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Revision as of 15:14, 17 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 472544120 of page Calcium_formate for the Chem/Drugbox validation project (updated: 'ChemSpiderID', 'StdInChI', 'StdInChIKey', 'CASNo').		Latest revision as of 09:25, 20 September 2024 edit Novadeluxer (talk | contribs)7 editsm Typo (missing preposition "of")Tag: Visual edit
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	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
	{{chembox		{{chembox
			| Verifiedfields = changed
	| Watchedfields = changed		| Watchedfields = changed
	| verifiedrevid = 444376086		| verifiedrevid = 477376233
	| Name = Calcium formate		| Name = Calcium formate
	| Reference = <ref name="hand">		| Reference =
			| ImageFile = Calcium formate structure.png
	{{Citation
	| last = Lide		| ImageSize =
			| ImageName = Calcium formate
	| first = David R.
			| ImageFile1 = Calcium diformate ball-and-stick.png
	| author-link =
			| PIN = Calcium diformate
	| last2 =
			| OtherNames = {{Unbulleted list|Formic acid calcium salt|calcoform}}
	| first2 =
			|Section1={{Chembox Identifiers
	| author2-link =
			| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| publication-date =
			| ChemSpiderID = 10531
	| date =
	| year = 1998
	| title = Handbook of Chemistry and Physics
	| edition = 87
	| volume =
	| series =
	| publication-place = Boca Raton, FL
	| place =
	| publisher = CRC Press
	| id =
	| isbn = 0-8493-0594-2
	| doi =
	| oclc =
	| pages = 4–49
	| url =
	| accessdate =
	}}</ref>
	| ImageFile = Calcium formate structure.png
	| ImageSize =
	| ImageName = Calcium formate
	| OtherNames = formic acid calcium salt, calcoform
	| Section1 = {{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 8932
	| InChI = 1/2CH2O2.Ca/c2*2-1-3;/h2*1H,(H,2,3);/q;;+2/p-2		| InChI = 1/2CH2O2.Ca/c2*2-1-3;/h2*1H,(H,2,3);/q;;+2/p-2
	| SMILES = .C=O.C=O		| SMILES = .C=O.C=O
	| InChIKey = CBOCVOKPQGJKKJ-NUQVWONBAS		| InChIKey = CBOCVOKPQGJKKJ-NUQVWONBAS
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/2C6H12O7.Ca/c2*7-1-2(8)3(9)4(10)5(11)6(12)13;/h2*2-5,7-11H,1H2,(H,12,13);/q;;+2/p-2/t2*2-,3-,4+,5-;/m11./s1		| StdInChI = 1S/2CH2O2.Ca/c2*2-1-3;/h2*1H,(H,2,3);/q;;+2/p-2
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = NEEHYRZPVYRGPP-IYEMJOQQSA-L		| StdInChIKey = CBOCVOKPQGJKKJ-UHFFFAOYSA-L
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|PubChem}}
	| CASNo = 299-28-5		| CASNo = 544-17-2
	| EINECS = 208-863-7		| ChEBI = 81851
			| EINECS = 208-863-7
	| KEGG_Ref = {{keggcite|correct|kegg}}		| KEGG_Ref = {{keggcite|correct|kegg}}
	| KEGG = C18586		| KEGG = C18586
	| PubChem = 10997		| PubChem = 10997
	| RTECS = LQ5600000		| RTECS = LQ5600000
			| UNII = NP3JD65NPY
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Formula = Ca(HCOO)<sub>2</sub>		| Formula = Ca(HCO<sub>2</sub>)<sub>2</sub>
	| MolarMass = 130.113 g/mol		| MolarMass = 130.113 g/mol
			| Appearance = white-to-yellow crystals or crystalline powder<ref>{{Cite web|url=http://www.ilo.org/dyn/icsc/showcard.display?p_lang=en&p_card_id=1634|title=ICSC 1634 – Calcium formate|website=www.ilo.org|access-date=2019-02-12}}</ref>
	| ExactMass = 129.9579
			| Odor = smells slightly like ]<ref name=":mer" />
	| Appearance = white powder
			| Density = 2.02 g/cm<sup>3</sup><ref name=":cr" />
	| Odor = weak, caramel-like odor
			| Solubility = 16.1 g/100 g (0 °C)<br>18.4 g/100 g (100 °C)
	| Density = 2.009 g/cm<sup>3</sup>
			| MeltingPt = decomposes at 300 °C<ref name=":cr">{{Cite book|title=CRC handbook of chemistry and physics|others=Haynes, WM|year=2014|isbn=9781482208689|edition=95th|pages=55|chapter=4|last1=Haynes|first1=William M.}}</ref>
	| Solubility = 16.1 g/100 mL (0 °C) <br> 16.6 g/100 mL (20°C) <br> 18.4 g/100 mL (100 °C)
