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Antimony(III) sulfate

Chemical compound From Wikipedia, the free encyclopedia

Antimony sulfate, Sb2(SO4)3, is a hygroscopic salt formed by reacting antimony or its compounds with hot sulfuric acid. It is used in doping of semiconductors and in the production of explosives and fireworks.[4]

Quick facts Names, Identifiers ...
Antimony sulfate
Names
IUPAC name
Antimony(III) sulfate
Other names
Antimonous sulfate
Antimony trisulfate
Diantimony trisulfate
Diantimony tris(sulphate)
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.370 Edit this at Wikidata
EC Number
  • 231-207-6
UNII
  • InChI=1S/3H2O4S.2Sb/c3*1-5(2,3)4;;/h3*(H2,1,2,3,4);;/q;;;2*+3/p-6 checkY
    Key: MVMLTMBYNXHXFI-UHFFFAOYSA-H checkY
  • [SbH3+3].[SbH3+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
Properties[1]
Sb2(SO4)3
Molar mass 531.7078 g/mol
Density 3.94 g/cm3[2]
Hydrolysis[2]
Structure[2]
monoclinic
P21/c
a = 13.12 Å, b = 4.75 Å, c = 17.55 Å
α = 90°, β = 126.3°, γ = 90°
881 Å3
Hazards
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[3]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[3]
Safety data sheet (SDS) MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure

Antimony(III) sulfate consists of interconnected SbO6 octahedra, which the corners are bonded to the sulfate ion.[2]

Production

Antimony(III) sulfate was first produced in 1827 by the reaction of antimony(III) oxide and 18 molar sulfuric acid at 200 °C:[2]

Sb2O3 + 3 H2SO4 → Sb2(SO4)3 + 3 H2O

The concentration of the sulfuric acid is important, as a lower concentration will produce basic antimony oxides, while a higher concentration will produce antimony(III) pyrosulfate. The reaction of elemental antimony and 18 M sulfuric acid will also produce antimony(III) sulfate:[4]

2 Sb + 6 H2SO4 → Sb2(SO4)3 + 3 SO2 + 6 H2O

Chemical properties

Antimony sulfate is deliquescent, hydrolyzing in moist air and water, producing various basic antimony oxides and antimony(III) oxide. It is soluble in acids.[2][4][5]

Uses

Owing to its solubility, antimony sulfate has uses in the doping of semiconductors.[6] It is also used for coating anodes in electrolysis and in the production of explosives and fireworks.[4]

Safety

Antimony(III) sulfate causes irritation to the skin and mucous membranes.[7]

Natural occurrence

Natural analogue of the exact compound is yet unknown. However, basic hydrated Sb sulfates are known as the minerals klebelsbergite[8][9] and coquandite.[10][9]

References

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