Barium carbonate

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:

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Reactions

Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:

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Pyrolysis of barium carbonate gives barium oxide.

Uses

Barium carbonate 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

References

1. Zumdahl, Steven S.. (2009). "Chemical Principles 6th Ed.". Houghton Mifflin Company.
2. "Barium carbonate".
3. {{Sigma-Aldrich
4. (29 March 2025). "Fisher SDS - Barium Carbonate". Fisher Scientific.
5. (2007). "Barium and Barium Compounds".
6. P. Ehrlich. (1963). "Handbook of Preparative Inorganic Chemistry, 2nd Ed.". Academic Press.
7. "Barium carbonate".