			| SolubleOther = insoluble in ]<ref name=":cr" /><br>]:<br>0.27 g/100 g (15 °C)<br>0.23 g/100 g (66 °C)<ref name=":ge" />
	| MeltingPt = decomposes at 300°C
	| BoilingPt =
	| SolubleOther = insoluble in ]
	}}		}}
	| Section7 = {{Chembox Hazards		|Section7={{Chembox Hazards
			| LD50 = rats: 2640 mg/kg (oral), 154 mg/kg (IV)<ref name=":ge" />
	| EUClass = not listed
			| GHSPictograms = {{GHS05}}{{GHS07}}
	| NFPA-H = 1
	| NFPA-R = 0		| GHSSignalWord = Danger
			| HPhrases = {{H-phrases|318}}
	| NFPA-F = 0
			| PPhrases = {{P-phrases|264|280|305+351+338|310|337+313}}
			| NFPA-H = 1
			| NFPA-R = 0
			| NFPA-F = 0
	}}		}}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherAnions = ]		| OtherAnions = ]
	| OtherCations = ]		| OtherCations = ]
	| OtherFunctn =		| OtherFunction =
			| OtherFunction_label =
	| Function =
	| OtherCpds =		| OtherCompounds =
	}}		}}
	}}		}}
			'''Calcium formate''' is the ] ] of ]. It is also known as '''E238'''. Under this ] it is used as an ] ] within ], but not in foods intended for people.<ref name=":0">{{Cite journal|date=2014|title=Scientific Opinion on the safety and efficacy of calcium formate when used as a technological additive for all animal species|journal=EFSA Journal|volume=12|issue=11|doi=10.2903/j.efsa.2014.3898|issn=1831-4732|doi-access=free}}</ref>
			Calcium formate is stable at room temperature,<ref name=":0" /> is flammable and forms ] crystals.<ref name=":mer">{{Cite book|title=The Merck index|date=2000|publisher=Chapman & Hall Electronic Pub. Division|others=S Budavari, M O'Neil, A Smith|isbn=9781584881292|edition=12th|pages=1675}}</ref> The mineral form is very rare and called formicaite, and is known from a few ] deposits.
			==Uses==
			Calcium formate is used within EU as an animal feed preservative. It acidifies the feed thus preventing microbe growth and increasing shelf life. About 15 g of calcium formate addition per kg of feed lowers its ] by one. 15 g/kg is the maximum recommended feed concentration within EU – this level is thought to be safe for pigs, chickens, fish and ]s. The compound is not environmentally harmful in feed use at these levels. Calcium formate prevents the growth of ] such as ''], ], ]'' and '']'' in ]. It also prevents the growth of ] like '']'' and '']''. However, the relevance of these experimental observations to feed preservation is not known.<ref name=":0" />
			Calcium formate is used as a masking agent in the ] of leather. Calcium formate in tannage formulation promotes faster, more efficient leather penetration of the chrome. Calcium formate can also be used as a replacement for ] in the pickling operation.<ref name=":ge">{{Cite web|url=http://www.geosc.com/Assets/Files/Products-Docs/P-C-Product-Docs/Trimet-Products/CAF-TDS-US-Format.pdf|title=Calcium Formate Product Data|date=2015|website=GEO Specialty Chemicals|access-date=2019-02-11}}</ref>
			As a ] and ] additive, calcium formate imparts a number of desirable properties in the final product, e.g. increased hardness and decreased setting time. Its addition is desirable for work at low temperature and for inhibition of corrosion of metal substrates within cement/grout. It is also effective in the prevention of ]. In ] (gypsum board), calcium formate can function as a ].<ref name=":ge" />
			Calcium formate and ] mixtures are effective ]s, and tend to cause less corrosion of steel and cement surfaces relative to some other deicers.<ref name=":ge" />
			==Research==
