Barium chlorate
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| Barium oxide | |
|---|---|
| Systematic name | Barium chlorate |
| Other names | Chloric acid |
| General | |
| Molecular formula | Ba(ClO3)2 |
| Molar mass | 304.23 g/mol |
| Appearance | white solid |
| CAS number | [13477-00-4] |
| Properties | |
| Density and phase | 3.18 g/cm3, solid |
| Solubility in water | 27.5 g/ml (20 °C) |
| Melting point | 414 C |
| Boiling point | |
| Structure | |
| Coordination geometry |
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| Crystal structure | |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Barium Chlorate is a white crystaline solid. It is an irritant, and if consumed can cause nausea, vomiting, and diarrhoea. It is used in pyrotechnics to produce a green colour.
[edit] Synthesis
Barium chlorate can be produced through a double displacement 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.
- C2O6H6 + NH4OH → C2O6H5NH4 + H2O — in this step tartaric acid is produced.
- C2O6H5NH4 + KClO3 → C2O6H5K + NH4ClO3 — in this step, the tartaric acid is added to potasium chlorate, which produces potasium 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].
[edit] References
- ^ Perigrin, Tom. Barium Chlorate. Geocities. Retrieved on February 22, 2007.
[edit] External links
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