Lithium bromide

Lithium bromide

Lithium bromide
IUPAC name
Lithium bromide
ChemSpider  Y
EC number 231-439-8
Jmol-3D images Image
RTECS number OJ5755000
Molar mass 86.845(3) g/mol
Appearance White solid
Density 3.464 g/cm3
Melting point 552 °C (1,026 °F; 825 K)
Boiling point 1,265 °C (2,309 °F; 1,538 K)
143 g/100 mL (0 °C)
166.7 g/100 mL (20 °C)
266 g/100 mL (100 °C)
Solubility soluble in methanol, ethanol, ether, acetone
slightly soluble in pyridine
51.88 J/mol K
66.9 J/mol K
-350.3 kJ/mol
-338.9 kJ/mol
-157 kJ/mol
NFPA 704
Flash point Not-flammable
Lethal dose or concentration (LD, LC):
LD50 (Median dose)
1800 mg/kg (oral, rat)[1]
Related compounds
Other anions
Lithium fluoride
Lithium chloride
Lithium iodide
Other cations
Sodium bromide
Potassium bromide
Rubidium bromide
Caesium bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 Y  (: Y/N?)

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.[2]


  • Production and properties 1
  • Uses 2
    • Medical applications 2.1
  • Hazards 3
  • References 4
  • External links 5

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.[3] The anhydrous salt forms cubic crystals similar to common salt (sodium chloride).

Lithium hydroxide and hydrobromic acid (aqueous solution of hydrogen bromide) will precipitate lithium bromide in the presence of water.

LiOH + HBr → LiBr + H2O


Lithium bromide is used in air-conditioning systems as desiccant.
Lithium bromide is used as a salt in absorption chilling along with water (see adducts with some pharmaceuticals.[2]

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.[4]
Like lithium carbonate and lithium chloride, it was used as treatment for bipolar disorder.

Doses as low as 225 mg/day of LiBr can lead to bromism.


Lithium salts are psychoactive and somewhat corrosive. Heat is quickly generated when lithium bromide is dissolved into water because it has a negative enthalpy of solution.


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

External links

  • "A PDF file from GFS Chemicals, a supplier of lithium bromide" (PDF). Retrieved 2005-09-15.