			Calcium formate seems to be safe as a ] for people with one time doses of 3.9 g (1200 of calcium) per day.<ref>{{Cite journal|last1=Hanzlik|first1=RP|last2=Fowler|first2=SC|last3=Eells|first3=JT|date=2005|title=Absorption and elimination of formate following oral administration of calcium formate in female human subjects|journal=Drug Metabolism and Disposition|volume=33|issue=2|pages=282–286|doi=10.1124/dmd.104.001289|issn=0090-9556|pmid=15547050|hdl=1808/5937|s2cid=5956107|hdl-access=free}}</ref> Increases in blood formate concentration have been observed with such doses, but in healthy subjects the formate does not accumulate, and is quickly metabolized. Calcium formate is shown to be more readily absorbed form of calcium than ] and ].<ref>{{Cite journal|last1=Hanzlik|first1=RP|last2=Fowler|first2=SC|last3=Fisher|first3=DH|date=2005|title=Relative bioavailability of calcium from calcium formate, calcium citrate, and calcium carbonate|journal=The Journal of Pharmacology and Experimental Therapeutics|volume=313|issue=3|pages=1217–1222|doi=10.1124/jpet.104.081893|issn=0022-3565|pmid=15734899|hdl=1808/5936|s2cid=4976426|hdl-access=free}}</ref> No optic nerve damage has been observed with calcium formate supplementation – along with ], formate is a major metabolic product of ], which can cause blindness upon ingestion.<ref>{{Cite journal|last=MM Altaweel|display-authors=etal|date=2009|title=Ocular and systemic safety evaluation of calcium formate as a dietary supplement|journal=Journal of Ocular Pharmacology and Therapeutics|volume=25|issue=3|pages=223–230|doi=10.1089/jop.2008.0128|issn=1557-7732|pmid=19456257|hdl=1808/8319|url=https://kuscholarworks.ku.edu/bitstream/1808/8319/1/39989396.pdf|hdl-access=free}}</ref>
			Calcium formate could be used to remove environmentally harmful (see ]) ] (SO<sub>X</sub>) from fossil fuel exhausts of e.g. power plants. Calcium formate is added to wet calcium carbonate to promote the formation of ] when exhaust is run through it. This process is called wet flue gas ] (WFGS). Gypsum binds sulfur oxides thus reducing their release to the environment via exhaust. Calcium formate seems to be more effective than or almost equally as effective as some other industrially used WFGS agents.<ref>{{Cite journal|last=Z Li|display-authors=etal|date=2017|title=Effect of calcium formate as an additive on desulfurization in power plants|journal=Journal of Environmental Sciences|volume=67|pages=89–95|doi=10.1016/j.jes.2017.06.023|pmid=29778177}}</ref>
			==Production==
			Calcium formate is formed as a co-product during ] production. Hydrated lime (]) is used as the source of calcium. ] and ] react in a water solution in the presence of a basic ], forming an unstable ], ] (DIMBA). DIMBA reacts further with formaldehyde to give trimethylolpropane and calcium formate. Calcium formate is separated from the solution, heat treated to remove formaldehyde and then dried.<ref name=":0" />
			Calcium formate can also be made from calcium hydroxide and ] at high pressure and temperature<ref name=":mer" /> – e.g., at 180 °C and 35 ].<ref>{{cite patent|country=US|number=1920851A|status=patent|title=Process for producing formates of alkaline earth metals|url=https://patents.google.com/patent/US1920851A}}</ref> It may also be made from ] and ].<ref name=":mer" />
			==Safety==
			Pure calcium formate powder irritates eyes severely, but causes no skin irritation. Powder inhalation can be dangerous.<ref name=":0" /> The compound has a stinging taste. Ingesting liquids with high calcium formate concentrations cause severe gastrointestinal lesions.<ref>{{Cite journal|last1=Scott|first1=DJ|last2=van Wijk|first2=N|date=2000|title=Comparison in dairy cattle of mucosal toxicity of calcium formate and calcium chloride in oil|journal=New Zealand Veterinary Journal|volume=48|issue=1|pages=24–26|doi=10.1080/00480169.2000.36153|issn=0048-0169|pmid=16032113|s2cid=42365225}}</ref>
			==References==
			{{Reflist}}
			{{Calcium compounds}}
			]
			]
			]