Barium chloride



Barium chloride
Identifiers
CAS number 10361-37-2
Properties
Molecular formula Cl2 (anhydrous)

BaCl2·2H2O

Molar mass 208.2324 g/mol
Appearance White solid
Density 3.856 g/cm3, solid
Melting point

962 °C

Boiling point

1560 °C

Solubility in water 37.5 g/100 ml (26°C)
Structure
Crystal structure orthorhombic
Coordination
geometry
7-9
Thermochemistry
Std enthalpy of
formation
ΔfHo298
−858.56 kJ/mol
Hazards
MSDS External MSDS
EU classification Toxic (T)
R-phrases R20, R25
S-phrases S45
Flash point Non-flammable
Related Compounds
Other anions Barium bromide
Barium iodide
Other cations Lead chloride
Supplementary data page
Structure and
properties
εr, etc.
Thermodynamic
data
Phase behaviour
Solid, liquid, gas
Spectral data MS
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

hygroscopic.

Structure and properties

BaCl2 crystallizes in both the pH.

Barium chloride reacts with barium sulfate.

BaCl2(aq) + SO42- → BaSO4(Cl-(aq)

Oxalate effects a similar reaction:

BaCl2(aq) + Na2C2O4(aq) → BaC2O4 (s) + 2 NaCl(aq)

Preparation

Although inexpensively available, barium chloride can be prepared from barium sulfate)[4]:

BaSO4 + 4 CO

This first step requires high temperatures.

BaS + CaCl2 → BaCl2 + CaS

The second step reqiures fusion of the reactants. The BaCl2 can then be leached out from the mixture with water.

Uses

As a cheap, soluble salt of steel, in the manufacture of pigments, and in the manufacture of other barium salts. BaCl2 is also used in fireworks to give a bright green color. However, its toxicity limits its applicability.

Safety

Barium chloride, along with other water-soluble barium salts, is toxic. Sodium sulfate is a potential antidote because it forms the insoluble solid BaSO4.

References

  1. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  1. Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford: Butterworth-Heinemann. ISBN 0-7506-3365-4.
  2. Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
  3. The Merck Index, 7th edition, Merck & Co., Rahway, New Jersey, 1960.
  4. H. Nechamkin, The Chemistry of the Element, McGraw-Hill, New York, 1968.
 
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