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Sodium sulfide nonahydrate

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Sodium sulfide nonahydrate Basic information
Sodium sulfide nonahydrate Chemical Properties
  • Melting point:50 °C
  • Boiling point:920°C
  • Density 1.427
  • storage temp. 2-8°C
  • form Solid
  • color colorless or slightly yellow
  • Specific Gravity1.427
  • Water Solubility 180 G/L (25 ºC)
  • Sensitive Hygroscopic
  • Merck 14,8681
  • Stability:Stable. Hygroscopic. Light-sensitive. Flammable. Avoid exposure to air, acids, oxidizers, strong bases, strong reducing agents, most common metals.
  • InChIKeyGDQBTRYKLOBMLL-UHFFFAOYSA-N
  • CAS DataBase Reference1313-84-4(CAS DataBase Reference)
  • EPA Substance Registry SystemSodium sulfide (Na2S), nonahydrate(1313-84-4)
Safety Information
  • Hazard Codes C,N,T
  • Risk Statements 31-34-50-24-22
  • Safety Statements 26-45-61-36/37/39
  • RIDADR UN 1849 8/PG 2
  • WGK Germany 2
  • RTECS WE1925000
  • 13
  • TSCA Yes
  • HazardClass 8
  • PackingGroup II
  • HS Code 28301010
MSDS
  • Language:EnglishProvider:ACROS
  • Language:EnglishProvider:ALFA
Sodium sulfide nonahydrate Usage And Synthesis
  • Physical PropertiesThe 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.
  • UsesSodium 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.
  • PreparationSodium 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
  • ReactionsSodium 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.
  • Chemical Propertiescolourless, white or yellow crystals with an odour of rotten eggs
  • Usessodium sulphide nonahydrate has the following uses:sulfur dyestuff; leather depilatory;rayon denitration;dyeing auxiliary;sodium sulphide;including crystallization water; sodium sulphide or sulfureT;dyeing auxiliary.
  • Purification MethodsSome purification of the hydrated salt can be achieved by selecting large crystals and removing the surface layer (contaminated with oxidation products) by washing with distilled water. Other metal ions can be removed from Na2S solutions by passage through a column of Dowex ion-exchange A-1 resin, Na+-form. The hydrated salt can be rendered anhydrous by heating it in a stream of H2 or N2 until water is no longer evolved. (The resulting cake should not be heated to fusion because it is readily oxidised.) Recrystallise it from distilled water [Anderson & Azowlay J Chem Soc, Dalton Trans 469 1986]. Note that sodium sulfide hydrolyses in H2O to form NaHS + H2O, and is therefore alkaline. A 0.1N solution in H2O is 86% hydrolysed at room temperature. Its solubility in H2O is 8% at 0o, 12% at 20o and 30% at 50o. The anhydrous salt is obtained by allowing it to stand in a vacuum over conc H2SO4 or P2O5 at 45o to start with, then at 30-35o when the salt contains 4% of water. The last traces of water are removed by heating to 700o in a glass or porcelain tube in a stream of H2 to give pure H2S. [Fehér in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 358-360 1963.]
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