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DOI: 10.1055/s-0031-1289560
Sodium Sulfide
Publikationsverlauf
Publikationsdatum:
25. Oktober 2011 (online)
Introduction
Sodium sulfide is pink to yellowish solid with a rotten egg-like odor. It is readily soluble in water, slightly soluble in alcohol and insoluble in ether. Anhydrous sodium sulfide can ignite spontaneously when exposed to air. [¹] It is used in chemical manufacturing as a sulfonation and sulfomethylation agent. It is used in the production of rubber chemicals, sulfur dyes, and other chemical compounds. It has also been used as a reducer for the reduction of nitro compounds to the corresponding amines. [²] It was found to be useful for the conversion of carboxylic acids into thioacids [³] and alkenoyl ketene dithioacetals into the corresponding [5+1]-annulation products [4] as well as for the synthesis of thiofuranose, [5] cyclic dithiocarbonates, [6] tetrahydrothiophene derivatives, [7] 4-bromo-2-nitrobenzenethiol, [8] a-lipoic acid, [9] thieno[2,3-c]pyrazoles, [¹0] unsaturated thiacrown ethers, [¹¹] thieno[3,2-c]cinnoline, [¹²] monomeric cyclic diketosulfides, [¹³] thiophenes, [¹4] 2H-thiopyran compounds, [¹5] 4H-thiochromen-4-ones [¹6] and benzo[b]thiophenes. [¹7] It can also act as an atom-economical inorganic nucleophile in transition-metal-catalyzed allylation substitutions. [¹8] Willgerodt-Kindler reaction between anilines and benzaldehydes has also been achieved by the use of Na2S˙9H2O as a base catalyst. [¹9]
Sodium sulfide is commercially available and it can be readily prepared by reduction of Na2SO4 with carbon or through a solid-gas reaction of a sulfidizing gas mixture of COS, CS2, and S2 with the reactant of Na2CO3. [²0]
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