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Lithium bromide
Lithium-bromide-3D-ionic.png
IUPAC name
Identifiers
CAS number 7550-35-8 Yes check.svgY
PubChem 82050
EC number 231-439-8
RTECS number OJ5755000
Properties
Molecular formula LiBr
Molar mass 86.845(3) g/mol
Appearance White solid
Density 3.464 g/cm3
Melting point

552 °C

Boiling point

1265 °C

Solubility in water 145 g/100 mL (4 °C)
254 g/100 mL (90 °C)
Solubility soluble in methanol, ethanol, ether
slightly soluble in pyridine
Refractive index (nD) 1.784
Thermochemistry
Std enthalpy of
formation
ΔfHo298
-4.044 kJ/g
Hazards
EU Index Not listed
NFPA 704
NFPA 704.svg
2
2
0
 
Flash point 29 °C
Related compounds
Other anions Lithium fluoride
Lithium chloride
Lithium iodide
Other cations Sodium bromide
Potassium bromide
Rubidium bromide
Caesium bromide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Lithium bromide, or LiBr, is a chemical compound of lithium and bromine. Its extreme hygroscopic character makes LiBr useful as a desiccant in certain air conditioning systems.[1]

Contents

Production and properties

LiBr is prepared by treatment of lithium carbonate with hydrobromic acid. The salt forms several crystalline hydrates, unlike the other alkali metal bromides.[2] The anhydrous salt forms cubic crystals similar to common salt

Uses

Lithium bromide is used in air-conditioning systems as desiccant. Otherwise the salt is useful as a reagent in organic synthesis. For example it reversibly forms adducts with some pharmaceuticals.[1]

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Medical applications

Lithium bromide was used as a sedative beginning in the early 1900s, but it fell into disfavor in the 1940s when some heart patients died after using it as a salt substitute.[3] Like lithium carbonate and lithium chloride it was used as treatment for bipolar disorder.

Hazards

Lithium salts are psychoactive and somewhat corrosive. Dosages for lithium carbonate are ca. 200 mg/day.

References

  1. ^ a b Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim.
  2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  3. ^ Bipolar disorder

External links


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