View source for Calcium acetate

{{short description|Chemical compound}}
{{chembox
| Verifiedfields = changed
| Watchedfields  = changed
| verifiedrevid  = 476999801
| ImageFile      = Calcium acetate.svg
| ImageSize      = 160px
| ImageFile1     = ca-acetate.png
| ImageCaption1  = Calcium acetate crystals
| PIN            = Calcium diacetate<ref>{{cite book |author=[[International Union of Pure and Applied Chemistry]] |date=2014 |title=Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 |publisher=[[Royal Society of Chemistry|The Royal Society of Chemistry]] |pages=801 |doi=10.1039/9781849733069 |isbn=978-0-85404-182-4}}</ref>
| OtherNames     = Acetate of lime<br>Calcium ethanoate
| Section1       = {{Chembox Identifiers
| Abbreviations = Ca(OAc)<sub>2</sub>
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 5890
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = Y882YXF34X
| UNII1_Ref = {{fdacite|correct|FDA}}
| UNII1 = 7ZA48GIM5H
| UNII1_Comment = (monohydrate)
| InChIKey = VSGNNIFQASZAOI-NUQVWONBAW
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = VSGNNIFQASZAOI-UHFFFAOYSA-L
| CASNo = 62-54-4
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo1 = 5743-26-0
| CASNo1_Ref = {{cascite|correct|CAS}}
| CASNo1_Comment = (monohydrate)
| EINECS = 269-613-0
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| ChEMBL = 1200800
| PubChem = 6116
| DrugBank_Ref = {{drugbankcite|correct|drugbank}}
| DrugBank = DB00258
| Beilstein = 3692527
| Gmelin = 22320
| SMILES = CC(=O)O[Ca]OC(=O)C
| SMILES1 = [Ca+2].[O-]C(=O)C.[O-]C(=O)C
| InChI = 1/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
| RTECS = AF7525000
| MeSHName =
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 3310
| KEGG_Ref = {{keggcite|correct|kegg}}
| KEGG = D00931
 }}
| Section2       = {{Chembox Properties
| C=4 | H=6 | O=4 | Ca=1
| MolarMass = 158.166 g/mol (anhydrous)<br />176.181 g/mol (monohydrate)
| Appearance = White solid <br> [[hygroscopic]]
| Odor = slight [[acetic acid]] odor
| Density = 1.509 g/cm<sup>3</sup>
| MeltingPtC = 160
| MeltingPt_ref = <ref>{{cite book|author=Dale L. Perry|title=Handbook of Inorganic Compounds|url=https://books.google.com/books?id=SFD30BvPBhoC&pg=PA84|edition=Second|date=May 19, 2011|publisher=Taylor & Francis|isbn=978-1-4398-1461-1|page=84}}</ref>
| MeltingPt_notes = decomposition to CaCO<sub>3</sub> + acetone
| BoilingPt = 
| BoilingPt_notes = 
| Solubility = 37.4 g/100 mL (0 °C) <br> 34.7 g/100 mL (20 °C) <br> 29.7 g/100 mL (100 °C)
| SolubleOther = slightly soluble in [[methanol]], [[hydrazine]] <br> insoluble in [[acetone]], [[ethanol]] and [[benzene]]
| pKa = ca. 0.7
| pKb =
| RefractIndex = 1.55
| MagSus = −70.7·10<sup>−6</sup> cm<sup>3</sup>/mol
 }}
| Section3       = {{Chembox Structure
| CrystalStruct = 
| Coordination = 
| MolShape = }}
| Section5       = {{Chembox Thermochemistry
| DeltaHf = 
| DeltaHc = 
| Entropy = 
| HeatCapacity = }}
| Section6       = {{Chembox Pharmacology
| ATCCode_prefix = V03
| ATCCode_suffix = AE07
| ATC_Supplemental =
| AdminRoutes =
| Bioavail = 
| Metabolism = 
| HalfLife = 
| ProteinBound =
| Excretion = 
| Legal_status =
| Legal_US =
| Legal_UK =
| Legal_AU =
| Legal_CA =
| Pregnancy_category = 
| Pregnancy_AU = 
 }}
| Section4       = {{Chembox Explosive
| ShockSens = 
| FrictionSens = 
| DetonationV = 
| REFactor = }}
| Section7       = {{Chembox Hazards
| MainHazards = 
| NFPA-H = 1
| NFPA-F = 1
| NFPA-R = 0
| NFPA-S =
| FlashPt = 
| AutoignitionPtC = 680 to 730
| ExploLimits = 
| LD50 = 4280 mg/kg (oral, rat)
| PEL = }}
| Section8       = {{Chembox Related
| OtherAnions = 
| OtherCations = [[Magnesium acetate]]
| OtherFunction = 
| OtherFunction_label = 
| OtherCompounds = }}
}}

