Ammonium hydrosulfide

Ammonium hydrosulfide
Ammonium hydrosulfide
General
Systematic ; name	Ammonium hydrosulfide
Traditional names	Sulfuric Acid Ammonium
Chem. formula	NH 4 HS
Physical properties
condition	colorless crystals
Molar mass	51.1 g / mol
Density	1.17 g / cm³
Thermal properties
T. melt.	under pressure 120 ° C
Chemical properties
Solubility in water	128.1 0 g / 100 ml
Classification
Reg. CAS number	12124-99-1
PubChem
Reg. EINECS number
Smiles
Inchi
RTECS	BS4900000
ChemSpider

Ammonium hydrosulfide is an inorganic compound, an acid salt of ammonium and hydrogen sulfide with the formula NH ₄ HS, colorless crystals, readily soluble in cold water, decompose in hot water.

Content

1 Receiving
2 Physical properties
3 Chemical properties
4 Literature

Getting

The interaction of ammonia and hydrogen sulfide in ether or passing an excess of hydrogen sulfide through an ammonia solution:

{\mathsf {NH_{3}+H_{2}S\ {\xrightarrow {0^{o}C}}\ NH_{4}HS}}

{\ displaystyle {\ mathsf {NH_ {3} + H_ {2} S \ {\ xrightarrow {0 ^ {o} C}} \ NH_ {4} HS}}}

Physical Properties

Ammonium hydrosulfide forms colorless crystals of tetragonal syngony , space group P 4 / nmm , cell parameters a = 0.6011 nm, c = 0.4009 nm, Z = 2.

Volatile, vapor pressure at room temperature is 350 mm Hg. Art. .

It is well soluble in water and ethanol .

Aqueous solutions have a slightly alkaline reaction.

With prolonged exposure to air, the solution turns yellow (oxidizes to sulfur).

Chemical Properties

With slight heating decomposes:

{\mathsf {NH_{4}HS\ {\xrightarrow {20^{o}C}}\ NH_{3}+H_{2}S}}

{\ displaystyle {\ mathsf {NH_ {4} HS \ {\ xrightarrow {20 ^ {o} C}} \ NH_ {3} + H_ {2} S}}}

Decomposed by diluted acids:

{\mathsf {NH_{4}HS+HCl\ {\xrightarrow {}}\ NH_{4}Cl+H_{2}S\uparrow }}

{\ displaystyle {\ mathsf {NH_ {4} HS + HCl \ {\ xrightarrow {}} \ NH_ {4} Cl + H_ {2} S \ uparrow}}}

Oxidized with concentrated nitric acid:

{\mathsf {NH_{4}HS+3HNO_{3}\ {\xrightarrow {}}\ S\downarrow +2NO_{2}\uparrow +NH_{4}NO_{3}+2H_{2}O}}

{\ displaystyle {\ mathsf {NH_ {4} HS + 3HNO_ {3} \ {\ xrightarrow {}} \ S \ downarrow + 2NO_ {2} \ uparrow + NH_ {4} NO_ {3} + 2H_ {2} O }}}

Slowly oxidizes in air with the formation of various products:

{\mathsf {NH_{4}HS+O_{2}\ {\xrightarrow[{-NH_{3}}]{O_{2}}}\ S,(NH_{4})_{2}S_{n},(NH_{4})_{2}SO_{3}S}}

{\ displaystyle {\ mathsf {NH_ {4} HS + O_ {2} \ {\ xrightarrow [{- NH_ {3}}] {O_ {2}}} \ S, (NH_ {4}) _ {2} S_ {n}, (NH_ {4}) _ {2} SO_ {3} S}}}

In excess of ammonia dissolves sulfur, forming ammonium polysulfides :

{\mathsf {NH_{4}HS+NH_{3}+({\mathit {n}}-1)S\ {\xrightarrow {}}\ (NH_{4})_{2}S_{n}}}

{\ displaystyle {\ mathsf {NH_ {4} HS + NH_ {3} + ({\ mathit {n}} - 1) S \ {\ xrightarrow {}} \ (NH_ {4}) _ {2} S_ { n}}}}

Literature

Chemistry Handbook / Editorial: Nikolsky B.P. et al. - 2nd ed., rev. - M.-L.: Chemistry, 1966. - T. 1. - 1072 p.
Chemistry Handbook / Editorial: Nikolsky B.P. et al. - 3rd ed., rev. - L .: Chemistry, 1971. - T. 2. - 1168 p.
Lidin R.A. and other Chemical properties of inorganic substances: Textbook. manual for universities. - 3rd ed., Rev. - M .: Chemistry, 2000 .-- 480 p. - ISBN 5-7245-1163-0 .