Ammonium sulfide

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Ammonium sulfide
CAS number 12135-76-1 YesY
PubChem 25519
ChemSpider 23808 YesY
UN number 2683 (solution)
RTECS number BS4900000
Jmol-3D images Image 1
Molecular formula (NH4)2S
Molar mass 68.154 g/mol
Appearance yellow crystals (> −18 °C)[1]
Density 0.997 g/cm3
Melting point decomposes at ambient temperatures
Solubility in water 128.1 g/100 mL
Solubility soluble in alcohol
very soluble in liquid ammonia
MSDS External MSDS
EU Index 016-008-00-2
EU classification Corrosive (C)
Dangerous for the environment (N)
R-phrases R31, R34, R50
S-phrases (S1/2), S26, S45, S61
NFPA 704
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g., gasoline) Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point 32.22 °C (90.00 °F; 305.37 K)
Related compounds
Other anions Ammonium hydroxide
Other cations Sodium sulfide
Potassium sulfide
Related compounds Ammonium hydrosulfide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Ammonium sulfide, also known as diammonium sulfide, is an unstable salt with the formula (NH4)2S. Aqueous solutions purporting to contain this salt are commercially available. With a pKa exceeding 15,[2] the hydrosulfide ion cannot be deprotonated to an appreciable amount by ammonia. Thus, such solutions mainly 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 foul pranks including the common stink bomb.


Solutions of "ammonium sulfide" are hazardous as liable sources of toxic hydrogen sulfide.[3]


  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ 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
  3. ^ J. T. Baker: MSDS for Ammonium Sulfide