| Barium chlorate | |
|---|---|
| Other names | Chloric acid barium salt |
| Identifiers | |
| CAS number | 13477-00-4 |
| Properties | |
| Molecular formula | Ba(ClO3)2 |
| Molar mass | 304.23 g/mol |
| Appearance | white solid |
| Density | 3.18 g/cm3, solid |
| Melting point |
414 °C |
| Solubility in water | 27.5 g/ml (20 °C) |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
| Infobox references | |
Barium chlorate is a white crystalline solid. It is an irritant, and if consumed can cause nausea, vomiting, and diarrhoea. It is used in pyrotechnics to produce a green colour.
Synthesis
Barium chlorate can be produced through a double replacement reaction of barium chloride and sodium chlorate.
- 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[1].
References
- ^ Perigrin, Tom. "Barium Chlorate". Geocities. http://www.geocities.com/CapeCanaveral/Campus/5361/chlorate/barium.html. Retrieved 2007-02-22.
External links
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