Sodium bromide

Sodium bromide
IUPAC name Sodium bromide
Identifiers
CAS number	7647-15-6 Y,  13466-08-5 (dihydrate)
PubChem	253881
ChemSpider	22712 Y
UNII	LC1V549NOM Y
ChEMBL	CHEMBL1644694 N
RTECS number	VZ3150000
Jmol-3D images	Image 1
SMILES [Na+].[Br-]
InChI InChI=1S/BrH.Na/h1H;/q;+1/p-1 Y Key: JHJLBTNAGRQEKS-UHFFFAOYSA-M Y InChI=1/BrH.Na/h1H;/q;+1/p-1 Key: JHJLBTNAGRQEKS-REWHXWOFAR
Properties
Molecular formula	NaBr
Molar mass	102.894 g/mol
Appearance	White powder
Density	3.21 g/cm3 (anhydrous) 2.18 g/cm3 (dihydrate)
Melting point	747 °C (anhydrous) 36 °C (dihydrate)
Boiling point	1396 °C
Solubility in water	90.5 g/100 mL (20 °C) 121.0 g/100 mL (100 °C)
Solubility in methanol	16.7 g/100mL
Refractive index (nD)	1.6459
Hazards
MSDS	External MSDS[dead link]
EU Index	Not listed
Flash point	800 °C
LD50	3500 mg/kg
Related compounds
Other anions	Sodium fluoride Sodium chloride Sodium iodide
Other cations	Lithium bromide Potassium bromide Rubidium bromide Caesium bromide
N (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

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.^[1]

Synthesis, structure, reactions

NaBr crystallizes in the same cubic motif as NaCl, NaF and NaI. It is produced by treating sodium hydroxide with hydrogen bromide. The anhydrous salt crystallizes above 50.7 °C.^[1]

Sodium bromide can be used as a source of the chemical element bromine. This can be accomplished by treating an aqueous solution of NaBr with chlorine gas:

2 NaBr + Cl₂ → Br₂ + 2 NaCl

Applications

Sodium bromide is the most useful inorganic bromide in industry.^[1]

Medicine

Main article: Potassium bromide#Medical and Veterinary

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.^[2]

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.

Disinfectant

NaBr is used in conjunction with chlorine as a disinfectant for swimming pools.

Petroleum industry

Sodium bromide is used to prepare dense fluids used in oil wells.

Safety

NaBr has a very low toxicity with an oral LD₅₀ estimated at 5 g/kg for rats.

References

1. ^ ^{a b c} 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
2. ^ Bromide

External links

• Information about NaBr.
• Bromide Poisoning in Angola