| IUPAC name
| Other names
|Molar mass||37.83 g/mol|
|Appearance||White or grayish solid|
|Melting point||400 °C (752 °F; 673 K)|
|Boiling point||500 °C (932 °F; 773 K) (decomposes)|
| 25 g/100 ml|
|Solubility|| Reacts with alcohols, aldehydes, carboxylic acids, halocarbons, ketones|
Soluble in liquid ammonia, amines, isopropylamine, methylamine, pyridine
Slightly soluble in DMSO, ethanol, THF, toluene
Insoluble in diethyl ether, hexane, pentane
|Solubility in acetonitrile||2 g/100 ml (28 °C)|
|Solubility in ammonia||104 g/100 ml (-33.3 °C)|
|Solubility in diethyl ether||0.02 g/100 ml|
|Solubility in diglyme|| 5.15 g/100 ml|
24 g/100 ml (25 °C)
|Solubility in dimethoxyethane||0.567488 g/100 ml (25 °C)|
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Flash point||70 °C (158 °F; 343 K)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
| 160 mg/kg (rat, oral)|
230 mg/kg (rabbit, dermal)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate, is an inorganic compound with the chemical formula NaBH4. It is widely used as reducing agent.
Sodium borohydride reacts with water to give hydrogen, though the reaction is very slow.
Sodium borohydride is a white solid, which reacts with water and alcohols, though the reaction is fairly slow. Complete decomposition in excess methanol can take nearly 90 min at 20 °C. It will decompose in neutral or acidic aqueous solutions but is stable at pH 14. It has good solubility in amines and poor solubility in ethers.
Sodium borohydride is sold by chemical suppliers.
- B(OCH3)3 + 4 NaH → NaBH4 + 3 NaOCH3
- Make hydrogen
- Reduce organic compounds
- Fuel cells
Sodium borohydride reacts with water to release hydrogen and may be pyrophoric if finely divided. Sodium borohydride itself is very flammable and burns with a bright yellow flame, leaving behind a residue or sodium and boron oxides.
Sodium borohydride should air-tight containers, away from moisture and air. While it can be stored in most bottles, it will not tolerate prolonged exposure to moisture, so it's best to use an air-tight cap or seal the bottle with parafilm, if you intend on using the borohydride for a long period of time.
Can be neutralized safely by adding it in a large volume of water, aq. acids or alcohol. Controlled incineration is also an option.
- Hurd, D. T.; Journal of the American Chemical Society; vol. 71; (1949); p. 20 - 22
- Gaylord, N. G.; Journal of the American Chemical Society; vol. 75; (1953); p. 186 - 190
- Kasper, J. S.; McCarty, L. V.; Newkirk, A. E.; Journal of the American Chemical Society; vol. 71; (1949); p. 2583
- Noeth,H.; Beyer,H.; Chemische Berichte; vol. 93; (1960); p. 928 - 938
- Schlesinger, H. I.; Brown, H. C.; Hoekstra, H. R.; Rapp, L. R.; Journal of the American Chemical Society; vol. 75; (1953); p. 199 - 204
Relevant Sciencemadness threads
- Sodium Borohydride
- Sodium Borohydride
- Sodium Borohydride Synthesis
- Borohydride synth?
- NaBH4 ester reduction to alcohol ?'s
- Using Sodium borohydride in aqueous media with PTC - stability in water?
- Potassium to Sodium Borohydride
- otc sodium borohyride
- Sodium hydride and borohydride
- Sodium borohydride for sale
- Sodium borohydride in Canada
- Sodium Borohydride from chinese supplier
- Source of Sodium Borohydride
- sodium borohydride to sodium triacetoxyborohydride
- In Search of NaBH4