Ammonium sulfide

Structural formula
General
Surname	Ammonium sulfide
other names	Ammonium sulfide
Molecular formula	(NH 4 ) 2 S.
Brief description	aqueous solution: colorless to yellowish, smelling of hydrogen sulfide
External identifiers / databases
CAS number 12135-76-1 EC number 235-223-4 ECHA InfoCard 100.032.009 PubChem 25519 ChemSpider 23808 Wikidata Q416913
properties
Molar mass	68.15 g mol −1
Physical state	firmly
density	1.00 g cm −3 (20 ° C)
Melting point	thermal decomposition: −18 ° C
Vapor pressure	546 hPa (at 20 ° C)
solubility	1280 g l −1 in water (at 20 ° C)
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 226-314-400 EUH: 031 P: 210-260-280-303 + 361 + 353-305 + 351 + 338-370 + 378
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Ammonium sulfide is an ammonium salt of hydrogen sulfide . It has the formula (NH ₄ ) ₂ S and belongs to the sulfide class .

Occurrence

In nature it arises as a product of putrefaction processes .

Extraction and presentation

Ammonium sulfide can be obtained from the reaction of ammonia (as a gas or in solution) with hydrogen sulfide.

The reaction equation is:

${\displaystyle \mathrm {2\;NH_{3}\;+\;H_{2}S\;\rightarrow (NH_{4})_{2}S} }$

Ion notation :

${\displaystyle \mathrm {2\;NH_{4}^{+}\;+\;S^{2-}\;\rightarrow (NH_{4})_{2}S} }$

use

Ammonium sulfide, together with ammonia, is often used in inorganic chemistry for qualitative analysis in order to precipitate the heavy metal cations of the elements nickel , cobalt , iron , manganese , chromium , aluminum and zinc as a group in the ammonium sulfide group from an unknown sample , separated and identified with the help of detection reactions.

Ammonium sulphide (like ammonium hydrogen sulphide and ammonium polysulphide ) is often a component of so-called stink bombs , which are sold in glass ampoules. This use is prohibited in Germany (Appendix 1 of the Consumer Goods Ordinance ).

The salt reacts with water to form hydrogen sulfide (HS ^- ) and hydroxide ions . An aqueous solution of ammonium sulfide is therefore only stable in a neutral and weakly basic environment - hydrogen sulfide gas escapes in acids , and ammonia gas in concentrated alkalis.

Ammonium sulfide can also be used to selectively reduce only one of the two nitro groups to an amino group in a dinitrobenzene .

Individual evidence

1. ↑ ^{a b c d e f} Entry on ammonium sulfide, aqueous solution in the GESTIS material database of the IFA , accessed on January 8, 2018(JavaScript required) .
2. ↑ ^{a b} entry on ammonium sulfide. In: Römpp Online . Georg Thieme Verlag, accessed on June 13, 2014.
3. ^ E. Schweda: Jander / Blasius: Inorganic Chemistry I - Introduction & Qualitative Analysis . 17th edition. Hirzel, 2012, ISBN 978-3-7776-2134-0 , pp. 505 .
4. ↑ PY Bruice: Organic Chemistry - compact studying . 5th edition. Pearson, 2011, ISBN 978-3-86894-102-9 , pp. 611 .