Sodium bromide

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Sodium bromide
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Template:Longitem NaBr
Molar mass Template:Chem molar mass
Appearance White powder, hygroscopic
Density 3.21 g/cm3 (anhydrous)
2.18 g/cm3 (dihydrate)
Melting point Template:Chembox CalcTemperatures
Boiling point Template:Chembox CalcTemperatures
Solubility Soluble in alcohol, liquid ammonia, pyridine, hydrazine, [[sulfur dioxide|Template:Chem2]]
Insoluble in acetone, acetonitrile[1]
Solubility in methanol 17.3 g/100 g (0 °C)
16.8 g/100 g (20 °C)
16.1 g/100 g (40 °C)
15.3 g/100 g (60 °C)[1]
Solubility in ethanol 2.45 g/100 g (0 °C)
2.32 g/100 g (20 °C)
2.29 g/100 g (30 °C)
2.35 g/100 g (70 °C)[1]
Solubility in formic acid 19.3 g/100 g (18 °C)
19.4 g/100 g (25 °C)[1]
Solubility in glycerol 38.7 g/100 g (20 °C)[1]
Solubility in dimethylformamide 3.2 g/100 g (10.3 °C)[1]
Vapor pressure 1 torr (806 °C)
5 torr (903 °C)[3]
Template:Longitem −41.0·10−6 cm3/mol
Thermal conductivity 5.6 W/(m·K) (150 K)[4]
Template:Longitem 1.6428 (24 °C)
nKrF = 1.8467 (24 °C)
nHe–Ne = 1.6389 (24 °C)[5]
Viscosity 1.42 cP (762 °C)
1.08 cP (857 °C)
0.96 cP (937 °C)[1]
Template:Longitem Cubic
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a = 5.97 Å[4]
Template:Longitem 51.4 J/(mol·K)[1]
Template:Longitem 86.82 J/(mol·K)[1]
Template:Longitem −361.41 kJ/mol[1]
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Sodium bromide is an inorganic compound with the formula Template:Chem2. 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.[6]

In repeated doses it is toxic to humans, leading to bromism, which may include symptoms such as skin rashes, drowsiness, nausea, and hallucinations.[7]

Synthesis, structure, reactions

NaBr crystallizes in the same cubic motif as NaCl, NaF and NaI. The anhydrous salt crystallizes above 50.7 °C.[6] Dihydrate salt (Template:Chem2) crystallize out of water solution below 50.7 °C.[8]

NaBr is produced by treating sodium hydroxide with hydrogen bromide.

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:

Template:Chem2

Applications

Sodium bromide is the most useful inorganic bromide in industry.[6] It is also used as a catalyst in TEMPO-mediated oxidation reactions.[9]

Medicine

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File:Bromo seltzer newspaper.png
Bromo-Seltzer newspaper ad (1908)

Also known as Sedoneural,[10] 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. In 1975, bromides were removed from drugs in the U.S. such as Bromo-Seltzer due to toxicity.[11]

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

Sodium bromide is used in conjunction with chlorine as a disinfectant for hot tubs and swimming pools.[12]

Petroleum industry

Because of its high solubility in water (943.2 g/L or 9.16 mol/L, at 25 °C) sodium bromide is used to prepare dense drilling fluids used in oil wells to compensate a possible overpressure arising in the fluid column and to counteract the associated trend to blow out. The presence of the sodium cation also causes the bentonite added to the drilling fluid to swell, while the high ionic strength induces bentonite flocculation.[13]

Safety

NaBr has a very low toxicity with an oral LD50 estimated at 3.5 g/kg for rats.[14] However, this is a single-dose value. Bromide ions are a cumulative toxin with a relatively long biological half-life (in excess of a week in humans): see potassium bromide.

Human consumption can lead to bromism.[15]

References

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  1. ↑ a b c d e f g h i j k l Script error: No such module "citation/CS1".
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  6. ↑ 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. Script error: No such module "CS1 identifiers".
  7. ↑ National Center for Biotechnology Information (2025). PubChem Compound Summary for CID 253877, Potassium Bromide. Retrieved November 18, 2025 from https://pubchem.ncbi.nlm.nih.gov/compound/Potassium-Bromide.
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External links

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