Difference between revisions of "Calcium sulfate"
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| − | '''Calcium sulfate''' is a virtually insoluble inorganic compound with the formula CaSO<sub>4</sub>. It is commonly formed as a by-product of reactions. | + | {{Chembox |
| + | | Name = Calcium sulfate | ||
| + | | Reference = | ||
| + | | IUPACName = Calcium sulfate | ||
| + | | PIN = | ||
| + | | SystematicName = | ||
| + | | OtherNames = Drierite (anhydrous)<br>Gypsum<br>Plaster of Paris | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
| + | | SMILES = | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = White solid | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = Decomposes | ||
| + | | Density = 2.96 g/cm<sup>3</sup> (anhydrous)<br>2.32 g/cm<sup>3</sup> (dihydrate) | ||
| + | | Formula = CaSO<sub>4</sub> | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 136.14 g/mol (anhydrous)<br>145.15 g/mol (hemihydrate)<br>172.172 g/mol (dihydrate) | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = ''anhydrous''<br>1,460 °C (2,660 °F; 1,730 K)<hr>''hemihydrate''<br>180 °C (356 °F; 453 K) (decomposes)<hr>''dihydrate''<br>100–150 °C (212–302 °F; 373–423 K) (decomposes) | ||
| + | | Odor = Odorless | ||
| + | | pKa = 10.4 (anhydrous)<br>7.3 (dihydrate) | ||
| + | | pKb = | ||
| + | | Solubility = 0.21 g/100 ml at 20 °C (anhydrous)<br>0.24 g/100 ml at 20 °C (dihydrate) | ||
| + | | SolubleOther = ''dihydrate''<br>Slightly soluble in [[glycerol]] | ||
| + | | Solvent = | ||
| + | | VaporPressure = | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
| + | | Coordination = | ||
| + | | CrystalStruct = Orthorhombic | ||
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| + | | Section4 = {{Chembox Thermochemistry | ||
| + | | DeltaGf = | ||
| + | | DeltaHc = | ||
| + | | DeltaHf = -1,433 kJ/mol | ||
| + | | Entropy = 107 J·mol<sup>−1</sup>·K<sup>−1</sup> | ||
| + | | HeatCapacity = | ||
| + | }} | ||
| + | | Section5 = {{Chembox Explosive | ||
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| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = Non-flammable | ||
| + | | ExploLimits = Non-explosive | ||
| + | | ExternalMSDS = [https://www.docdroid.net/mGpTgLd/calcium-sulfate-anhydrous-sa.pdf.html Sigma-Aldrich] (drierite)<br>[https://www.docdroid.net/XDuFe6j/calcium-sulfate-hemihydrate-sa.pdf.html Sigma-Aldrich] (hemihydrate)<br>[https://www.docdroid.net/uZK74UP/calcium-sulfate-dihydrate-sa.pdf.html Sigma-Aldrich] (dihydrate) | ||
| + | | FlashPt = Non-flammable | ||
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| + | | MainHazards = Irritant | ||
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| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Magnesium sulfate]]<br>[[Strontium sulfate]]<br>[[Barium sulfate]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Calcium sulfate''' is a virtually insoluble inorganic compound with the formula '''CaSO<sub>4</sub>'''. It is commonly formed as a by-product of reactions. Since it's hygroscopic, it's commonly encountered as hydrate. | ||
| + | |||
| + | Anhydrous calcium sulfate is called ''drierite''. | ||
==Properties== | ==Properties== | ||
===Chemical=== | ===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. | |
| − | 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: | 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)<sub>2</sub> + K<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + | + | :Ca(OCl)<sub>2</sub> + K<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + 2 KOCl |
| + | |||
| + | Anhydrous calcium sulfate (drierite) is one of the few [[desiccant]]s that can be safely used to dry [[acetone]], as most common desiccants tend to cause it to self-condense. Neutral calcium sulfate (no traces of bisulfate or hydroxide) is necessary, as any impurities like bisulfate or hydroxide will cause minor self-condensation. | ||
| + | |||
===Physical=== | ===Physical=== | ||
| − | It is generally considered to be insoluble, but does have a very low solubility of 0. | + | It is generally considered to be insoluble, but does have a very low solubility of 0.21 g/100ml at 20 °C.<ref>https://en.wikipedia.org/wiki/Calcium_sulfate</ref> |
| − | 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. | + | 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 Celsius. These two forms will slowly absorb water at room temperature to revert back to the dihydrate. |
==Availability== | ==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. | + | The hemihydrate is easily available as 'plaster of Paris' in hardware stores. The dihydrate is heavily used as 'drywall', a calcium sulfate construction material. Chalk sticks tend to contain calcium sulfate rather than calcium carbonate (a chalk is not made from [[calcium carbonate|chalk]], who knew), though some formulas may contain traces of calcium carbonate and in many locations it can be found in the ground as the mineral gypsum. |
