is sodium borohydride flammable

is sodium borohydride flammable

xref It is decomposed by water to form sodium hydroxide, a corrosive material, and hydrogen, a flammable gas. Lower Explosive Limit (LEL): data unavailable, Upper Explosive Limit (UEL): data unavailable, Autoignition Temperature: data unavailable, Vapor Density (Relative to Air): data unavailable, Metal Hydrides, Metal Alkyls, Metal Aryls, and Silanes. [17] NaBH4 reacts with water and alcohols, with evolution of hydrogen gas and formation of the corresponding borate, the reaction being especially fast at low pH. Search for more papers by this author. 29 0 obj<> endobj The material itself is easily ignited and burns vigorously once ignited. Hydrolysis generates enough heat to ignite adjacent combustible material [Haz. It is decomposed by water to form sodium hydroxide, a corrosive material, and hydrogen, a flammable gas. Schubert, F.; Lang, K.; Burger, A. Spontaneous ignition can result from solution of sodium borohydride in dimethylformamide. [22], The reactivity of NaBH4 can be enhanced or augmented by a variety of compounds. Università, di Genova, Italy. 1:1 ratio at >100 °C with or without H pressure". It was suggested that the simultaneous activation of the carbonyl compound and borohydride occurs, via interaction with the alcohol and alkoxide ion, respectively, and that the reaction proceeds through an open transition state. Nikola Stiasni. Sodium borohydride: … �Ҩ��6�j����w�b�I-�%�. German patent DE 1088930 19600915 (ChemAbs: 55:120851). Purification: crystallize from diglyme 3 or isopropylamine. [10] It decomposes in neutral or acidic aqueous solutions, but is stable at pH 14. It efficiently reduces acyl chlorides, anhydrides, α-hydroxylactones, thioesters, and imines at room temperature or below. 0000002586 00000 n In the presence of metal catalysts, sodium borohydride releases hydrogen. P210, P260, P264, P273, P280, P284: NFPA 704 (fire diamond) 3. CAS No. Although practical temperatures and pressures for hydrogen storage have not been achieved, in 2012 a core–shell nanostructure of sodium borohydride was used successfully to store, release and reabsorb hydrogen under moderate conditions. The heat of this reaction may be sufficient to ignite the hydrogen. Calcium oxide or sodium hydroxide react with phosphorus pentaoxide extremely violently when initiated by local heating [Mellor 8 Supp.3:406 (1971]. [19] Hydrogen-bonding activation is required, as no reduction occurs in an aprotic solvent like diglyme. 0000000016 00000 n Gov. Exploiting this reactivity, sodium borohydride is used in prototypes of the direct borohydride fuel cell. Brown, H. C. “Organic Syntheses via Boranes” John Wiley & Sons, Inc. New York: 1975. The material itself is easily ignited and burns vigorously once ignited. including trade names and synonyms. 0000001626 00000 n Variations in the counterion also affect the reactivity of the borohydride. Handling, Storage, and Precautions: harmful if inhaled or absorbed through skin. There is a newer version of this article Luca Banfi. (USCG, 1999). 0000002115 00000 n Threshold limit value (TLV) 5 mg/m3 (TWA) Related compounds Other anions. 2. These can perform a variety of reductions not normally associated with borohydride chemistry, such as alcohols to hydrocarbons and nitriles to primary amines. trailer NaBH4 reduces many organic carbonyls, depending on the precise conditions. Sodium borohydride reduces aldehydes and ketones to give the related alcohols. The compound was discovered in the 1940s by H. I. Schlesinger, who led a team seeking volatile uranium compounds. The hydrogen is generated for a fuel cell by catalytic decomposition of the aqueous borohydride solution: The principal application of sodium borohydride is the production of sodium dithionite from sulfur dioxide: Sodium dithionite is used as a bleaching agent for wood pulp and in the dyeing industry. 0000003946 00000 n This is an outdated version. * Sodium Borohydridereacts with WATER or MOIST AIR to produce flammable and explosive Hydrogen gas. %PDF-1.5 %���� [9] Sodium borohydride is soluble in protic solvents such as water and lower alcohols. [7][8] Results of this wartime research were declassified and published in 1953. Various steroids and vitamin A are prepared using sodium borohydride in at least one step. Natriumborhydrid Sodium borohydride for analysis. <<6fe2a16dfa5a514881011077fe625937>]>> Sodium borohydride is a white to grayish crystalline powder. Sodium borohydride is a source of basic borate salts which can be corrosive, and hydrogen or diborane, which are both flammable. This reaction is used in the production of various antibiotics including chloramphenicol, dihydrostreptomycin, and thiophenicol. 0 It also reacts with these protic solvents to produce H2; however, these reactions are fairly slow. These usually involve replacing hydride with alkyl groups, such as lithium triethylborohydride and L-selectride (lithium tri-sec-butylborohydride), or replacing B with Al. It is used to make other chemicals, treat waste water, and for many other uses. 0000008653 00000 n The heat of this reaction may be sufficient to ignite the hydrogen.

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