|CAS number||, (dihydrate)|
|Jmol-3D images||Image 1|
|Molar mass||102.894 g/mol|
|Density||3.21 g/cm3 (anhydrous)
2.18 g/cm3 (dihydrate)
747 °C (anhydrous)
|Solubility in water||90.5 g/100 mL (20 °C) 121.0 g/100 mL (100 °C)|
|Solubility in methanol||16.7 g/100 mL|
|Refractive index (nD)||1.6459|
|Std enthalpy of
|EU Index||Not listed|
|Flash point||800 °C (1,470 °F)|
|Other anions||Sodium fluoride
|Other cations||Lithium bromide
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Sodium bromide is an inorganic compound with the formula NaBr. It is a high-melting white, crystalline solid that resembles sodium chloride. It is a widely used source of the bromide ion and has many applications.
Synthesis, structure, reactions
It is produced by treating sodium hydroxide with hydrogen bromide.
- 2 NaBr + Cl2 → Br2 + 2 NaCl
Sodium bromide is the most useful inorganic bromide in industry.
Also known as Sedoneural, sodium bromide has been used as a hypnotic, anticonvulsant, and sedative in medicine, widely used as an anticonvulsant and a sedative in the late 19th and early 20th centuries. Its action is due to the bromide ion, and for this reason potassium bromide is equally effective.
Preparation of other bromine compounds
Sodium bromide is widely used for the preparation of other bromides in organic synthesis and other areas. It is a source of the bromide nucleophile to convert alkyl chlorides to more reactive alkyl bromides by the Finkelstein reaction:
- NaBr + RCl → RBr + NaCl (R = alkyl)
Once a large need in photography, but now shrinking, the photosensitive salt silver bromide is prepared using NaBr.
NaBr is used in conjunction with chlorine as a disinfectant for swimming pools.
Sodium bromide is used to prepare dense fluids used in oil wells.
NaBr has a very low toxicity with an oral LD50 estimated at 3.5 g/kg for rats. However, this is a single-dose value. Bromide ion is a cumulative toxin with a relatively long half life (in excess of a week in humans): see potassium bromide.
- Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 0-618-94690-X.
- Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders "Bromine Compounds" in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2000. doi:10.1002/14356007.a04_405
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