Sodium sulfide

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Sodium sulfide
Other names Disodium sulfide
Identifiers
CAS number anhydrous: [1313-82-2]
nonahydrate: [1313-84-4]
Properties
Molecular formula anhydrous: Na2S,
nonahydrate: Na2S • 9H2O
Molar mass anhydrous: 78.046 g/mol,
nonahydrate: 240.182 g/mol
Appearance colorless, hygroscopic solid
Melting point

950 °C (anhydrous)
Solubility in water readily soluble
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Sodium sulfide is the name used to refer to the chemical compound Na2S but more commonly its hydrate Na2S.9H2O. Both are a colorless water-soluble salts that give strongly alkaline solutions. When exposed to moist air, Na2S and its hydrates emit hydrogen sulfide, which smells much like rotten eggs.

Contents

[edit] Structure

Na2S adopts the "antifluorite" structure, which means that the Na+ centers occupy sites of the fluoride in the CaF2 framework, and the larger S2- occupy the sites for Ca2+. In solution, the salt, by definition, dissociates. The dianion S2- does not, however, exist in appreciable amounts in water. Sulfide is too strong of a base to coexist with water. Thus, the dissolution process can be described as follows:

Na2S + H2O → Na+,SH- + Na+,OH-

[edit] Production

Industrially Na2S is produced by reduction of Na2SO4 with carbon, in the form of coal:[1]

Na2SO4 + 4 C → Na2S + 4 CO

In the laboratory, the anhydrous salt can be prepared by reduction of sulfur with sodium in anhydrous ammonia. Alternatively, sulfur can be reduced by sodium in dry THF with a catalytic amount of naphthalene:[2]

2 Na + S → Na2S

[edit] Safety

Na2S and its hydrates are dangerous and should only be handled by experts. Like lye, it is strongly alkaline and will cause skin burns. Acids react rapidly to produce hydrogen sulfide, which is a highly toxic gas.

[edit] References

  1. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  2. ^ J.-H. So and P. Boudjouk (1992). "Hexamethyldisilathiane". Inorganic Syntheses. doi:10.1002/9780470132609.ch11. 

[edit] External links

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