'''Calcium acetate''' is a [[chemical compound]] which is a [[calcium]] [[salt (chemistry)|salt]] of [[acetic acid]]. It has the formula Ca(C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>)<sub>2</sub>. 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 mono[[hydrate]] (Ca(CH<sub>3</sub>COO)<sub>2</sub>•H<sub>2</sub>O) 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 [[Calcium hydroxide|hydrated lime]] in [[vinegar]]:
:CaCO<sub>3</sub>(s) + [[Acetic acid|2CH<sub>3</sub>COOH]](aq) → Ca(CH<sub>3</sub>COO)<sub>2</sub>(aq) + H<sub>2</sub>O(l) + CO<sub>2</sub>(g)
:Ca(OH)<sub>2</sub>(s) + 2CH<sub>3</sub>COOH(aq) → Ca(CH<sub>3</sub>COO)<sub>2</sub>(aq) + 2H<sub>2</sub>O(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.<ref>{{cite web |title=Calcium Acetate |url=https://www.mayoclinic.org/drugs-supplements/calcium-acetate-oral-route/description/drg-20062494 |website=Mayo Clinic |access-date=19 November 2019}}</ref>
* 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.<ref name=jylu>{{cite journal | doi = 10.1111/j.1365-2621.1980.tb03864.x | title = Use of Calcium Salts for Soybean Curd Preparation | date = 1980 | last1 = Lu | first1 = J. Y. | last2 = Carter | first2 = Eloise | last3 = Chung | first3 = R. A. | journal = Journal of Food Science | volume = 45 | pages = 32–34 }}</ref>
* Because it is inexpensive, calcium acetate was once a common starting material for the synthesis of [[acetone]] before the development of the [[cumene process]]:<ref>{{cite journal
| title = Losses Incurred in the Preparation of Acetone by the Distillation of Acetate of Lime.
|author1=Leo Frank Goodwin |author2=Edward Tyghe Sterne | journal = Industrial & Engineering Chemistry
| volume = 12
| issue = 3
| year = 1920
| pages = 240–243
| doi = 10.1021/ie50123a012 |url=https://zenodo.org/record/1428748 }}</ref><ref>{{cite journal
| title = Distillation of Acetate of Lime.
|author1=E. G. R. Ardagh |author2=A. D. Barbour |author3=G. E. McClellan |author4=E. W. McBride | journal = Industrial & Engineering Chemistry
| volume = 16
| issue = 11
| year = 1924
| pages = 1133–1139
| doi = 10.1021/ie50179a013 }}</ref>
: Ca(CH<sub>3</sub>COO)<sub>2</sub> →  CaCO<sub>3</sub>(s) + (CH<sub>3</sub>)<sub>2</sub>CO
* A saturated solution of calcium acetate in alcohol forms a semisolid, flammable gel that is much like "canned heat" products such as [[Sterno]].<ref>{{Cite web |url=http://jchemed.chem.wisc.edu/jcesoft/CCA/CCA3/MAIN/CANHEAT/PAGE1.HTM |title="Canned Heat" at Journal of Chemical Education "Chemistry comes alive!" |access-date=2008-03-26 |archive-date=2008-10-03 |archive-url=https://web.archive.org/web/20081003142048/http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA3/MAIN/CANHEAT/PAGE1.HTM |url-status=dead }}</ref>  Chemistry teachers often prepare "California Snowballs", a mixture of calcium acetate solution and [[ethanol]].<ref>{{cite web |url=http://umanitoba.ca/outreach/crystal/chemistry.html |title=Chemistry Teaching Resources |archive-url=https://web.archive.org/web/20110923051746/https://umanitoba.ca/outreach/crystal/chemistry.html |archive-date=2011-09-23 |url-status=dead |website=[[University of Manitoba]]}}</ref> The resulting gel is whitish in color, resembling a [[snowball]] and can be lit on fire; it will burn for around 20 minutes.<ref>{{cite web |title=CA (California) Snowball |url=https://chem.libretexts.org/Courses/University_of_California_Davis/UCDemos/CA_(California)_Snowball |website=[[LibreTexts]] |publisher=[[University of California Davis]] |access-date=2024-12-31}}</ref>

==Natural occurrence==
Pure calcium acetate is yet unknown among minerals. {{nowrap|[[Calclacite]]{{mdash}}}}calcium acetate chloride {{nowrap|pentahydrate{{mdash}}}}is listed as a known mineral,<ref>{{Cite web |url=http://www.mindat.org/min-862.html |title=Calclacite |access-date=2024-12-31 |archive-date=2017-01-20 |archive-url=https://web.archive.org/web/20170120095111/http://www.mindat.org/min-862.html |url-status=live |website=mindat.org}}</ref> but its genesis is anthropogenic (human-generated, as opposed to naturally occurring).<ref>{{cite web |title=Man made minerals |url=https://australian.museum/learn/minerals/what-are-minerals/man-made-minerals/ |website=[[The Australian Museum]] |publisher=[[New South Wales Government]] |date=2022-12-08 |quote=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.}}</ref>

==References==
<references/>

{{Drugs for treatment of hyperkalemia and hyperphosphatemia}}
{{clear}}
{{Acetates}}{{Calcium compounds}}
[[Category:Acetates]]
[[Category:Calcium compounds]]
[[Category:Phosphate binders]]
[[Category:E-number additives]]