Sodium borohydride
Chemical compound / From Wikipedia, the free encyclopedia
Dear Wikiwand AI, let's keep it short by simply answering these key questions:
Can you list the top facts and stats about Sodium borohydride?
Summarize this article for a 10 year old
SHOW ALL QUESTIONS
Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate,[5] 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.[6]
Quick Facts Names, Identifiers ...
| |||
Names | |||
---|---|---|---|
IUPAC name
Sodium tetrahydridoborate(1–) | |||
Systematic IUPAC name
Sodium boranuide | |||
Identifiers | |||
| |||
3D model (JSmol) |
|||
ChEBI | |||
ChemSpider | |||
ECHA InfoCard | 100.037.262 | ||
EC Number |
| ||
23167 | |||
MeSH | Sodium+borohydride | ||
PubChem CID |
|||
RTECS number |
| ||
UNII | |||
UN number | 1426 | ||
CompTox Dashboard (EPA) |
|||
| |||
| |||
Properties | |||
Na[BH4] | |||
Molar mass | 37.83 g·mol−1 | ||
Appearance | white crystals hygroscopic | ||
Density | 1.07 g/cm3[1] | ||
Melting point | 400 °C (752 °F; 673 K)(decomposes)[1] | ||
550 g/L[1] | |||
Solubility | soluble in liquid ammonia, amines, pyridine | ||
Structure[2] | |||
Cubic (NaCl), cF8 | |||
Fm3m, No. 225 | |||
a = 0.6157 nm | |||
Thermochemistry[3] | |||
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:[4] | |||
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).
|
Close
The compound was discovered in the 1940s by H. I. Schlesinger, who led a team seeking volatile uranium compounds.[7][8] Results of this wartime research were declassified and published in 1953.