Calcium acetate
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2008-05-28T08:01:12Z
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| ImageFile = Calcium acetate.png
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| IUPACName = Calcium acetate
| OtherNames = Acetate of lime<br>Calcium ethanoate
| Section1 = {{Chembox Identifiers
| Abbreviations = Ca(OAc)<sub>2</sub>
| CASNo = 62-54-4
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| SMILES = CC([O-)]=O.CC([O-])=O.[Ca++]
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| Section2 = {{Chembox Properties
| Formula = C<sub>4</sub>H<sub>6</sub>O<sub>4</sub>Ca
| MolarMass = 158.138 g/mol
| Appearance = White solid
| Density = 1.6 kg/L
| MeltingPt = 160 °C
| Melting_notes = decomposition to acetone
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| Solubility = 400 g/l
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| Autoignition = 680 - 730 °C
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The [[chemical compound]] '''calcium acetate''' is the [[calcium]] salt of [[acetic acid]]. It has the formula Ca(C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>)<sub>2</sub>. Its standard name is calcium acetate, while calcium ethanoate is the systematic IUPAC name. An older name is acetate of lime. The anhydrous form is very [[hygroscopic]]; therefore the mono[[hydrate]] (Ca(CH<sub>3</sub>COO)<sub>2</sub>.H<sub>2</sub>O, CAS [5743-26-0]) is the common form.
If an alcohol is added to a saturated solution of calcium acetate, a semisolid, flammable gel forms that is much like "canned heat" products such as [[Sterno Canned Heat|Sterno]].<ref>[http://jchemed.chem.wisc.edu/jcesoft/CCA/CCA3/MAIN/CANHEAT/PAGE1.HTM "Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"]</ref>
Chemistry teachers often prepare "California Snowballs", a mixture of calcium acetate solution and [[ethanol]]. The resulting gel is whitish in color, and can be formed to resemble a [[snowball]].
==History==
Because it is inexpensive, calcium acetate was once a common starting material for the synthesis of [[acetone]] before the development of the [[cumene process]].<ref>{{cite journal
| title = Losses Incurred in the Preparation of Acetone by the Distillation of Acetate of Lime.
| author = Leo Frank Goodwin and Edward Tyghe Sterne
| journal = Industrial & Engineering Chemistry
| volume = 12
| issue = 3
| year = 1920
| pages = 240–243
| doi = 10.1021/ie50123a012 }}
</ref>
<ref>{{cite journal
| title = Distillation of Acetate of Lime.
| author = E. G. R. Ardagh, A. D. Bbarbour, G. E. McClellan, and E. W. McBride
| journal = Industrial & Engineering Chemistry
| volume = 16
| issue = 11
| year = 1924
| pages = 1133–1139
| doi = 10.1021/ie50179a013 }}
</ref>
==Uses==
In [[kidney disease]], blood levels of [[phosphate]] may rise (called [[hyperphosphatemia]]) leading to bone problems. Calcium acetate binds phosphate in the diet to lower blood phosphate levels. Side effects of this treatment include upset stomach.
Calcium acetate is a [[food additive]], mainly in candy products.
==References==
<references/>
{{inorganic-compound-stub}}
[[Category:Acetates]]
[[Category:Calcium compounds]]
[[Category:Phosphate binders]]
[[Category:Carboxylic acids]]
[[ar:خلات كالسيوم]]
[[de:Calciumacetat]]
[[es:Acetato de calcio]]
[[fr:Acétate de calcium]]
[[it:Acetato di calcio idrato]]
[[hu:Kalcium-acetát]]
[[nl:Calciumacetaat]]
[[ja:酢酸カルシウム]]
[[pl:Octan wapnia]]