Sodium thioantimoniate
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{{Chembox new
| Name = Sodium thioantimoniate
| IUPACName = Sodium thioantimoniate
| Section2 = {{Chembox Properties
| Formula = Na<sub>3</sub>(SbS<sub>4</sub>)9H<sub>2</sub>O
| Appearance = Yellow crystals
| Density = 1.806 g/cm³, solid
| MeltingPt = 87°C (360.15 K)
| BoilingPt =
}}
| Section8 = {{Chembox Related
| OtherAnions = Potassium thioantimoniate
| OtherCpds = [[Antimony(III) sulfide]]}}
}}
'''Sodium thioantimoniate''', also known as '''Schlippe's salt''', is an [[inorganic compound]] with the [[chemical formula|formula]] Na<sub>3</sub>SbS<sub>4</sub><sup>.</sup>9H<sub>2</sub>O. This [[sulfosalt]] is named after K. F. Schlippe (1799-1867). Sodium thioantimoniate is used to make "quinsulfide antimony," Sb<sub>2</sub>S<sub>5</sub>. This salt consists of the tetrahedral SbS<sub>4</sub><sup>3-</sup> anion (r<sub>Sb-S</sub> = 2.33 Å) and sodium cations, which are [[water of crystallization|hydrated]].<ref>Krebs, B., "Thio- and Seleno Compounds of Main Group Elements - New Inorganic Oligomers and Polymers", Angewandte Chemie, 1983, volume 95, pages 113-34.</ref><ref>K. Mereiter, A. Preisinger and H. Guth “Hydrogen bonds in Schlippe's salt: refinement of the crystal structures of Na<sub>3</sub>SbS<sub>4</sub><sup>.</sup>9H<sub>2</sub>O by X-ray diffraction and Na<sub>3</sub>SbS<sub>4</sub><sup>.</sup>9D<sub>2</sub>O by neutron diffraction at room temperature” Acta Crystallographica 1979, vol. B35, 19-25. doi:10.1107/S0567740879002442.</ref> Related salts are known for different cations including [[ammonium]] and [[potassium]].
==Preparation==
Sodium thioantimoniate is prepared by the reaction of [[antimony trisulfide]], elemental [[sulfur]], and aqueous [[sulfide]] source.
:3 Na<sub>2</sub>S + 2 S + Sb<sub>2</sub>S<sub>3</sub> + 9 H<sub>2</sub>O → 2 Na<sub>3</sub>SbS<sub>4</sub> • 9 H<sub>2</sub>O
The sulfide can be generated indirectly by the thermal reaction of elemental sulfur with [[sodium hydroxide]] or even charcoal:
:Sb<sub>2</sub>S<sub>3</sub> + 8 NaOH + 6 S → 2 Na<sub>3</sub>SbS<sub>4</sub> + Na<sub>2</sub>SO<sub>4</sub> + 4 H<sub>2</sub>O
In the latter route, a mixture of [[sodium sulfate]] (16 parts) is reduced by fusion with [[charcoal]] (4-5 parts) in the presence of antimony [[sulfide]] (13 parts). The melt is extracted into [[water]] which is treated with sulfur (4 parts). Upon evaporation of the solution , the [[salt]] crystallizes as large [[tetrahedra]], which are easily soluble in water. The [[anhydrous]] salt melts easily on heating, and in the hydrated condition, on exposure to moist air becomes coated with a red film.
The required antimony(III) sulfide is prepared in the usual way by treatment of virtually any Sb(III) compound with sulfide sources:
:2 SbCl<sub>3</sub> + 3 H<sub>2</sub>S → Sb<sub>2</sub>S<sub>3</sub> + 6 HCl
==Applications==
The Schlippes Salt was used to generate antimony(V) sulfide, which was used as an "amplifier" in silver-based photography, in matches as a flammable component, and for vulcanizing rubber. It is used in the [[electrolytic deposition]] of [[zinc]].{{Fact|date=March 2008}}
==Related compounds==
*Antimony(III)sulfide, Sb<sub>2</sub>S<sub>3</sub>
*"quinsulfide antimony" or "gold sulfur" Sb<sub>2</sub>S<sub>5</sub>
==References==
{{reflist}}
[[Category:Antimony compounds]]
[[Category:Sulfides]]
[[Category:Sodium compounds]]
[[ar:ثيوأنتيموانات صوديوم]]
[[ru:Соль Шлиппе]]