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			{{Short description|Chemical compound}}
	{{chembox		{{chembox
			| Verifiedfields = changed
	| verifiedrevid = 401813215
			| Watchedfields = changed
	| Name = Barium carbonate
			| verifiedrevid = 443182359
	| ImageFile=Barium carbonate.png
			| Name = Barium carbonate
	| ImageSize=120px
			| ImageFile = Barium carbonate.png
	| ImageFile2=Uhličitan barnatý.JPG
			| ImageSize = 150px
	| ImageSize2=120px
	| ImageName2=Barium carbonate		| ImageName = Skeletal formula of barium carbonate
			| ImageFile1 = Uhličitan barnatý.JPG
	| OtherNames = ]
			| ImageFile2 = Barium-carbonate-3D-vdW.png
	| Section1 = {{Chembox Identifiers
			| ImageName1 = Powder of barium carbonate
	| UNII_Ref = {{fdacite|correct|FDA}}
			| OtherNames = ]
			| IUPACName =
			| SystematicName =
			| Section1 = {{Chembox Identifiers
			| UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = 6P669D8HQ8		| UNII = 6P669D8HQ8
	| InChI = 1/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2		| InChI = 1/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
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	| StdInChIKey = AYJRCSIUFZENHW-UHFFFAOYSA-L		| StdInChIKey = AYJRCSIUFZENHW-UHFFFAOYSA-L
	| CASNo = 513-77-9		| CASNo = 513-77-9
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
	| EINECS = 208-167-3		| EINECS = 208-167-3
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=10121		| ChemSpiderID=10121
	| UNNumber = 1564		| ChEBI = 190439
	| RTECS = CQ8600000		| UNNumber = 1564
			| RTECS = CQ8600000
			| PubChem = 10563
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = BaCO<sub>3</sub>		| Formula = BaCO<sub>3</sub>
			| Appearance = white crystals
	| MolarMass = 197.34 g/mol
			| Odor = odorless
	| Appearance = white crystals
	| Density = 4.286 g/cm<sup>3</sup>		| Density = 4.286 g/cm<sup>3</sup>
	| Solubility = 0.0024 g/100 mL (20 °C)		| MolarMass = 197.34 g/mol
			| Solubility = 16 mg/L (8.8°C)<br> 22 mg/L (18 °C)<br> 24 mg/L (20 °C)<br> 24 mg/L (24.2 °C)<ref name=chemister />
	| SolubleOther = soluble in ], ], ] <br> insoluble in ]
			| SolubleOther = decomposes in ]<br> insoluble in ]
	| MeltingPt = 811 °C
			| MeltingPtC = 811
	| BoilingPt = 1360 °C (decomp)
			| MeltingPt_notes = <br> polymorphic transformation
	| RefractIndex = 1.60
			| BoilingPtC = 1450
			| BoilingPt_notes = <br> decomposes<ref name=chemister /> from 1360&nbsp;°C
			| RefractIndex = 1.676
			| SolubilityProduct = 2.58·10<sup>−9</sup>
			| MagSus = -58.9·10<sup>−6</sup> cm<sup>3</sup>/mol
			}}
			| Section3 = {{Chembox Structure
			| Coordination =
			| CrystalStruct = orthorhombic
	}}		}}
	| Section7 = {{Chembox Hazards		| Section4 = {{Chembox Thermochemistry
			| DeltaHf = -1219 kJ/mol<ref name=zum>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7}}</ref>
	| ExternalMSDS =
			| Entropy = 112 J/mol·K<ref name=zum />
	| EUIndex = 056-003-00-2
			| DeltaGf = -1139 kJ/mol<ref name=chemister>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=377|title=Barium carbonate|access-date=2014-05-06|archive-date=2014-05-06|archive-url=https://web.archive.org/web/20140506103011/http://chemister.ru/Database/properties-en.php?dbid=1&id=377|url-status=dead}}</ref>
	| EUClass = Harmful ('''Xn''')
			| HeatCapacity = 85.35 J/mol·K<ref name=chemister />
	| NFPA-H = 2
			}}
	| NFPA-F = 0
	| NFPA-R = 0		| Section5 =
	| NFPA-O =		| Section6 =
	| RPhrases = {{R22}}		| Section7 = {{Chembox Hazards
			| ExternalSDS =
	| SPhrases = {{S2}}, {{S24/25}}
			| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=202711|name=Barium carbonate|accessdate=2014-05-06}}</ref>
	| FlashPt = Non-flammable
			| GHSSignalWord = Warning
	| LD50 = 418 mg/kg, oral (rat)
			| HPhrases = {{H-phrases|302}}<ref name="sigma" />
			| NFPA_ref= <ref></ref>
			| NFPA-H = 2
			| NFPA-F = 0
			| NFPA-R = 0
			| NFPA-S =
			| FlashPt = Non-flammable
			| LD50 = 418 mg/kg, oral (rat)
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions =		| OtherAnions =
	| OtherCations = ]<br/>]<br/>]		| OtherCations = ]<br/>]<br/>]<br/>]<br/>]
	| OtherCpds =		| OtherCompounds =
	}}		}}
	}}		}}
			'''Barium carbonate''' is the ] with the formula BaCO<sub>3</sub>. Like most ] ]s, it is a white salt that is poorly soluble in water. It occurs as the mineral known as ]. In a commercial sense, it is one of the most important ] compounds.<ref name=Ull>{{Ullmann |doi=10.1002/14356007.a03_325.pub2|title=Barium and Barium Compounds|year=2007|last1=Kresse|first1=Robert|last2=Baudis|first2=Ulrich|last3=Jäger|first3=Paul|last4=Riechers|first4=H. Hermann|last5=Wagner|first5=Heinz|last6=Winkler|first6=Jochen|last7=Wolf|first7=Hans Uwe|isbn=978-3527306732}}</ref>
	'''Barium carbonate''' (]]<sub>3</sub>), also known as '''witherite''', is a ] compound used in ], ]s, ceramic glazes and ].
