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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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Latest revision as of 10:04, 8 March 2024

Ammonium hydrosulfide
Names
IUPAC name ammonium hydrosulfide
Other names ammonium bisulfide
ammonium hydrogen sulfide
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.974 Edit this at Wikidata
EC Number
  • 235-184-3
PubChem CID
RTECS number
  • BS4900000
UNII
UN number 2683
CompTox Dashboard (EPA)
InChI
  • InChI=1S/H3N.H2S/h1H3;1H2Key: HIVLDXAAFGCOFU-UHFFFAOYSA-N
  • InChI=1/H3N.H2S/h1H3;1H2Key: HIVLDXAAFGCOFU-UHFFFAOYAU
SMILES
  • .
Properties
Chemical formula [NH4]SH
Molar mass 51.111 g/mol
Appearance Yellow-orange fuming liquid (in solution). White rhombic crystals (anhydrous).
Density 1.17 g/cm
Boiling point 56.6 °C (133.9 °F; 329.8 K)
Solubility in water Miscible
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 Toxic
GHS labelling:
Pictograms GHS05: CorrosiveGHS09: Environmental hazard
Signal word Danger
Hazard statements H314, H400.
Precautionary statements P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P391, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 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. gasolineInstability (yellow): no hazard codeSpecial hazards (white): no code
3 3
Lethal dose or concentration (LD, LC):
LD50 (median dose) 168 mg/kg (rat, oral)
Related compounds
Other anions Ammonia solution
Other cations Sodium hydrosulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Ammonium hydrosulfide is the chemical compound with the formula [NH4]SH.

Composition

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 [NH4]SH 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.

Preparation

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·2[NH4]SH. When this species is cooled to 0 °C and treated with additional hydrogen sulfide, one obtains [NH4]2S·12[NH4]SH. 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

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:

NH3 + H2S → NH4SH

"Ammonium sulfide"

A bottle of ammonium sulfide solution

Aqueous solutions of ammonium sulfide (CAS registry number 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 [NH4]SH. Ammonium sulfide solutions are used occasionally in photographic developing, to apply patina to bronze, and in textile manufacturing. It can be used as a selective reducing agent (cf. 2,4-dinitrochlorobenzene); where there are two nitro groups, only one of them is selectively reduced.

The 1990–91 CRC Handbook of Chemistry and Physics gives information for anhydrous ammonium monosulfide ([NH4]2S) and ammonium pentasulfide ([NH4]2S5) as separate from anhydrous ammonium hydrosulfide ([NH4]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 °C for the pentasulfide), but the latter as a white crystalline solid (which also decomposes in hot water). Thus, it seems that solid ammonium sulfide can be distinct from solid ammonium hydrosulfide, even if this is not true in aqueous solution.

References

  1. ^ Lide, David R., ed. (1990). "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (71st ed.). CRC Press, inc. p. 4-45.
  2. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  3. Record of ammonium hydrosulfide in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on October 22, 2010.
  4. Goodman, J. T.; Rauchfuss, T. B. (2002). "Useful Reagents and Ligands". Inorganic Syntheses. Inorganic Syntheses. Vol. 33. pp. 107–110. doi:10.1002/0471224502.ch2. ISBN 978-0-471-20825-9.
  5. W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277.
  6. C. D. West (1934). "The Crystal Structures of Some Alkali Hydrosulfides and Monosulfides". Zeitschrift für Kristallographie - Crystalline Materials. 88 (1–6): 97–115. doi:10.1524/zkri.1934.88.1.97. S2CID 100849097.
Ammonium salts
Inorganic salts
monatomic anions
oxyanions
other anions
Organic salts
Sulfur compounds
Sulfides and
disulfides
Sulfur halides
Sulfur oxides
and oxyhalides
Sulfites
Sulfates
Sulfur nitrides
Thiocyanates
Organic compounds


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