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{{chembox {{chembox
| Watchedfields = changed | Watchedfields = changed
| verifiedrevid = 399518300 | verifiedrevid = 431911872
| Name = Ammonium hydrosulfide | Name = Ammonium hydrosulfide
| ImageFileL1 = Ammonium-2D.svg | ImageFile =
| ImageFileL1 = Ammonium-2D.svg
| ImageFileR1 = Hydrogen sulfide ion.svg | ImageFileR1 = Hydrogen sulfide ion.svg
| IUPACName = ammonium hydrosulfide | ImageFile2 = Ammonium-hydrosulfide-3D-vdW.png
| OtherNames = ammonium bisulfide<br />ammonium hydrogen sulfide | IUPACName = ammonium hydrosulfide
| OtherNames = ammonium bisulfide<br />ammonium hydrogen sulfide
| SystematicName =
| Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 23805 | ChemSpiderID = 23805
| InChI = 1/H3N.H2S/h1H3;1H2 | InChI = 1/H3N.H2S/h1H3;1H2
Line 17: Line 20:
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = HIVLDXAAFGCOFU-UHFFFAOYSA-N | StdInChIKey = HIVLDXAAFGCOFU-UHFFFAOYSA-N
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 12124-99-1 | CASNo = 12124-99-1
| RTECS = BS4900000
| <!-- Ammonium Sulfide (NH4)2S CAS = has its own article and is actually a different molecule than Ammonium HydroSulfide (NH4)HS -->
| RTECS = BS4900000 | PubChem = 25515
| EC_number = 235-184-3
| UNNumber = 2683
| UNII = A824D6LXMB
}} }}
| Section2 = {{Chembox Properties | Section2 = {{Chembox Properties
| Formula = H<sub>5</sub>NS | Formula = {{chem2|SH}}
| MolarMass = 51.111 g/mol | MolarMass = 51.111 g/mol
| Appearance = Yellow-orange fuming liquid (in solution). White rhombic crystals (anhydrous).<ref name="CRC">{{cite book|year=1990|chapter=Physical Constants of Inorganic Compounds|editor-last=Lide|editor-first=David R.|title=CRC Handbook of Chemistry and Physics|edition=71st|page=4-45|publisher=CRC Press, inc.}}</ref>
| Appearance = Yellow-orange fuming liquid.
| Density = 1.17 g/cm<sup>3</sup><ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref> | Density = 1.17 g/cm<sup>3</sup><ref name="CRC" /><ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref>
| Solubility = Infinitely soluble | Solubility = Miscible
| SolubleOther = soluble in ], liquid ], liquid ]; insoluble in ], ] and ] | SolubleOther = soluble in ], liquid ], liquid ]; insoluble in ], ] and ]
| MeltingPt = | MeltingPt =
| BoilingPt = | BoilingPtC = 56.6
| pKb = | pKb =
| RefractIndex = 1.74 | RefractIndex = 1.74
}} }}
| Section3 =
⚫ | Section7 = {{Chembox Hazards
| Section4 =
| ExternalMSDS =
| Section5 =
⚫ | MainHazards = Toxic
| NFPA-H = 3 | Section6 =
⚫ | Section7 = {{Chembox Hazards
⚫ | NFPA-F = 3
| NFPA-R = | ExternalSDS =
⚫ | MainHazards = Toxic
⚫ | FlashPt =
⚫ | NFPA-H = 3
| RPhrases = {{R11}}, {{R23}}, {{R24}}, {{R25}}.
| SPhrases = | NFPA-F = 3
| NFPA-R =
⚫ | LD50 = 168 mg/kg (rat, oral)<ref name=GESTIS>{{GESTIS | CAS = 12124-99-1 | ZVG = 492163 | Name = ammonium hydrosulfide | Date = October 22, 2010}}</ref>
⚫ | FlashPt =
| GHSPictograms = {{GHS05}}{{GHS09}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|314|400}}.
| PPhrases = {{P-phrases|260|264|273|280|301+330+331|303+361+353|304+340|305+351+338|310|321|363|391|405|501}}
⚫ | LD50 = 168 mg/kg (rat, oral)<ref name=GESTIS>{{GESTIS | CAS = 12124-99-1 | ZVG = 492163 | Name = ammonium hydrosulfide | Date = October 22, 2010}}</ref>
}} }}
| Section8 = {{Chembox Related | Section8 = {{Chembox Related
| OtherAnions = ] | OtherAnions = ]
| OtherCations = ] | OtherCations = ]
}} }}
}} }}


'''Ammonium hydrosulfide''' is the ] with the ] (NH<sub>4</sub>)SH. It is the ] derived from the ] ] and the ] ]. The salt exists as colourless, water soluble, ]ceous crystals. The compound is encountered mainly as a solution, not as the solid. It is generated by mixing ] and ]. '''Ammonium hydrosulfide''' is the ] with the ] {{chem2|SH}}.

==Composition==
It is the ] derived from the ] ] and the ] ]. The salt exists as colourless, water-soluble, ]ceous crystals. On Earth the compound is encountered mainly as a solution, not as the solid, but {{chem2|SH}} ice is believed to be a substantial component of the cloud decks of the gas-giant planets ] and ], with sulfur produced by its ] responsible for the color of some of those planets' clouds. It can be generated by mixing ] and ].


