Barium chlorate

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Barium chlorate
Other names

Chloric acid barium salt

Identifiers
CAS number 13477-00-4 YesY
PubChem 26059
ChemSpider 24273 YesY
RTECS number FN9770000
Jmol-3D images {{#if:[Ba+2].[O-]Cl(=O)=O.[O-]Cl(=O)=O|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 413.9 °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
0
3
3
OX
 YesY (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references
Barium chlorate

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. It does not have a long list of uses and is not a very common compound compared to other Barium compounds and other chlorate compounds.

Barium chlorate in its powder form

MSDS (Material Safety Data Sheet) for Barium Chlorate

Acute Health effects: skin and eye irritation upon contact, lung and mucus membrane irritation upon inhalation, Flammability: none Proper storage: store at room temperature and protect from oxygen during storage Toxicity: EPA classified toxic chemical. At this time, there are no known long term effects caused by exposure to the compound. Protective clothing and eye wear are always needed when working with this substance.[1]

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.[2]
The green seen in this firework is produced by barium chlorate and barium nitrate

Decomposition

When exposed to heat, barium chlorate alone will decompose in this reaction:

  • Ba(ClO3)2→BaCl2+3O2

Barium chlorate also participated in double replacement reactions with multiple other compounds in order to decompose and produce energy:

  • Ba(ClO3)2 + H2SO4 → BaSO4 + HClO3
  • 3Ba(ClO3)2(aq) + 2 Na3PO4(aq) ---> Ba3(PO4)2 (s) + 6 NaClO3(aq)

For additional information, refer to the activity series link

Commercial Uses

Fireworks
Barium Chlorate, when burned with a fuel, produces a vibrant green light. This makes it the optimum chemical to use in firework. Because it is an oxidizer, is a chlorine donor when reacted, and contains a metal, allow this compound to produce a green color that is unparalleled. Due to the instability of all chlorates to sulfur, acids, and ammonium ions; chlorates have been banned from use in class C fireworks in the United States. Therefore, more and more firework producers have begun to use most stable compound such as barium nitrate and copper carbonate.[3]

Environmental Hazard

Barium chlorate is toxic to humans if ingested through any body cavity. This compound can also harm the environment. It is very harmful to aquatic organisms if it is leached into bodies of water. Chemical spills of this compound, although not common, can harm entire ecosystems and should be prevented.[4] It is nesseccary to dispose of this compound as hazardous waste. The Environmental Protection Agency (EPA) lists barium chlorate as hazardous.[5]

Nicknames

  • Chloric acid
  • Ba Chlorate
  • Barium salt

History of the components (Ba and ClO3)

  • Barium

Barium was discovered by a Swedish chemist named Carl Wilhelm Scheele in 1774 in the form of BaO. For a short time it was called "Bologna Stones" because of its prevalence in Bologna and because of how dense it is.[6]

  • Chlorate

Research into the explosive abilities of chlorates dates back to 1788. There were many research facilities opened up in Europe to work with these compound but now a lot of evidence remain from them because most of them blew up. Due to this problem, chlorates have not been used in explosives for a long time. They are much too unstable.[7]

Products containing Barium Chlorate

  • Fireworks
  • Matches
  • Some rat poisons
  • Some cigarettes

References

  1. ↑ Dugan, Mark. "Barium Chlorate." Material Safety Data Sheet. Hummel Croton Inc., 24 Apr. 2007. Web. 28 Jan. 2013.
  2. ↑ Perigrin, Tom. "Barium Chlorate". GeoCities. Archived from the original on 2007-10-30. Retrieved 2007-02-22. 
  3. ↑ Wilson, Elizabeth. "C&EN: SCIENCE & TECHNOLOGY - WHAT'S THAT STUFF? FIREWORKS." WHAT'S THAT STUFF? FIREWORKS. Chemical and Engineering News, 2 July 2001. Web. 28 Jan. 2013.
  4. ↑ http://www.inchem.org/documents/icsc/icsc/eics0613.htm
  5. ↑ http://nj.gov/health/eoh/rtkweb/documents/fs/0183.pdf
  6. ↑ http://www.britannica.com/EBchecked/topic/53345/barium-Ba/?anchor=ref168256
  7. ↑ http://www.britannica.com/EBchecked/topic/198577/explosive/82371/Other-explosives?anchor=ref624959

External links

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