an acid or base?

Acidic calcium sulphate (ACS) is a very acidic (pH 1.0-1.5) blend of calcium hydroxide, sulphuric acid and calcium sulphate.

What is the symbol of sulfate?


How do you dissolve calcium sulfate?

According to the present invention, calcium sulfate scale is removed by direct dissolution using DTPA as the chelating agent. The method is particularly useful for the removal of such scale from oil field equipment used to bring oil and/or water from subterranean formations to the surface.

What do you use calcium sulfate for?

Which is better calcium citrate or calcium carbonate?

Calcium citrate supplements are absorbed more easily than calcium carbonate. They can be taken on an empty stomach and are more readily absorbed by people who take acid-reducing heartburn medications. But because calcium citrate is only 21% calcium, you may need to take more tablets to get your daily requirement.

What is the main use of calcium sulfate?

The main use of calcium sulfate is to produce plaster of Paris and stucco. These applications exploit the fact that calcium sulfate which has been powdered and calcined forms a moldable paste upon hydration and hardens as crystalline calcium sulfate dihydrate.

Which is the best way to dissolve caclium sulfate?

Another way to dissolve it, which is unfortunately slow, is to suspend the finely powdered material in water and then to bubble air through it. The CO2 in air gradually dissolves it by producing calcium hydrogen carbonate, which is somewhat more soluble than the original calcium sulphate.

What is the formula for calcium sulfate hemihydrate?

With judicious heating, gypsum converts to the partially dehydrated mineral called calcium sulfate hemihydrate, calcined gypsum, and plaster of Paris.This material has the formula CaSO4·(nH2O), where 0.5 ≤ n ≤ 0.8.

Where does calcium sulfate in cement come from?

In addition to natural sources, calcium sulfate is produced as a by-product in a number of processes: In flue-gas desulfurization, exhaust gases from fossil-fuel power stations and other processes (e.g. cement manufacture) are scrubbed to reduce their sulfur oxide content, by injecting finely ground limestone or lime.