Calcium acetate
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| Calcium acetate | |
|---|---|
 |
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| IUPAC name | Calcium acetate |
| Other names | Acetate of lime Calcium ethanoate |
| Identifiers | |
| Abbreviations | Ca(OAc)2 |
| CAS number | [62-54-4] |
| SMILES | CC([O-)]=O.CC([O-])=O.[Ca++] |
| Properties | |
| Molecular formula | C4H6O4Ca |
| Molar mass | 158.138 g/mol |
| Appearance | White solid |
| Density | 1.6 kg/L |
| Melting point |
160 °C (decomposition to acetone) |
| Solubility in water | 400 g/l |
| Hazards | |
| NFPA 704 |
 1
1
0
|
| Autoignition temperature |
680 - 730 °C |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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The chemical compound calcium acetate is the calcium salt of acetic acid. It has the formula Ca(C2H3O2)2. 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 monohydrate (Ca(CH3COO)2.H2O, 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.[1] 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.
[edit] 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.[2] [3]
[edit] 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.
[edit] References
- ^ "Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"
- ^ 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:.
- ^ E. G. R. Ardagh, A. D. Bbarbour, G. E. McClellan, and E. W. McBride (1924). "Distillation of Acetate of Lime.". Industrial & Engineering Chemistry 16 (11): 1133–1139. doi:.
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