	Witherite crystallizes in the orthorhombic system. The ]s are invariably twinned together in groups of three, giving rise to pseudo-hexagonal forms somewhat resembling bipyramidal crystals of ], the faces are usually rough and striated horizontally.
	]
	The mineral is named after ], who in 1784 recognized it to be chemically distinct from ]s. It occurs in veins of ] ] at ] in ], ] in ], ], near ] in ] and a few other localities. Witherite is readily altered to barium ] by the action of water containing ] in solution and crystals are therefore frequently encrusted with ]s. It is the chief source of barium ]s and is mined in considerable amounts in Northumberland. It is used for the preparation of rat poison, in the manufacture of ] and ], and formerly for refining ]. It is also used for controlling the ] to ] ratio in ] ] baths.<ref>{{cite web
	| last = Whitelaw
	| first = G.P.
	| coauthors =
	| title = Standard Chrome Bath Control
	| work =
	| pages =
	| publisher = finishing.com
	| date = 2003-10-25
	| url = http://www.finishing.com/Library/Whitelawchrome.html
	| accessdate = 2006-11-29 }}</ref>
	==Preparation==		==Preparation==
	Barium carbonate is made commercially from ] either by treatment with ] at 60 to 70 °C (] method) or by passing ] at 40 to 90 °C.		Barium carbonate is made commercially from ] by treatment with ] at 60 to 70&nbsp;°C (] method) or, more commonly ] at 40 to 90&nbsp;°C:
	In the soda ash process, solid or dissolved sodium carbonate is added to barium sulfide solution, and the barium carbonate precipitate is filtered, washed and dried.<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref>		In the soda ash process, an aqueous solution of barium sulfide is treated with sodium carbonate:<ref name=Ull/>
			:{{chem2 | BaS + H2O + CO2 -> BaCO3 + H2S }}
	==Reactions==		==Reactions==
	Barium carbonate reacts with acids such as ] to soluble barium salts, such as ]:		Barium carbonate reacts with acids such as ] to form soluble barium salts, such as ]:
			:{{chem2 | BaCO3 + 2 HCl -> BaCl2 + CO2 + H2O }}
			Pyrolysis of barium carbonate gives ].<ref name=Brauer>{{cite book|author=P. Ehrlich|chapter=Barium Oxide|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=1|pages=933–944}}</ref>
	:{{chem|BaCO|3}} (s) + 2 HCl (aq) → {{chem|BaCl|2}} (aq) + {{chem|CO|2}} (g) + {{chem|H|2|O}} (l)
	However, the reaction with ] is poor, because ] is highly ].
	==Uses==		==Uses==
			It is mainly used to remove sulfate impurities from feedstock of the ]. Otherwise it is a common precursor to barium-containing compounds such as ferrites.<ref name=Ull/>
	Barium carbonate is widely used in the ceramics industry as an ingredient in glazes. It acts as a flux, a matting and crystallizing agent and combines with certain coloring oxides to produce unique colors not easily attainable by other means. Its use is somewhat controversial since some claim that it can leach from glazes into food and drink. To provide a safe means of use, BaO is often used in ]ted form.
			===Other uses===
			Barium carbonate is widely used in the ceramics industry as an ingredient in glazes. It acts as a flux, a matting and crystallizing agent and combines with certain colouring oxides to produce unique colours not easily attainable by other means. Its use is somewhat controversial since it can leach from glazes into food and drink. To reduce toxicity concerns, it is often substituted with ], which behaves in a similar way in glazes but is of lower toxicity.
	In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (] and ]) that cause ].		In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (] and ]) that cause ].
			It is sometimes used as an "energiser" in the ] process.
	==References==		==References==
			{{reflist}}
	<references />
			==External links==
	* {{1911}}
			{{Cite web|url=http://www.ijcea.org/show-32-387-1.html|title=Preparation and Characterization of Barium Carbonate Nanoparticles - Volume 2 Number 4 (Aug. 2011) - IJCEA|website=www.ijcea.org|access-date=2017-12-13}}
			{{Commons category|Barium carbonate}}
			{{Clear}}
			{{carbonates}}
	{{Barium compounds}}		{{Barium compounds}}
	{{Rodenticides}}		{{Rodenticides}}
			{{Authority control}}
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