Difference between revisions of "Calcium sulfate"
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:Ca(OCl)<sub>2</sub> + K<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + 2KOCl | :Ca(OCl)<sub>2</sub> + K<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + 2KOCl | ||
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===Physical=== | ===Physical=== | ||
It is generally considered to be insoluble, but does have a very low solubility of 0.21g/100ml @20 degrees (Wikipedia) | It is generally considered to be insoluble, but does have a very low solubility of 0.21g/100ml @20 degrees (Wikipedia) | ||
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Calcium sulfate [[thermite]], from which elemental [[calcium]] can be obtained. | Calcium sulfate [[thermite]], from which elemental [[calcium]] can be obtained. | ||
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==Safety== | ==Safety== | ||
| − | + | Anhydrous calcium sulfate will release large amounts of heat if mixed with water. | |
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==References== | ==References== | ||
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===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| − | + | [[Category:Chemical compounds]] | |
[[Category:Calcium compounds]] | [[Category:Calcium compounds]] | ||
[[Category:Sulfates]] | [[Category:Sulfates]] | ||
| + | [[Category:Easily prepared chemicals]] | ||
[[Category:Readily available chemicals]] | [[Category:Readily available chemicals]] | ||
Revision as of 08:54, 5 August 2015
Calcium sulfate is a virtually insoluble inorganic compound with the formula CaSO4. It is commonly formed as a by-product of reactions.
Contents
Properties
Chemical
A very exothermic thermite reaction occurs with aluminium powder, which is used to 'heat boost' reactions such as a titanium dioxide thermite, where the extra heat is needed to reduce the oxide all the way to titanium metal
Double displacement reactions often are chosen to form calcium sulfate as the precipitation of the solid not only drives the reaction but makes the two formed chemicals easy to separate by simply filtering off the sulfate:
- Ca(OCl)2 + K2SO4 → CaSO4 + 2KOCl
Physical
It is generally considered to be insoluble, but does have a very low solubility of 0.21g/100ml @20 degrees (Wikipedia)
Calcium sulfate exists in three hydrates, a dihydrate, a hemihydrate and a anhydrous form. Over 100 degrees the hemihydrate is formed and it looses water to form the anhydrous over 180 degrees. These two forms will slowly absorb water at room temperature to revert back to the dihydrate.
Availability
The hemihydrate is easily available as 'plaster of Paris' in hardware stores. The dihydrate is heavily used as 'drywall', a calcium sulfate construction material. A chalk is made from calcium sulfate (a chalk is not made from chalk, who knew) and in many locations it can be found on the ground as the mineral gypsum
Preparation
A solutions of a soluble sulphate salt such as ammonium sulfate and calcium chloride will precipitate calcium sulfate, which can be washed with cold water and dried.
Projects
Calcium sulfate thermite, from which elemental calcium can be obtained.
Safety
Anhydrous calcium sulfate will release large amounts of heat if mixed with water.
