Barium chlorate, Ba(ClO3)2, is the barium salt of chloric acid. It is a white crystalline solid, and like all soluble barium compounds, irritant and toxic. It is sometimes used in pyrotechnics to produce a green color. It also finds use in the production of chloric acid.
Names | |
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IUPAC name
Barium dichlorate
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Other names
Chloric acid, barium salt
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Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.033.404 |
EC Number |
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PubChem CID
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RTECS number |
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UNII | |
UN number | 1445 |
CompTox Dashboard (EPA)
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Properties | |
Ba(ClO3)2 | |
Molar mass | 304.23 g/mol |
Appearance | white solid |
Density | 3.18 g/cm3, solid |
Melting point | 413.9 °C (777.0 °F; 687.0 K) (decomposes) |
27.5 g/100 ml (20 °C) | |
-87.5·10−6 cm3/mol | |
Hazards[1] | |
GHS labelling: | |
Danger | |
H271, H302, H332, H411 | |
P210, P220, P221, P261, P264, P270, P271, P273, P280, P283, P301+P312, P304+P312, P304+P340, P306+P360, P312, P330, P370+P378, P371+P380+P375, P391, P501 | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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500.1 mg/kg |
LC50 (median concentration)
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(4h) 1.5 mg/l - dust/mist |
NIOSH (US health exposure limits): | |
PEL (Permissible)
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0.5 mg/m3 (Vacated) |
IDLH (Immediate danger)
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50 mg/m3 |
Safety data sheet (SDS) | Barium Chlorate MSDS |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Reactions
editSynthesis
editBarium chlorate can be produced through a double replacement reaction between solutions of barium chloride and sodium chlorate:
- BaCl2 + 2 NaClO3 → Ba(ClO3)2 + 2 NaCl
On concentrating and chilling the resulting mixture, barium chlorate precipitates. This is perhaps the most common preparation, exploiting the lower solubility of barium chlorate compared to sodium chlorate.[citation needed]
The above method does result in some sodium contamination, which is undesirable for pyrotechnic purposes, where the strong yellow of sodium can easily overpower the green of barium. Sodium-free barium chlorate can be produced directly through electrolysis:[2][unreliable source?]
- BaCl2 + 6 H2O → Ba(ClO3)2 + 6 H2
It can also be produced by the reaction of barium carbonate with boiling ammonium chlorate solution:[3]
- 2 NH4ClO3 + BaCO3 → Ba(ClO3)2 + 2 NH3 + H2O + CO2
The reaction initially produces barium chlorate and ammonium carbonate; boiling the solution decomposes the ammonium carbonate and drives off the resulting ammonia and carbon dioxide, leaving only barium chlorate in solution.
Decomposition
editWhen exposed to heat, barium chlorate alone will decompose to barium chloride and oxygen:
- Ba(ClO3)2 → BaCl2 + 3 O2
Chloric acid
editBarium chlorate is sometimes used to produce chloric acid.[3]: 312–313
Commercial uses
editBarium chlorate, when burned with a fuel, produces a vibrant green light. Because it is an oxidizer, a chlorine donor, and contains a metal, this compound produces a green color that is unparalleled.[citation needed] However, 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 more stable compound such as barium nitrate and barium carbonate.[4]
Environmental Hazard
editBarium chlorate is toxic to humans and 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.[5] It is necessary to dispose of this compound as hazardous waste. The Environmental Protection Agency (EPA) lists barium chlorate as hazardous.[6]
References
edit- ^ Sigma-Aldrich Co., Barium chlorate. Retrieved on 6 December 2024.
- ^ Perigrin, Tom. "Barium Chlorate". GeoCities. Archived from the original on 2007-10-30. Retrieved 2007-02-22.
- ^ a b Brauer, Georg; Schmeisser, M. (1963). "5. Chlorine, Bromine, Iodine". In Riley, Reed F. (ed.). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York, London: Academic Press. pp. 314–315. ISBN 9780121266011. Retrieved 6 December 2024.
- ^ Wilson, Elizabeth (July 2, 2001). "What's That Stuff? Fireworks". Chemical & Engineering News. 79 (27): 30.
- ^ "Barium Chlorate". inchem.org.
- ^ "Barium Chlorate" (PDF). Hazardous Substance Fact Sheet. New Jersey Department of Health and Human Services.