Calcium acetate crystals
|CAS number||, (monohydrate)|
|Jmol-3D images||Image 1|
|Molar mass||158.17 g mol−1|
|Odor||slight acetic acid odor|
|Melting point||160 °C (320 °F; 433 K) decomposition to CaCO3 + acetone|
|Solubility in water||37.4 g/100 mL (0 °C)
34.7 g/100 mL (20 °C)
29.7 g/100 mL (100 °C)
|Solubility||slightly soluble in methanol, hydrazine
insoluble in acetone, ethanol and benzene
|Refractive index (nD)||1.55|
|Autoignition temperature||680 to 730 °C (1,256 to 1,346 °F; 953 to 1,003 K)|
|LD50||4280 mg/kg (oral, rat)|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Calcium acetate is a chemical compound which is a calcium salt of acetic acid. It has the formula Ca(C2H3O2)2. Its standard name is calcium acetate, while calcium ethanoate is the systematic name. An older name is acetate of lime. The anhydrous form is very hygroscopic; therefore the monohydrate (Ca(CH3COO)2•H2O) is the common form.
- CaCO3(s) + 2CH3COOH(l) → Ca(CH3COO)2(l) + H2O(l) + CO2(g)
- Ca(OH)2(s) + 2CH3COOH(l) → Ca(CH3COO)2(l) + 2H2O(l)
Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then.
- 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 used as a food additive, as a stabilizer, buffer and sequestrant, mainly in candy products under the number E263. It also neutralizes fluoride in water.
- Because it is inexpensive, calcium acetate was once a common starting material for the synthesis of acetone before the development of the cumene process:
- Ca(CH3COO)2 → CaO(s) + CO2(g) + (CH3)2CO(v)
- A saturated solution of calcium acetate in alcohol forms a semisolid, flammable gel forms that is much like "canned heat" products such as Sterno.
- Dale L. Perry (May 19, 2011). Handbook of Inorganic Compounds (Second ed.). Taylor & Francis. p. 84. ISBN 978-1-4398-1461-1.
- Polymeric calcium phosphate cements: setting reaction modifiers
- Leo Frank Goodwin and Edward Tyghe Sterne (1920). "Losses Incurred in the Preparation of Acetone by the Distillation of Acetate of Lime.". Industrial & Engineering Chemistry 12 (3): 240–243. doi:10.1021/ie50123a012.
- E. G. R. Ardagh, A. D. Barbour, G. E. McClellan, and E. W. McBride (1924). "Distillation of Acetate of Lime.". Industrial & Engineering Chemistry 16 (11): 1133–1139. doi:10.1021/ie50179a013.
- "Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"
- Chemistry Teaching Resources