Lithium bromide
| Lithium bromide | |
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Lithium bromide |
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| Identifiers | |
| CAS number | 7550-35-8  |
| PubChem | 82050 |
| ChemSpider | 74049 |
| UNII | 864G646I84 |
| EC number | 231-439-8 |
| RTECS number | OJ5755000 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | LiBr |
| Molar mass | 86.845(3) g/mol |
| Appearance | White solid hygroscopic |
| Density | 3.464 g/cm3 |
| Melting point |
552 °C |
| Boiling point |
1265 °C |
| Solubility in water | 145 g/100 mL (4 °C) 166.7 g/100 mL (20 °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 ΔfH |
-4.044 kJ/g |
| Hazards | |
| EU Index | Not listed |
| NFPA 704 |
 0
2
0
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| Flash point | not flammable |
| Related compounds | |
| Other anions | Lithium fluoride Lithium chloride Lithium iodide |
| Other cations | Sodium bromide Potassium bromide Rubidium bromide Caesium bromide |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| 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]
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[edit] 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.
Lithium Hydroxide and Hydrobromic Acid (Aqueous solution of Hydrogen Bromide) will precipitate Lithium Bromide in the presence of water.
LiOH + HBr → LiBr + H2O
[edit] 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]
[edit] 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.
Doses as low as 225 mg/day of LiBr can lead to Bromism.
[edit] Hazards
Lithium salts are psychoactive and somewhat corrosive. When lithium bromide is dissolved into water, the reaction is very exothermic.
[edit] References
- ^ a b Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Bipolar disorder
[edit] External links
- "A PDF file from GFS Chemicals, a supplier of lithium bromide". http://www.gfschemicals.com/Search/MSDS/5035MSDS.PDF. Retrieved 2005-09-15.
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