Sodium Trithiostate

Sodium Trithiostate
Sodium Trithiostate
Are common
Systematic ; name	Sodium trithiostate (III)
Traditional names	sodium trithioantimonate; sodium trithioantimonite
Chem. formula	Na 3 [SbS 3 ]
Physical properties
condition	light yellow crystals
Molar mass	286.92 g / mol
Thermal properties
T. melt.	≈600 ° C
Chemical properties
Solubility in water	230 20 g / 100 ml

Sodium trithiostibate is an inorganic compound, a complex salt of antimony and sodium sulfides with the formula Na ₃ [SbS ₃ ], light yellow crystals soluble in water form a crystalline hydrate .

Content

Getting

Dissolution of antimony trisulfide in a hot solution of sodium hydroxide :

{\mathsf {Sb_{2}S_{3}+NaOH\ {\xrightarrow {100^{o}C}}\ Na_{3}[SbS_{3}]+Na[Sb(OH)_{4}]}}

{\ displaystyle {\ mathsf {Sb_ {2} S_ {3} + NaOH \ {\ xrightarrow {100 ^ {o} C}} \ Na_ {3} [SbS_ {3}] + Na [Sb (OH) _ { four}]}}}

Dissolution of antimony trisulfide in a concentrated solution of sodium sulfide :

{\mathsf {Sb_{2}S_{3}+3Na_{2}S\ {\xrightarrow {100^{o}C}}\ 2Na_{3}[SbS_{3}]}}

{\ displaystyle {\ mathsf {Sb_ {2} S_ {3} + 3Na_ {2} S \ {\ xrightarrow {100 ^ {o} C}} \ 2Na_ {3} [SbS_ {3}]}}}

Physical Properties

Sodium trithiostibate forms light yellow crystals that are readily soluble in water.

Forms a crystalline hydrate of the composition Na ₃ [SbS ₃ ] • 9H ₂ O.

Chemical Properties

Crystalline hydrate loses water when heated:

{\mathsf {Na_{3}[SbS_{3}]\cdot 9H_{2}O\ {\xrightarrow {150^{o}C}}\ Na_{3}[SbS_{3}]+9H_{2}O}}

{\ displaystyle {\ mathsf {Na_ {3} [SbS_ {3}] \ cdot 9H_ {2} O \ {\ xrightarrow {150 ^ {o} C}} \ Na_ {3} [SbS_ {3}] + 9H_ {2} O}}}

Destroyed by diluted acids:

{\mathsf {2Na_{3}[SbS_{3}]+6HCl\ {\xrightarrow {}}\ Sb_{2}S_{3}\downarrow +3H_{2}S\uparrow +6NaCl}}

{\ displaystyle {\ mathsf {2Na_ {3} [SbS_ {3}] + 6HCl \ {\ xrightarrow {}} \ Sb_ {2} S_ {3} \ downarrow + 3H_ {2} S \ uparrow + 6NaCl}}}

Destroyed by concentrated hot alkalis:

{\mathsf {Na_{3}[SbS_{3}]+4NaOH\ {\xrightarrow {100^{o}C}}\ Na[Sb(OH)_{4}]+3Na_{2}S}}

{\ displaystyle {\ mathsf {Na_ {3} [SbS_ {3}] + 4NaOH \ {\ xrightarrow {100 ^ {o} C}} \ Na [Sb (OH) _ {4}] + 3Na_ {2} S }}}

In the wet state, it is oxidized by atmospheric oxygen:

{\mathsf {Na_{3}[SbS_{3}]\ {\xrightarrow[{-S}]{O_{2}}}\ Na_{3}[SbS_{2}O],Na_{3}[SbSO_{2}]}}

{\ displaystyle {\ mathsf {Na_ {3} [SbS_ {3}] \ {\ xrightarrow [{- S}] {O_ {2}}} \ Na_ {3} [SbS_ {2} O], Na_ {3 } [SbSO_ {2}]}}}

In a boiling solution of sodium sulfide attaches sulfur:

{\mathsf {Na_{3}[SbS_{3}]+S\ {\xrightarrow {Na_{2}S}}\ Na_{3}[SbS_{4}]}}

{\ displaystyle {\ mathsf {Na_ {3} [SbS_ {3}] + S \ {\ xrightarrow {Na_ {2} S}} \ Na_ {3} [SbS_ {4}]}}}

Literature

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 .
Ripan R., Chetyanu I. Inorganic chemistry. Chemistry of metals. - M .: Mir, 1971. - T. 1. - 561 p.