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• Physical Properties

  The nonahydrate is a yellowish-white crystalline solid; tetragonal crystals; odor of hydrogen sulfide; the color changes on exposure to light and air, first turning to yellow and then becoming brownish-black, deliquescent; density 1.43 g/cm3; decomposes at about 50°C; very soluble in water; aqueous solution strongly alkaline; slightly soluble in alcohol; insoluble in ether. ;

• Uses

  Sodium sulfide is used in making sulfur dyes; for dehairing of hides; removing sulfur from viscous rayon; engraving and lithography; cotton printing; manufacturing rubber; paper pulp; and as a photographic reagent. Other major applications are for treating paper and for extracting gold ores where oxidized metal ores are converted to sulfides prior to froth flotation. Sodium sulfide also is used in preparing many other sulfides and as an analytical reagent. ;

• Preparation

  Sodium sulfide is prepared by heating sodium bisulfate with sodium chloride and coal above 950°C. The product mixture is extracted with water and the hydrated sulfide is obtained from the solution by crystallization:
  NaHSO4 + NaCl + 2C → Na2S + 2CO2↑ + HCl↑
  Sodium sulfide also is produced from its elements in liquid ammonia:
  Na + 2S → Na2S ;

• Reactions

  Sodium sulfide in solid form reacts with carbon dioxide in the presence of moisture to form hydrogen sulfide and sodium carbonate. Thus, the H2S odor of sodium sulfide crystals is attributed to its exposure to moist air:
  Na2S + H2O + CO2 → Na2CO3 + H2S
  In aqueous solution, sodium sulfide reacts with a number of metal salts forming insoluble sulfides.
  When added to dilute mineral acids, hydrogen sulfide is generated. ;

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