Calcium acetate

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Calcium acetate
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Calcium acetate crystals
Names
Preferred IUPAC name
Calcium diacetate[1]
Other names
Acetate of lime
Calcium ethanoate
Identifiers
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3D model (JSmol)
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Abbreviations Ca(OAc)2
3692527
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EC Number Page Template:Plainlist/styles.css has no content.
22320
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  • InChI=1S/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 checkY
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  • InChI=1/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
    Key: VSGNNIFQASZAOI-NUQVWONBAW
  • CC(=O)O[Ca]OC(=O)C
  • [Ca+2].[O-]C(=O)C.[O-]C(=O)C
Properties
Page Module:Chem2/styles.css has no content.Ca(CH3COO)2
Molar mass 158.166 g/mol (anhydrous)
176.181 g/mol (monohydrate)
Appearance White solid
hygroscopic
Odor slight acetic acid odor
Density 1.509 g/cm3
Melting point 160 °C (320 °F; 433 K)[2] decomposition to CaCO3 + acetone
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
Acidity (pKa) ca. 0.7
−70.7·10−6 cm3/mol
1.55
Pharmacology
V03AE07 (WHO)
Hazards
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1
1
0
680 to 730 °C (1,256 to 1,346 °F; 953 to 1,003 K)
Lethal dose or concentration (LD, LC):
4280 mg/kg (oral, rat)
Related compounds
Other cations
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Calcium acetate is a chemical compound which is a calcium salt of acetic acid. It has the formula Page Module:Chem2/styles.css has no content.Ca(CH3COO)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 (Page Module:Chem2/styles.css has no content.Ca(CH3COO)2·H2O) is the common form.

Production

Calcium acetate can be prepared by soaking calcium carbonate (found in eggshells, or in common carbonate rocks such as limestone or marble) or hydrated lime in vinegar:

Page Module:Chem2/styles.css has no content.CaCO3(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + H2O(l) + CO2(g)
Page Module:Chem2/styles.css has no content.Ca(OH)2(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + 2 H2O(l)

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.[3]
  • Calcium acetate is used as a food additive, as a stabilizer, buffer and sequestrant, mainly in candy products under the number E263.
  • Tofu is traditionally obtained by coagulating soy milk with calcium sulfate. Calcium acetate has been found to be a better alternative; being soluble, it requires less skill and a smaller amount.[4]
  • Because it is inexpensive, calcium acetate was once a common starting material for the synthesis of acetone before the development of the cumene process:[5][6]
Page Module:Chem2/styles.css has no content.Ca(CH3COO)2 → CaCO3(s) + (CH3)2CO
  • A saturated solution of calcium acetate in alcohol forms a semisolid, flammable gel that is much like "canned heat" products such as Sterno.[7] Chemistry teachers often prepare "California Snowballs", a mixture of calcium acetate solution and ethanol.[8] The resulting gel is whitish in color, resembling a snowball and can be lit on fire; it will burn for around 20 minutes.[9]

Natural occurrence

Pure calcium acetate is yet unknown among minerals. Calclacite—calcium acetate chloride pentahydrate—is listed as a known mineral,[10] but its genesis is anthropogenic (human-generated, as opposed to naturally occurring).[11]

References

  1. ^ Page Module:Citation/CS1/styles.css has no content.International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. p. 801. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
  2. ^ Page Module:Citation/CS1/styles.css has no content.Dale L. Perry (May 19, 2011). Handbook of Inorganic Compounds (Second ed.). Taylor & Francis. p. 84. ISBN 978-1-4398-1461-1.
  3. ^ Page Module:Citation/CS1/styles.css has no content."Calcium Acetate". Mayo Clinic. Retrieved 19 November 2019.
  4. ^ Page Module:Citation/CS1/styles.css has no content.Lu, J. Y.; Carter, Eloise; Chung, R. A. (1980). "Use of Calcium Salts for Soybean Curd Preparation". Journal of Food Science. 45: 32–34. doi:10.1111/j.1365-2621.1980.tb03864.x.
  5. ^ Page Module:Citation/CS1/styles.css has no content.Leo Frank Goodwin; 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.
  6. ^ Page Module:Citation/CS1/styles.css has no content.E. G. R. Ardagh; A. D. Barbour; G. E. McClellan; E. W. McBride (1924). "Distillation of Acetate of Lime". Industrial & Engineering Chemistry. 16 (11): 1133–1139. doi:10.1021/ie50179a013.
  7. ^ Page Module:Citation/CS1/styles.css has no content.""Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"". Archived from the original on 2008-10-03. Retrieved 2008-03-26.
  8. ^ Page Module:Citation/CS1/styles.css has no content."Chemistry Teaching Resources". University of Manitoba. Archived from the original on 2011-09-23.
  9. ^ Page Module:Citation/CS1/styles.css has no content."CA (California) Snowball". LibreTexts. University of California Davis. Retrieved 2024-12-31.
  10. ^ Page Module:Citation/CS1/styles.css has no content."Calclacite". mindat.org. Archived from the original on 2017-01-20. Retrieved 2024-12-31.
  11. ^ Page Module:Citation/CS1/styles.css has no content."Man made minerals". The Australian Museum. New South Wales Government. 2022-12-08. It [calclacite] owes its existence to humans – it only grows naturally in old oak drawers as it forms when calcium-rich rocks or fossils react with acetic acid in the wood.

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