Ammonium hydrosulfide


Ammonium hydrosulfide
Ammonium-2D.svg
Hydrogen sulfide ion.svg
IUPAC name
ammonium hydrosulfide
other names
ammonium bisulfide
ammonium hydrogen sulfide
Identifiers
CAS number 12124-99-1
RTECS number BS4900000
Properties
Molecular formula H5NS
Molar mass 51.111 g/mol
Appearance Yellow-orange fuming liquid.
Density 1.17 g/cm3[1]
Solubility in water Infinitely soluble
Solubility soluble in alcohol, liquid ammonia, liquid hydrogen sulfide; insoluble in benzene, hexane and ether
Refractive index (nD) 1.74
Hazards
R-phrases R11, R23, R24, R25.
NFPA 704
NFPA 704.svg
3
3
0
Related compounds
Other anions Ammonium sulfate
Other cations Sodium hydrosulfide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Ammonium hydrosulfide is the chemical compound with the formula (NH4)SH. It is the salt derived from the ammonium cation and the hydrosulfide anion. The salt exists as colourless, water soluble, micaceous crystals. The compound is encountered mainly as a solution, not as the solid. It is generated by mixing hydrogen sulfide and ammonia.

Preparation

Solutions of ammonium hydrosulfide can be prepared by passing hydrogen sulfide gas through concentrated ammonia solution.[2] According to a detailed 1895 report, hydrogen sulfide reacts with concentrated aqueous ammonia solution at room temperature to give (NH4)2S·2NH4HS. When this species is cooled to 0 °C and treated with additional hydrogen sulfide, one obtains (NH4)2S·12NH4HS.[3] An ice-cold solution of this substance kept at 0°C and having hydrogen sulfide continually passed through it gives the hydrosulfide.

The common "stink bomb" consists of an aqueous solution of ammonium sulfide. The mixture easily converts to ammonia and hydrogen sulfide gases. This conversion illustrates the ease of the following equilibrium:

(NH4)SH\overrightarrow{\leftarrow} NH3 + H2S

Both ammonia and hydrogen sulfide have a powerfully unpleasant smell.

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ Goodman, J. T.; Rauchfuss, T. B., (2002). "Tetraethylammonium-tetrathioperrhenate [Et4N][ReS4]". Inorganic Syntheses 33: 107–110. 
  3. ^ W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277. 






stock | retire | vm
Why are we here?
All text is available under the terms of the GNU Free Documentation License
This page is cache of Wikipedia. History