Calcium acetate: Difference between revisions
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<ref>{{cite journal |
<ref>{{cite journal |
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| title = Distillation of Acetate of Lime. |
| title = Distillation of Acetate of Lime. |
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| author = E. G. R. Ardagh, A. D. |
| author = E. G. R. Ardagh, A. D. Barbour, G. E. McClellan, and E. W. McBride |
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| journal = Industrial & Engineering Chemistry |
| journal = Industrial & Engineering Chemistry |
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| volume = 16 |
| volume = 16 |
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Revision as of 18:40, 31 August 2010
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| Names | |
|---|---|
| IUPAC name
Calcium acetate
| |
| Other names
Acetate of lime
Calcium ethanoate | |
| Identifiers | |
3D model (JSmol)
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| Abbreviations | Ca(OAc)2 |
| ChemSpider | |
| ECHA InfoCard | 100.000.492 |
| E number | E263 (preservatives) |
CompTox Dashboard (EPA)
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|
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| Properties | |
| C4H6CaO4 | |
| Molar mass | 158.166 g·mol−1 |
| Appearance | White solid hygroscopic |
| Density | 1.6 g/cm3 |
| Melting point | 160 °C |
| 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 insoluble in acetone, ethanol and benzene |
| Acidity (pKa) | 6.3-9.6 |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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4280 mg/kg (oral, rat) |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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.
Calclacite is a name for calcium acetate chloride pentahydrate, which is treated as mineral species but possess anthropogenic origin.
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]
Calcium Acetate can be prepared by soaking eggshells in vinegar. Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then.
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 used as a food additive, as a stabilizer, buffer and sequestrant, mainly in candy products. It also neutralizes fluoride in water.
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: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.
{{cite journal}}: CS1 maint: multiple names: authors list (link)