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In the laboratory, this liquid serves as a source of HCN, which is inconveniently volatile. [4] Thus, acetone cyanohydrin can be used for the preparation of other cyanohydrins, for the transformation of HCN to Michael acceptors, and for the formylation of arenes. Treatment of this cyanohydrin with lithium hydride affords anhydrous lithium cyanide:
It is used as a surrogate in place of HCN, as illustrated by its use as a precursor to lithium cyanide: [8] (CH 3) 2 C(OH)CN + LiH → (CH 3) 2 CO + LiCN + H 2. In transhydrocyanation, an equivalent of HCN is transferred from acetone cyanohydrin to another acceptor, with acetone as byproduct. The transfer is an equilibrium process, initiated by ...
Cyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide: . 2 Hg(CN) 2 → (CN) 2 + Hg 2 (CN) 2 Or, one can combine solutions of copper(II) salts (such as copper(II) sulfate) with cyanides; an unstable copper(II) cyanide is formed which rapidly decomposes into copper(I) cyanide and cyanogen.
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Chloral cyanohydrin is the cyanohydrin derivative of chloral (trichloroacetaldehyde). It was historically used as a source of hydrogen cyanide for medicinal purposes. [1]
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Ethylene oxide easily reacts with hydrogen cyanide forming ethylene cyanohydrin: (CH 2 CH 2)O + HCN → HO–CH 2 CH 2 –CN. A slightly chilled (10–20 °C) aqueous solution of calcium cyanide can be used instead of HCN: [38] 2 (CH 2 CH 2)O + Ca(CN) 2 + 2 H 2 O → 2 HO–CH 2 CH 2 –CN + Ca(OH) 2. Ethylene cyanohydrin easily loses water ...