==Preparation== | ==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 | + | A solutions of a soluble sulphate salt such as [[ammonium sulfate]] and [[calcium chloride]] will precipitate calcium sulfate, which can be filtered and washed with cold water, then dried. To obtain perfectly neutral CaSO<sub>4</sub>, add a slight excess of ammonium sulfate to make sure all the calcium has precipitated, filter it, thoroughly wash the CaSO<sub>4</sub> precipitate and dry it in an oven at 180 °C. |
==Projects== | ==Projects== | ||
| + | *Calcium sulfate [[thermite]], from which elemental [[calcium]] can be obtained. | ||
| + | *Sulfur dioxide generation | ||
| + | *Dry [[acetone]] | ||
| − | + | ==Handling== | |
| − | ==Safety== | + | ===Safety=== |
| + | Anhydrous calcium sulfate will release large amounts of heat if mixed with water. | ||
| + | ===Storage=== | ||
| + | Should be stored in closed containers, away from moisture. | ||
| + | ===Disposal=== | ||
| + | Unless it's contaminated with heavy metals or sodium ions, calcium sulfate can be safely dumped in the ground or trash. Do not pour it down the drain as it may clog the pipes. | ||
==References== | ==References== | ||
<references /> | <references /> | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=21332 Calcium Sulfate and Titanium Thermite] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=66628 Calcium Sulfate as a desiccant - Will anhydrous work?] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=8338 anhydrous calcium sulfate or alumina silicate] | ||
| + | *[https://www.sciencemadness.org/whisper/viewthread.php?tid=6255 What form of Calcium sulfate?] | ||
| + | |||
| + | [[Category:Chemical compounds]] | ||
| + | [[Category:Inorganic compounds]] | ||
| + | [[Category:Calcium compounds]] | ||
| + | [[Category:Sulfates]] | ||
| + | [[Category:Desiccants]] | ||
| + | [[Category:Easily prepared chemicals]] | ||
| + | [[Category:Readily available chemicals]] | ||
| + | [[Category:Essential reagents]] | ||
| + | [[Category:Neutral salts]] | ||
Latest revision as of 21:54, 18 November 2019
| Names | |
|---|---|
| IUPAC name
Calcium sulfate
| |
| Other names
Drierite (anhydrous)
Gypsum Plaster of Paris | |
| Properties | |
| CaSO4 | |
| Molar mass | 136.14 g/mol (anhydrous) 145.15 g/mol (hemihydrate) 172.172 g/mol (dihydrate) |
| Appearance | White solid |
| Odor | Odorless |
| Density | 2.96 g/cm3 (anhydrous) 2.32 g/cm3 (dihydrate) |
| Melting point | anhydrous 1,460 °C (2,660 °F; 1,730 K) hemihydrate 180 °C (356 °F; 453 K) (decomposes) dihydrate 100–150 °C (212–302 °F; 373–423 K) (decomposes) |
| Boiling point | Decomposes |
| 0.21 g/100 ml at 20 °C (anhydrous) 0.24 g/100 ml at 20 °C (dihydrate) | |
| Solubility | dihydrate Slightly soluble in glycerol |
| Acidity (pKa) | 10.4 (anhydrous) 7.3 (dihydrate) |
| Thermochemistry | |
| Std molar
entropy (S |
107 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
-1,433 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (drierite) Sigma-Aldrich (hemihydrate) Sigma-Aldrich (dihydrate) |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Magnesium sulfate Strontium sulfate Barium sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Calcium sulfate is a virtually insoluble inorganic compound with the formula CaSO4. It is commonly formed as a by-product of reactions. Since it's hygroscopic, it's commonly encountered as hydrate.
Anhydrous calcium sulfate is called drierite.
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 + 2 KOCl
Anhydrous calcium sulfate (drierite) is one of the few desiccants that can be safely used to dry acetone, as most common desiccants tend to cause it to self-condense. Neutral calcium sulfate (no traces of bisulfate or hydroxide) is necessary, as any impurities like bisulfate or hydroxide will cause minor self-condensation.
Physical
It is generally considered to be insoluble, but does have a very low solubility of 0.21 g/100ml at 20 °C.[1]
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 Celsius. 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. Chalk sticks tend to contain calcium sulfate rather than calcium carbonate (a chalk is not made from chalk, who knew), though some formulas may contain traces of calcium carbonate and in many locations it can be found in 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 filtered and washed with cold water, then dried. To obtain perfectly neutral CaSO4, add a slight excess of ammonium sulfate to make sure all the calcium has precipitated, filter it, thoroughly wash the CaSO4 precipitate and dry it in an oven at 180 °C.
Projects
- Calcium sulfate thermite, from which elemental calcium can be obtained.
- Sulfur dioxide generation
- Dry acetone
Handling
Safety
Anhydrous calcium sulfate will release large amounts of heat if mixed with water.
Storage
Should be stored in closed containers, away from moisture.
Disposal
Unless it's contaminated with heavy metals or sodium ions, calcium sulfate can be safely dumped in the ground or trash. Do not pour it down the drain as it may clog the pipes.
