Lithium bromide

Lithium bromide

Names
IUPAC name Lithium bromide
Identifiers
CAS Number	7550-35-8 Y
ChemSpider	74049 Y
EC Number	231-439-8
Jmol 3D model	Interactive image
PubChem	82050
RTECS number	OJ5755000
UNII	864G646I84 Y
InChI InChI=1S/BrH.Li/h1H;/q;+1/p-1 Y Key: AMXOYNBUYSYVKV-UHFFFAOYSA-M Y InChI=1/BrH.Li/h1H;/q;+1/p-1 Key: AMXOYNBUYSYVKV-REWHXWOFAS
SMILES [Li+].[Br-]
Properties
Chemical formula	LiBr
Molar mass	86.845(3) g/mol
Appearance	White solid hygroscopic
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)
Solubility in water	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
Refractive index (nD)	1.784
Thermochemistry
Specific heat capacity (C)	51.88 J/mol K
Std molar entropy (So298)	66.9 J/mol K
Std enthalpy of formation (ΔfHo298)	-350.3 kJ/mol
Gibbs free energy (ΔfG˚)	-338.9 kJ/mol
Std enthalpy of combustion (ΔcHo298)	-157 kJ/mol
Vapor pressure	{{{value}}}
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 verify (what is YN ?)
Infobox references

Lithium bromide (LiBr) is a chemical compound of lithium and bromine. Its extreme hygroscopic character makes LiBr useful as a desiccant in certain air conditioning systems.

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. 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

Uses

Lithium bromide is used in air-conditioning systems as desiccant.
Lithium bromide is used as a salt in absorption chilling along with water (see absorption refrigerator). Otherwise the salt is useful as a reagent in organic synthesis. For example it reversibly forms adducts with some pharmaceuticals.

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.
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.

Hazards

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.