| Sodium thioantimoniate | |
|---|---|
|
Sodium thioantimoniate |
|
| Properties | |
| Molecular formula | Na3SbS4·9H2O |
| Appearance | Yellow crystals |
| Density | 1.806 g/cm³, solid |
| Melting point |
87°C (360.15 K) |
| Related compounds | |
| Other anions | Potassium thioantimoniate |
| Related compounds | Antimony(III) sulfide |
| (verify) (what is: /?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
|
| Infobox references | |
Sodium thioantimoniate, also known as Schlippe's salt, is an inorganic compound with the formula Na3SbS4.9H2O. This sulfosalt is named after K. F. Schlippe (1799-1867). Sodium thioantimoniate is used to make "quinsulfide antimony," Sb2S5. This salt consists of the tetrahedral SbS43- anion (rSb-S = 2.33 Å) and sodium cations, which are hydrated.[1][2] Related salts are known for different cations including ammonium and potassium.
Contents |
Sodium thioantimoniate is prepared by the reaction of antimony trisulfide, elemental sulfur, and aqueous sulfide source.
The sulfide can be generated indirectly by the thermal reaction of elemental sulfur with sodium hydroxide or even charcoal:
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:
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.
This article incorporates text from a publication now in the public domain: Chisholm, Hugh, ed (1911). "Schlippe's Salt". Encyclopædia Britannica (11th ed.). Cambridge University Press.