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Revision as of 18:00, 9 January 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 455227473 of page Strontium_carbonate for the Chem/Drugbox validation project (updated: '').		Latest revision as of 11:46, 7 October 2024 edit Itz.mas10 (talk | contribs)Extended confirmed users704 edits →Uses: appropriate reference to ferrite magnet included
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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
			|Watchedfields = changed
	| verifiedrevid = 442347136
			|verifiedrevid = 470471219
	| ImageFile = SrCO3.jpg
			|ImageFile = SrCO3.jpg
	| ImageSize =
	| IUPACName = Strontium carbonate		|IUPACName = Strontium carbonate
	| OtherNames = ]		|OtherNames = ]
	| Section1 = {{Chembox Identifiers		|Section1 = {{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 14666		|ChemSpiderID = 14666
	| UNII_Ref = {{fdacite|correct|FDA}}		|UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = 41YPU4MMCA		|UNII = 41YPU4MMCA
	| InChI = 1/CH2O3.Sr/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2		|InChI = 1/CH2O3.Sr/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
	| InChIKey = LEDMRZGFZIAGGB-NUQVWONBAS		|InChIKey = LEDMRZGFZIAGGB-NUQVWONBAS
	| SMILES = .C()=O		|SMILES = .C()=O
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/CH2O3.Sr/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2		|StdInChI = 1S/CH2O3.Sr/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = LEDMRZGFZIAGGB-UHFFFAOYSA-L		|StdInChIKey = LEDMRZGFZIAGGB-UHFFFAOYSA-L
	| CASNo = 1633-05-2		|CASNo = 1633-05-2
	| CASNo_Ref = {{cascite|correct|CAS}}		|CASNo_Ref = {{cascite|correct|CAS}}
	| PubChem = 15407		|PubChem = 15407
	| RTECS = WK8305000		|RTECS = WK8305000
			|EINECS = 216-643-7
	}}
	| Section2 = {{Chembox Properties
	| Formula = SrCO<sub>3</sub>
	| MolarMass = 147.63 g/mol
	| Appearance = White or grey powder <br> ]
	| Odor = Odorless
	| Density = 3.5 g/cm<sup>3</sup>
	| MeltingPt = 1290 ºC decomp.
	| Solubility = 0.0011 g/100 ml (18 ºC)
	| RefractIndex = 1.518 <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref>
	}}
	| Section7 = {{Chembox Hazards
	| EUIndex = Not listed
	| NFPA-H = 1
	| NFPA-F = 0
	| NFPA-R = 0
	| NFPA-O =
	| ExternalMSDS =
	| MainHazards =
	| FlashPt = Non-flammable
	}}
	| Section8 = {{Chembox Related
	| OtherAnions =
	| OtherCations = ]<br/>]<br/>]
	| OtherCpds =
	}}
	}}		}}
			|Section2 = {{Chembox Properties
			|Formula = {{chem2|SrCO3}}
			|Sr=1|C=1|O=3
			|Appearance = White powder
			|Odor = Odorless
			|Density = 3.5 g/cm<sup>3</sup><ref name="GESTIS">{{GESTIS|Name=Strontiumcarbonat|ZVG=5190|CAS=1633-05-2|Date=2019-12-19}}</ref>
			|MeltingPtC = 1494
			|MeltingPt_notes = (decomposes)
			|Solubility = 0.0011 g/100 mL (18 °C) <br> 0.065 g/100 mL (100 °C)
			|SolubleOther = Soluble in ] <br> Slightly soluble in ]
			|Solvent = other solvents
			|SolubilityProduct = 5.6{{e|&minus;10}}<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=5–189|edition=99 |language=English}}</ref>
			|RefractIndex = 1.518
			|MagSus = &minus;47.0·10<sup>−6</sup> cm<sup>3</sup>/mol
			}}
			|Section3 = {{Chembox Structure
			|CrystalStruct = Rhombic
			}}
			|Section4 = {{Chembox Hazards
			|NFPA-H = 1
			|NFPA-F = 0
			|NFPA-R = 0
			|ExternalSDS =
			|FlashPt = Non-flammable
			}}
			|Section5 = {{Chembox Related
			|OtherCations = ]<br/>]<br/>]<br/>]<br/>]
			}}
			}}
			'''Strontium carbonate''' (SrCO<sub>3</sub>) is the carbonate salt of ] that has the appearance of a white or grey powder. It occurs in nature as the mineral ].
			== Chemical properties ==
			Strontium carbonate is a white, odorless, tasteless ]. Being a ], it is a weak ] and therefore is reactive with ]s. It is otherwise stable and safe to work with. It is practically insoluble in ] (0.0001&nbsp;g per 100&nbsp;ml). The ] is increased significantly if the water is saturated with ], to 0.1&nbsp;g per 100&nbsp;ml.
