Sodium Borohydride CAS 16940-66-2

Sodium Borohydride CAS 16940-66-2 BH4Na

Sodium Borohydride CAS 16940-66-2 BH4Na, hot in Canada/USA/Europe, stock available.

BH4Na Basic Parameter

CAS 16940-66-2 Picture

What is 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.

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.

Structure

NaBH₄ is a salt, consisting of the tetrahedral [BH₄]⁻ anion. The solid is known to exist as three polymorphs: α, β and γ. The stable phase at room temperature and pressure is α–NaBH₄, which is cubic and adopts an NaCl-type structure, in the Fm3m space group. At a pressure of 6.3 GPa, the structure changes to the tetragonal β–NaBH₄ (space group P42₁c) and at 8.9 GPa, the orthorhombic γ–NaBH₄ (space group Pnma) becomes the most stable.

• •               
                _{α-NaBH4                                                   β-NaBH4                                                           γ-NaBH4}

Synthesis and handling

For commercial NaBH₄ production, the Brown-Schlesinger process and the Bayer process are the most popular methods. In the Brown-Schlesinger process sodium borohydride is industrially prepared from sodium hydride (produced by reacting Na and H₂) and trimethyl borate at 250–270 °C:

B(OCH₃)₃ + 4 NaH → NaBH₄ + 3 NaOCH₃

Millions of kilograms are produced annually, far exceeding the production levels of any other hydride reducing agent. In the Bayer process, it is produced from inorganic borates, including borosilicate glass and borax (Na₂B₄O₇):

Na₂B₄O₇ + 16 Na + 8 H₂ + 7 SiO₂ → 4 NaBH₄ + 7 Na₂SiO₃

Magnesium is a less expensive reductant, and could in principle be used instead:

8 MgH₂ + Na₂B₄O₇ + Na₂CO₃ → 4 NaBH₄ + 8 MgO + CO₂

and

2 MgH₂ + NaBO₂ → NaBH₄ + 2 MgO

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