Barium carbonate
{{Short description|Chemical compound}}
{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 443182359
| Name = Barium carbonate
| ImageFile = Barium carbonate.png
| ImageSize = 150px
| ImageName = Skeletal formula of barium carbonate
| ImageFile1 = Uhličitan barnatý.JPG
| ImageFile2 = Barium-carbonate-3D-vdW.png
| ImageName1 = Powder of barium carbonate
| OtherNames = Witherite
| IUPACName =
| SystematicName =
| Section1 = {{Chembox Identifiers
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 6P669D8HQ8
| InChI = 1/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
| SMILES = [Ba+2].[O-]C([O-])=O
| InChIKey = AYJRCSIUFZENHW-NUQVWONBAT
| SMILES1 = C(=O)([O-])[O-].[Ba+2]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = AYJRCSIUFZENHW-UHFFFAOYSA-L
| CASNo = 513-77-9
| CASNo_Ref = {{cascite|correct|CAS}}
| EINECS = 208-167-3
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID=10121
| ChEBI = 190439
| UNNumber = 1564
| RTECS = CQ8600000
| PubChem = 10563
}}
| Section2 = {{Chembox Properties
| Formula = BaCO3
| Appearance = white crystals
| Odor = odorless
| Density = 4.286 g/cm3
| MolarMass = 197.34 g/mol
| Solubility = 16 mg/L (8.8°C)
22 mg/L (18 °C)
24 mg/L (20 °C)
24 mg/L (24.2 °C)
| SolubleOther = decomposes in acid
insoluble in methanol
| MeltingPtC = 811
| MeltingPt_notes =
polymorphic transformation
| BoilingPtC = 1450
| BoilingPt_notes =
decomposes from 1360 °C
| RefractIndex = 1.676
| SolubilityProduct = 2.58·10−9
| MagSus = −58.9·10−6 cm3/mol
}}
| Section3 = {{Chembox Structure
| Coordination =
| CrystalStruct = orthorhombic
}}
| Section4 = {{Chembox Thermochemistry
| DeltaHf = −1219 kJ/mol{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7}}
| HeatCapacity = 85.35 J/mol·K
}}
| Section5 =
| Section6 =
| Section7 = {{Chembox Hazards
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0777.htm ICSC 0777]
| GHSPictograms = {{GHS07}}{{Sigma-Aldrich|id=202711|name=Barium carbonate|accessdate=2014-05-06}}
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|302}}
| NFPA_ref= [http://www.sciencelab.com/msds.php?msdsId=9927090 Sciences labs MSDS]
| NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S =
| FlashPt = Non-flammable
| LD50 = 418 mg/kg, oral (rat)
}}
| Section8 = {{Chembox Related
| OtherAnions =
| OtherCations = Beryllium carbonate
Magnesium carbonate
Calcium carbonate
Strontium carbonate
Radium carbonate
| OtherCompounds =
}}
}}
Barium carbonate is the inorganic compound with the formula BaCO3. Like most alkaline earth metal carbonates, it is a white salt that is poorly soluble in water. It occurs as the mineral known as witherite. In a commercial sense, it is one of the most important barium compounds.{{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}}
Preparation
Barium carbonate is made commercially from barium sulfide by treatment with sodium carbonate at 60 to 70 °C (soda ash method) or, more commonly carbon dioxide at 40 to 90 °C:
In the soda ash process, an aqueous solution of barium sulfide is treated with sodium carbonate:
:{{chem2 | BaS + H2O + CO2 -> BaCO3 + H2S }}
Reactions
Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:
:{{chem2 | BaCO3 + 2 HCl -> BaCl2 + CO2 + H2O }}
Pyrolysis of barium carbonate gives barium oxide.{{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}}
Uses
It is mainly used to remove sulfate impurities from feedstock of the chlor-alkali process. Otherwise it is a common precursor to barium-containing compounds such as ferrites.
=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 strontium carbonate, 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 (calcium sulfate and magnesium sulfate) that cause efflorescence.
It is sometimes used as an "energiser" in the Case-hardening process.
References
{{reflist}}
External links
{{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}}
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