Calcium acetate

Calcium acetate crystals
Preferred IUPAC name
Calcium diacetate[1]
Other names
Acetate of lime
Calcium ethanoate
3D model (JSmol)
Abbreviations Ca(OAc)2
ECHA InfoCard 100.000.492 Edit this at Wikidata
EC Number
  • 269-613-0
E number E263 (preservatives)
RTECS number
  • AF7525000
  • InChI=1S/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 checkY
  • InChI=1/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
  • CC(=O)O[Ca]OC(=O)C
  • [Ca+2].[O-]C(=O)C.[O-]C(=O)C
Molar mass 158.166 g/mol (anhydrous)
176.181 g/mol (monohydrate)
Appearance White solid
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
V03AE07 (WHO)
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
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
Magnesium acetate
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 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.


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:

CaCO3(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + H2O(l) + CO2(g)
Ca(OH)2(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + 2H2O(l)

Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then.


Ca(CH3COO)2 → CaCO3(s) + (CH3)2CO

Natural occurrence

Pure calcium acetate is yet unknown among minerals. Calclacitecalcium acetate chloride pentahydrate—is listed as a known mineral,[9] but its genesis is likely anthropogenic (human-generated, as opposed to naturally occurring).[10][failed verification]


  1. ^ 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. ^ Dale L. Perry (May 19, 2011). Handbook of Inorganic Compounds (Second ed.). Taylor & Francis. p. 84. ISBN 978-1-4398-1461-1.
  3. ^ "Calcium Acetate". Mayo Clinic. Retrieved 19 November 2019.
  4. ^ J. Y. Lu, Eloise Carter and R. A. Chung (1980): "Use of Calcium Salts for Soybean Curd Preparation" Journal of Food Science, volume 45, issue 1, pages 32–34 doi:10.1111/j.1365-2621.1980.tb03864.x
  5. ^ 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. ^ 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. ^ ""Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"". Archived from the original on 2008-10-03. Retrieved 2008-03-26.
  8. ^ Chemistry Teaching Resources
  9. ^ "Calclacite".
  10. ^ RRUFF (13 Jan 2024). "Database of Mineral Properties". International Mineralogical Association. Calclacite (dropdown option at left).