Barium chlorate
Barium chlorate
Identifiers
CAS number 13477-00-4
PubChem 26059
ChemSpider 24273 YesY
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

414 °C

Solubility in water 27.5 g/100 ml (20 °C)
Hazards
EU classification Oxidant (O)
Harmful (Xn)
R-phrases R9, R20/22
S-phrases S13, S27
NFPA 704
NFPA 704.svg
0
3
3
OX
 YesY chlorate (verify) (what is: YesY/N?)
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, 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.

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.

  1. 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.
  2. C4H6O6 + NH4OH → NH4C4H5O6 + H2O — in this step ammonium bitartrate is produced.
  3. NH4C4H5O6 + KClO3 → KC4H5O6 + NH4ClO3 — in this step, the ammonium bitartrate is added to potassium chlorate, which produces potassium bitartrate, but more importantly, ammonium chlorate.
  4. 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

  1. ^ 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. 

External links



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