| IUPAC name
| Other names
Lithium boron hydride
|Molar mass||21.784 g/mol|
|Appearance||White or grayish solid|
|Density||0.666 g/cm3 (20 °C)|
|Melting point||268 °C (514 °F; 541 K)|
|Boiling point||380 °C (716 °F; 653 K) (decomposes)|
|Solubility|| Reacts with alcohols, carboxylic acids, aldehydes, halocarbons, ketones|
Soluble in ethers
Insoluble in cyclohexane, heptane, hexane, pentane, toluene, xylene
|Solubility in 1,4-Dioxane||0.3 g/100 ml (18 °C)|
|Solubility in diethyl ether|| 1.32 g/100 ml (0 °C)|
3.04973 g/100 ml (25 °C)
6.62228 g/100 ml (34 °C)
|Solubility in dimethoxyethane|| 4.13892 g/100 ml (0 °C)|
4.5746 g/100 ml (75 °C)
|Solubility in dimethyl ether||1.6 g/100 ml (-45.2 °C)|
|Solubility in tetrahydrofuran||24.8989 g/100 ml (25 °C)|
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|87.8 mg/kg (mouse, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Lithium borohydride (LiBH4) is a chemical compound widely used in organic synthesis as a reducing agent, often for esters.
Lithium borohydride reacts with water to release hydrogen gas.
- LiBH4 + 4 H2O → LiOH + B(OH)3 + 4 H2
Lithium borohydride is a white solid, which reacts with water and alcohols, but it's soluble in ethers.
Lithium borohydride has the highest energy density of all known chemical energy carriers, with a value of 65.2 MJ/kg or 43.4 MJ/l, higher than gasoline.
It is sold by chemical suppliers.
- NaBH4 + LiBr → NaBr + LiBH4
- BF3 + 4 LiH → LiBH4 + 3 LiF
- Reducing agent
- Fuel cells
Lithium borohydride reacts with water and moisture, and may ignite in open air.
Lithium borohydride should be kept in closed bottles, under inert gas.
Can be safely neutralized by adding it slowly in a large volume of alcohol or water.
- Peter Rittmeyer, Ulrich Wietelmann “Hydrides” in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim.
- Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. Newyork: Academic Press. p. 775