==Preparation== ==Preparation==
Solutions of ammonium hydrosulfide can be prepared by passing ] gas through concentrated ] solution.<ref>{{cite journal | author = Goodman, J. T.; Rauchfuss, T. B., | title = Tetraethylammonium-tetrathioperrhenate | journal = ] | year = 2002 | volume = 33 | pages = 107–110}}</ref> According to a detailed 1895 report, hydrogen sulfide reacts with concentrated aqueous ammonia solution at room temperature to give (NH<sub>4</sub>)<sub>2</sub>S·2NH<sub>4</sub>HS. When this species is cooled to 0 °C and treated with additional hydrogen sulfide, one obtains (NH<sub>4</sub>)<sub>2</sub>S·12NH<sub>4</sub>HS.<ref>{{cite journal | author = W. P. Bloxam | title = The Sulphides and Polysulphides of Ammonium | journal = ] | year = 1895 | volume = 67 | pages = 283 | doi = 10.1039/CT8956700277}}</ref> An ice-cold solution of this substance kept at 0°C and having hydrogen sulfide continually passed through it gives the hydrosulfide. Solutions of ammonium hydrosulfide can be prepared by passing ] gas through concentrated ] solution.<ref>{{cite book |author1=Goodman, J. T. |author2=Rauchfuss, T. B. |chapter=Useful Reagents and Ligands | title = Inorganic Syntheses | series = ] | year = 2002 | volume = 33 | pages = 107–110 | doi=10.1002/0471224502.ch2|isbn=978-0-471-20825-9 }}</ref> According to a detailed 1895 report, hydrogen sulfide reacts with concentrated aqueous ammonia solution at room temperature to give {{chem2|2S*2SH}}. When this species is cooled to 0&nbsp;°C and treated with additional hydrogen sulfide, one obtains {{chem2|2S*12SH}}.<ref>{{cite journal | author = W. P. Bloxam | title = The Sulphides and Polysulphides of Ammonium | journal = ] | year = 1895 | volume = 67 | pages = 283 | doi = 10.1039/CT8956700277| url = https://zenodo.org/record/1603071 }}</ref> An ice-cold solution of this substance kept at 0&nbsp;°C and having hydrogen sulfide continually passed through it gives the hydrosulfide.


The common "]" consists of an aqueous solution of ammonium sulfide. The mixture easily converts to ] and ] gases. This conversion illustrates the ease of the following equilibrium: The common "]" consists of an aqueous solution of ammonium sulfide. The mixture easily converts to ] and ] gases. This conversion illustrates the ease of the following equilibrium:
:{{chem2|SH ⇌ NH3 + H2S}}
: (NH<sub>4</sub>)SH<math>\overrightarrow{\leftarrow}</math> NH<sub>3</sub> + H<sub>2</sub>S
Both ammonia and hydrogen sulfide have a powerfully unpleasant smell. Ammonia and hydrogen sulfide each have a powerful and unpleasant smell.

Solid ammonium hydrosulfide can be produced by reacting an equimolar mixture of ammonia and hydrogen sulfide under -18 °C:<ref name="crys">{{cite journal |author1=C. D. West |title=The Crystal Structures of Some Alkali Hydrosulfides and Monosulfides. |journal=Zeitschrift für Kristallographie - Crystalline Materials |date=1934 |volume=88 |issue=1–6 |pages=97–115 |doi=10.1524/zkri.1934.88.1.97 |s2cid=100849097 |language=en}}</ref>
:NH<sub>3</sub> + H<sub>2</sub>S → NH<sub>4</sub>SH

=="Ammonium sulfide"==

]

Aqueous solutions of '''ammonium sulfide''' (CAS registry number {{CAS|12135-76-1}}), also known as '''diammonium sulfide''' are commercially available, although the composition of these solutions is uncertain as they could consist of a mixture of ammonia and {{chem2|SH}}. Ammonium sulfide solutions are used occasionally in ], to apply ] to ], and in ] manufacturing. It can be used as a selective reducing agent (cf. ]); where there are two nitro groups, only one of them is selectively reduced.

The 1990–91 '']'' gives information for anhydrous ammonium monosulfide ({{chem2|2S}}) and ammonium pentasulfide ({{chem2|2S5}}) as separate from anhydrous ammonium hydrosulfide ({{chem2|SH}}), describing the former two both as yellow crystalline substances that are soluble in cold water and alcohol, and which both decompose in hot water or at high temperature in general (115&nbsp;°C for the pentasulfide), but the latter as a white crystalline solid (which also decomposes in hot water).<ref name="CRC" /> Thus, it seems that solid ammonium sulfide can be distinct from solid ammonium hydrosulfide, even if this is not true in aqueous solution.


==References== ==References==
{{reflist}} {{reflist}}

{{Ammonium salts}}
{{sulfur compounds}}


] ]
] ]


<!-- this link is to ammoniumsulfide, not the hydrogensulfide ] --> <!-- this link is to ammoniumsulfide, not the hydrogensulfide ] -->
<!-- this link is to ammoniumsulfide, not the hydrogensulfide ] --> <!-- this link is to ammoniumsulfide, not the hydrogensulfide ] -->

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