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BARIUM CARBONATE  BaCO3 197.34

CAS

513-77-9

Density G/Cm3

4.43
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Catalog
No

Product Description

Purity
%

Particle
Size

Cost Per Pound

1-2

3-10

11-25

26-100

BA-301

barium carbonate

99+

sub-micron

N/A

8.34

7.77

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HISTORY:
The mineral witherite 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.

BACKGROUND:
Barium carbonate (BaCO3), known as witherite, is a chemical compound. 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. 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.

APPLICATIONS:
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.

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 fritted form.

In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (calcium and magnesium sulfates) that cause efflorescence.

CHEMISTRY:
Barium carbonate is made commercially from barium sulfide either by treatment with sodium carbonate at 60 to 70 °C (soda ash method) or by passing carbon dioxide at 40 to 90 °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.

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.

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