Barium carbonate

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Template:Chembox E numberTemplate:Chembox SolubilityInWater
Barium carbonate
Other names witherite
Identifiers
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Properties
BaCO3
Molar mass 197.336 g/mol
Appearance white crystals
Density 4.2865 g/cm3, solid
Melting point
Boiling point
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Barium carbonate (BaCO3), also known as witherite, is a chemical compound used in rat poison, bricks and cement.

Witherite crystallizes in the orthorhombic system. The crystals are invariably twinned together in groups of three, giving rise to pseudo-hexagonal forms somewhat resembling bipyramidal crystals of quartz, the faces are usually rough and striated horizontally.

The mineral is named after William Withering, who in 1784 recognized it to be chemically distinct from barytes. It occurs in veins of lead ore at Hexham in Northumberland, Alston in Cumbria, Anglezarke, near Chorley in Lancashire and a few other localities. Witherite is readily altered to barium sulfate by the action of water containing calcium sulfate in solution and crystals are therefore frequently encrusted with barytes. It is the chief source of barium salts and is mined in considerable amounts in Northumberland. It is used for the preparation of rat poison, in the manufacture of glass and porcelain, and formerly for refining sugar. It is also used for controlling the chromate to sulfate ratio in chromium electroplating baths.[1]

Reactions

Barium carbonate reacts with many acids to soluble barium salts, for example barium chloride:

BaCO3(s) + 2 HCl(aq) → BaCl2(aq) + CO2(g) + H2O(l)

However the reaction with sulfuric acid is poor, because barium sulfate is highly insoluble.

References

  1. Whitelaw, G.P. (2003-10-25). "Standard Chrome Bath Control". finishing.com. Retrieved 2006-11-29. Check date values in: |date= (help)

bs:Barijum karbonat de:Bariumcarbonat lv:Bārija karbonāts nl:Bariumcarbonaat


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