Sodium borohydride
Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate, is an inorganic compound with the formula NaBH4 (sometimes written as Na[BH4]). It is a white crystalline solid, usually encountered as an aqueous basic solution. Sodium borohydride is a reducing agent that finds application in papermaking and dye industries. It is also used as a reagent in organic synthesis.
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| Names | |||
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| IUPAC name
Sodium tetrahydridoborate(1–) | |||
| Systematic IUPAC name
Sodium boranuide | |||
| Identifiers | |||
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3D model (JSmol) |
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| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.037.262 | ||
| EC Number |
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| 23167 | |||
| MeSH | Sodium+borohydride | ||
PubChem CID |
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| RTECS number |
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| UNII | |||
| UN number | 1426 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| Na[BH4] | |||
| Molar mass | 37.83 g·mol−1 | ||
| Appearance | white crystals hygroscopic | ||
| Density | 1.07 g/cm3 | ||
| Melting point | 400 °C (752 °F; 673 K)(decomposes) | ||
| 550 g/L | |||
| Solubility | soluble in liquid ammonia, amines, pyridine | ||
| Structure | |||
| Cubic (NaCl), cF8 | |||
| Fm3m, No. 225 | |||
a = 0.6157 nm | |||
| Thermochemistry | |||
Heat capacity (C) |
86.8 J·mol−1·K−1 | ||
Std molar entropy (S⦵298) |
101.3 J·mol−1·K−1 | ||
Std enthalpy of formation (ΔfH⦵298) |
−188.6 kJ·mol−1 | ||
Gibbs free energy (ΔfG⦵) |
−123.9 kJ·mol−1 | ||
| Hazards | |||
| GHS labelling: | |||
| Danger | |||
| H260, H301, H314, H360F | |||
| P201, P231+P232, P280, P308+P313, P370+P378, P402+P404 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | 70 °C (158 °F; 343 K) | ||
| ca. 220 °C (428 °F; 493 K) | |||
| Explosive limits | 3% | ||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose) |
160 mg/kg (Oral – Rat) 230 mg/kg (Dermal – Rabbit) | ||
| Related compounds | |||
Other anions |
Sodium cyanoborohydride Sodium hydride Sodium borate Borax Sodium aluminum hydride | ||
Other cations |
Lithium borohydride | ||
Related compounds |
Lithium aluminium hydride Sodium triacetoxyborohydride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references | |||
The compound was discovered in the 1940s by H. I. Schlesinger, who led a team seeking volatile uranium compounds. Results of this wartime research were declassified and published in 1953.
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