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Calcium acetate

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Calcium acetate is a chemical compound which is a calcium saltofacetic 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
Names

Calcium acetate crystals
Preferred IUPAC name Calcium diacetate^[1]
Other names Acetate of lime Calcium ethanoate
Identifiers
CAS Number	62-54-4^Y 5743-26-0 (monohydrate)^Y
3D model (JSmol)	Interactive image Interactive image
Abbreviations	Ca(OAc)₂
Beilstein Reference	3692527
ChEBI	CHEBI:3310^Y
ChEMBL	ChEMBL1200800^N
ChemSpider	5890^Y
DrugBank	DB00258^Y
ECHA InfoCard	100.000.492
EC Number	269-613-0
E number	E263 (preservatives)
Gmelin Reference	22320
KEGG	D00931^Y
PubChem CID	6116
RTECS number	AF7525000
UNII	Y882YXF34X^Y 7ZA48GIM5H (monohydrate)^Y
CompTox Dashboard (EPA)	DTXSID0020234
InChI InChI=1S/2C2H4O2.Ca/c21-2(3)4;/h21H3,(H,3,4);/q;;+2/p-2^Y Key: VSGNNIFQASZAOI-UHFFFAOYSA-L^Y InChI=1/2C2H4O2.Ca/c21-2(3)4;/h21H3,(H,3,4);/q;;+2/p-2 Key: VSGNNIFQASZAOI-NUQVWONBAW
SMILES CC(=O)O[Ca]OC(=O)C [Ca+2].[O-]C(=O)C.[O-]C(=O)C
Properties
Chemical formula	C₄H₆CaO₄
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
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
Acidity (pK_a)	ca. 0.7
Magnetic susceptibility (χ)	-70.7·10⁻⁶cm³/mol
Refractive index (n_D)	1.55
Pharmacology
ATC code	V03AE07 (WHO)
Hazards
NFPA 704 (fire diamond)	1 1 0
Autoignition temperature	680 to 730 °C (1,256 to 1,346 °F; 953 to 1,003 K)
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	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). N verify (what is ^YN ?) Infobox references

Production

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Calcium acetate can be prepared by soaking calcium carbonate (found in eggshells, or in common carbonate rocks such as limestoneormarble) or hydrated limeinvinegar:

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.

Uses

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Inkidney 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]

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, and can be formed to resemble a snowball.

Natural occurrence

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Pure calcium acetate is yet unknown among minerals. Calclacite—calcium 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]}

References

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^ 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.

^ Dale L. Perry (May 19, 2011). Handbook of Inorganic Compounds (Second ed.). Taylor & Francis. p. 84. ISBN 978-1-4398-1461-1.

^ "Calcium Acetate". Mayo Clinic. Retrieved 19 November 2019.

^ 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

^ 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.

^ 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.

^ ""Canned Heat" at Journal of Chemical Education "Chemistry comes alive!"". Archived from the original on 2008-10-03. Retrieved 2008-03-26.

^ Chemistry Teaching Resources

^ "Calclacite".

^ RRUFF (13 Jan 2024). "Database of Mineral Properties". International Mineralogical Association. Calclacite (dropdown option at left).

Retrieved from "https://en.wikipedia.org/w/index.php?title=Calcium_acetate&oldid=1211700415" Last edited on 3 March 2024, at 23:45

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