| 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 acids, 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 a reducing agent.
Sodium borohydride reacts with water to release 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. It can also be found on eBay and Amazon.
- B(OCH3)3 + 4 NaH → NaBH4 + 3 NaOCH3
- Make hydrogen
- Reduce organic compounds (reducing agent)
- 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 of 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
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