			== Preparation ==
			Other than the natural occurrence as a mineral, strontium carbonate is prepared synthetically in one of two processes, both of which start with naturally occurring ], a mineral form of ] (SrSO<sub>4</sub>). In the "black ash" process, celesite is ] with ] at 1100–1300&nbsp;°C to form ].<ref name=hydrometallurgy>{{cite journal |journal= Hydrometallurgy |volume= 84 |issue= 3–4 |year= 2006 |pages= 239–246 |title= Dissolution kinetics of celestite (SrSO<sub>4</sub>) in HCl solution with BaCl<sub>2</sub> |first1= Salih |last1= Aydoğan |first2= Murat |last2= Erdemoğlu |first3= Ali |last3= Aras |first4= Gökhan |last4= Uçar |first5= Alper |last5= Özkan |doi= 10.1016/j.hydromet.2006.06.001 |bibcode= 2006HydMe..84..239A}}</ref> The sulfate is ], leaving the sulfide:
			:SrSO<sub>4</sub> + 2 C → SrS + 2 CO<sub>2</sub>
			A mixture of strontium sulfide with either ] gas or ] then leads to formation of a ] of strontium carbonate.<ref name=Ullmann>{{Ullmann|first1= J. Paul |last1= MacMillan |first2= Jai Won |last2= Park |first3= Rolf |last3= Gerstenberg |first4= Heinz |last4= Wagner |first5= Karl |last5= Köhler |first6= Peter |last6= Wallbrecht |title= Strontium and Strontium Compounds |doi= 10.1002/14356007.a25_321}}</ref><ref name=hydrometallurgy/>
			:SrS + H<sub>2</sub>O + CO<sub>2</sub> → SrCO<sub>3</sub> + H<sub>2</sub>S
			:SrS + Na<sub>2</sub>CO<sub>3</sub> → SrCO<sub>3</sub> + Na<sub>2</sub>S
			In the "direct conversion" or double-decomposition method, a mixture of celesite and sodium carbonate is treated with steam to form strontium carbonate with substantial amounts of undissolved other solids.<ref name=hydrometallurgy/> This material is mixed with ], which dissolves the strontium carbonate to form a solution of ]. Carbon dioxide or sodium carbonate is then used to re-precipitate strontium carbonate, as in the black-ash process.
			== Uses ==
			].]]
			The most common use is as an inexpensive ] in ]s. Strontium and its salts emit a brilliant red color in flame. Unlike other strontium salts, the carbonate salt is generally preferred because of its cost and the fact that it is not ]. Its ability to neutralize acid is also very helpful in pyrotechnics. Another similar application is in ]s.
			Strontium carbonate is used for electronic applications. It is used for manufacturing ] receivers to absorb electrons resulting from the ].<ref>{{cite web |url=http://www.primaryinfo.com/strontium-carbonate.htm |title=Strontium Carbonate |website=primaryinfo.com |accessdate=May 31, 2017}}</ref>
			It is used in the preparation of ], ], strontium oxide, and strontium salts and in refining sugar and certain drugs.
			It is widely used in the ceramics industry as an ingredient in glazes. It acts as a ] and also modifies the color of certain metallic oxides. It has some properties similar to ].
			It is also used in the manufacturing of strontium ] for ]s which are used in ]s and door magnets.<ref>{{cite web |url=https://www.stanfordmagnets.com/ceramic-ferrite-magnets.html |title=Ceramic Ferrite Magnets |website=Stanford Magnets |access-date=Oct 7, 2024}}</ref>
			Strontium carbonate is also used for making some ]s such as ] and also for electroluminescent materials where it is first calcined into ] and then mixed with ] to make ]:x where x is typically ].{{Citation needed|date=November 2015}} This is the "blue/green" phosphor which is sensitive to ] and changes from lime green to blue.{{Citation needed|date=November 2015}} Other ]s can also be used such as ], or ] to get a yellow/orange glow instead.
			Because of its status as a weak ], strontium carbonate can be used to produce many different strontium compounds by simple use of the corresponding acid.
			==Microbial precipitation==
			The ] '']'', '']'' and '']'' can precipitate strontian ] in ]. The strontium exists as ] in ] within the host calcite with the strontium content of up to one percent.<ref>{{cite book|title=Geomicrobiology, Fifth Edition| author1=Henry Lutz Ehrlich| author2=Dianne K Newman| publisher=CRC Press| date=2009|page=177}}</ref>
			==References==
			<references/>
			== External links ==
			*
			{{Strontium compounds}}
			{{Carbonates}}
			{{Authority control}}
			]
			]
			]