Barium chlorate

In this article, we will explore in depth the topic of Barium chlorate and its implications in today's society. From its origins to its impact today, we will analyze the different aspects related to Barium chlorate and its relevance in different areas. Through careful research and analysis, we will seek to better understand the role Barium chlorate plays in our lives and how it influences the way we think, act, and relate to the world around us. Additionally, we will closely examine expert opinions and current trends regarding Barium chlorate, in order to provide a comprehensive and up-to-date view on this highly relevant topic.

Barium chlorate
Names
IUPAC name
Barium dichlorate
Other names
Chloric acid, barium salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.404 Edit this at Wikidata
EC Number
  • 236-760-7
RTECS number
  • FN9770000
UNII
UN number 1445
  • InChI=1S/Ba.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 checkY
    Key: ISFLYIRWQDJPDR-UHFFFAOYSA-L checkY
  • InChI=1/Ba.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2
    Key: ISFLYIRWQDJPDR-NUQVWONBAT
  • .Cl(=O)=O.Cl(=O)=O
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:
GHS03: OxidizingGHS07: Exclamation markGHS09: Environmental hazard
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)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
3
OX
Lethal dose or concentration (LD, LC):
500.1 mg/kg
(4h) 1.5 mg/l - dust/mist
NIOSH (US health exposure limits):
PEL (Permissible)
 0.5 mg/m3 (Vacated)
IDLH (Immediate danger)
 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 , 100 kPa).
checkY verify (what is checkY☒N ?)

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 colour. It also finds use in the production of chloric acid.

Reactions

Synthesis

Barium 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

After concentrating and cooling 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 colour 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.

The green seen in this firework is produced by barium chlorate and barium nitrate

Decomposition

When exposed to heat, barium chlorate alone will decompose to barium chloride and oxygen:

Ba(ClO3)2 → BaCl2 + 3 O2

Chloric acid

Barium chlorate is sometimes used to produce chloric acid.[3]: 312–313 

Commercial uses

When barium chlorate is heated with a fuel, it burns to produce a vibrant green light, which is also a flame test for the presence of bariom ions. Because it is an oxidizer, a chlorine donor, and contains a metal ion, this compound produces a distinctive green colour.[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 compounds such as barium nitrate and barium carbonate.[4]

Environmental Hazard

Barium chlorate, like all oxidizing agents, is dangerous to human health and is also classed as toxic to 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 pollute 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

  1. ^ Sigma-Aldrich Co., Barium chlorate. Retrieved on 6 December 2024.
  2. ^ Perigrin, Tom. "Barium Chlorate". GeoCities. Archived from the original on 30 October 2007. Retrieved 22 February 2007.
  3. ^ 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. {{cite book}}: ISBN / Date incompatibility (help)
  4. ^ Wilson, Elizabeth (2 July 2001). "What's That Stuff? Fireworks". Chemical & Engineering News. 79 (27): 30.
  5. ^ "Barium Chlorate". inchem.org.
  6. ^ "Barium Chlorate" (PDF). Hazardous Substance Fact Sheet. New Jersey Department of Health and Human Services.