Ammonium hydrosulfide
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| Names | |||
|---|---|---|---|
| IUPAC name
ammonium hydrosulfide
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| Other names
ammonium bisulfide
ammonium hydrogen sulfide | |||
| Identifiers | |||
| ECHA InfoCard | 100.031.974 | ||
| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | |||
| H5NS | |||
| Molar mass | 51.111 g/mol | ||
| Appearance | Yellow-orange fuming liquid. | ||
| Density | 1.17 g/cm3[1] | ||
| Infinitely soluble | |||
| Solubility | soluble in alcohol, liquid ammonia, liquid hydrogen sulfide; insoluble in benzene, hexane and ether | ||
Refractive index (nD)
|
1.74 | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
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Toxic | ||
| NFPA 704 (fire diamond) | |||
| Related compounds | |||
Other anions
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Ammonium sulfate | ||
Other cations
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Sodium hydrosulfide | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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 NH3 + H2S
Both ammonia and hydrogen sulfide have a powerfully unpleasant smell.
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
- ^ Goodman, J. T.; Rauchfuss, T. B., (2002). "Tetraethylammonium-tetrathioperrhenate [Et4N][ReS4]". Inorganic Syntheses. 33: 107–110.
{{cite journal}}: CS1 maint: extra punctuation (link) CS1 maint: multiple names: authors list (link) - ^ W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277.