ammonium hydrogen sulfide
3D model (JSmol)
|Molar mass||51.111 g/mol|
|Appearance||Yellow-orange fuming liquid.|
|Boiling point||56.6 °C (133.9 °F; 329.8 K)|
|Solubility||soluble in alcohol, liquid ammonia, liquid hydrogen sulfide; insoluble in benzene, hexane and ether|
Refractive index (nD)
|GHS signal word||Danger|
|P260, P264, P273, P280, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P321, P363, P391, P405, P501|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|168 mg/kg (rat, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
It is the salt derived from the ammonium cation and the hydrosulfide anion. The salt exists as colourless, water-soluble, micaceous crystals. On Earth the compound is encountered mainly as a solution, not as the solid, but NH4SH ice is believed to be a substantial component of the cloud decks of the gas-giant planets Jupiter and Saturn, with sulfur produced by its photolysis responsible for the color of some of those planets' clouds. It can be generated by mixing hydrogen sulfide and ammonia.
Solutions of ammonium hydrosulfide can be prepared by passing hydrogen sulfide gas through concentrated ammonia solution. 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. 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 powerful and unpleasant smell.
Ammonium sulfide (CAS registry number 12135-76-1), also known as diammonium sulfide, is an hypothetical salt with the formula (NH4)2S. Aqueous solutions purporting to contain this salt are commercially available. With a pKa exceeding 15, the hydrosulfide ion cannot be deprotonated by ammonia. Thus, solutions of "ammonium sulfide" consist of a mixture of ammonia and NH4)SH. Ammonium sulfide solutions are used occasionally in photographic developing, to apply patina to bronze, and in textile manufacturing. Also, due to its offensive smell, it is the active ingredient in a variety of pranks including the common stink bomb. It can be used as a selective reducing agent (cf Clonitazene), where there are two nitro groups only one of them is selectively reduced.
- Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- Record of ammonium hydrosulfide in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on October 22, 2010.
- Goodman, J. T.; Rauchfuss, T. B. (2002). "Tetraethylammonium-tetrathioperrhenate [Et4N][ReS4]". Inorganic Syntheses. 33: 107–110. doi:10.1002/0471224502.ch2.
- W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277.
- Meyer B, Ward K, Koshlap K, Peter L "Second dissociation constant of hydrogen sulfide" Inorganic Chemistry', (1983). volume 22, pp. 2345.doi:10.1021/ic00158a027