- Barium chlorate
Barium chlorate Identifiers CAS number PubChem ChemSpider Jmol-3D images Image 1 Properties Molecular formula Ba(ClO3)2 Molar mass 304.23 g/mol Appearance white solid Density 3.18 g/cm3, solid Melting point
Solubility in water 27.5 g/100 ml (20 °C) Hazards EU classification Oxidant (O)
R-phrases , S-phrases , NFPA 704 (what is: /?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Barium chlorate is a white crystalline solid. It is an irritant, as are all barium compounds. If consumed, barium chlorate can cause nausea, vomiting, and diarrhea. It is used in pyrotechnics to produce a green color. A powerful oxidizing agent, the compound is used to manufacture explosives and matches.
- BaCl2 + 2 NaClO3 → Ba(ClO3)2 + 2 NaCl
It can also be produced through a more complicated non-electrolytic process.
- BaCl2 + Na2CO3 → BaCO3 + 2 NaCl or BaCl2 + 2 NaHCO3 → BaCO3 + 2 NaCl + H2O + CO2 — In this step barium carbonate is produced, which will be used later.
- C4H6O6 + NH4OH → NH4C4H5O6 + H2O — in this step ammonium bitartrate is produced.
- NH4C4H5O6 + KClO3 → KC4H5O6 + NH4ClO3 — in this step, the ammonium bitartrate is added to potassium chlorate, which produces potassium bitartrate, but more importantly, ammonium chlorate.
- 2 NH4ClO3 + BaCO3 + Q → Ba(ClO3)2 + 2 NH3 + H2O + CO2 — in this step, the ammonium chlorate is added to the barium carbonate and boiled, to produce barium chlorate.
- ^ Perigrin, Tom. "Barium Chlorate". Geocities. Archived from the original on 2007-10-30. http://web.archive.org/web/20071030002126/http://www.geocities.com/CapeCanaveral/Campus/5361/chlorate/barium.html. Retrieved 2007-02-22.
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