Antimony(III) sulfate

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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[2]
Sb2(SO4)3
Molar mass 531.7078 g/mol
Density 3.94 g/cm3[1]
Hydrolysis[1]
Structure[1]
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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Antimony sulfate, Sb2(SO4)3, is a hygroscopic salt formed by reacting antimony or its compounds with hot

semiconductors and in the production of explosives and fireworks.[4]

Structure

Antimony(III) sulfate consists of interconnected SbO6 octahedra, which the corners are bonded to the sulfate ion.[1]

Production

Antimony(III) sulfate was first produced in 1827 by the reaction of

antimony(III) oxide and 18 molar sulfuric acid at 200 °C:[1]

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.[1][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

  1. ^
    doi:10.1107/S0567740876008881
    .
  2. ISBN 0-8493-0486-5
    .
  3. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  4. ^
    ISBN 3-527-20103-3
    .
  5. ISBN 978-0-7514-0389-3
    .
  6. ^ Method of forming phase change layer, method of manufacturing a storage node using the same, and method of manufacturing phase change memory device using the same – Samsung Electronics Co., Ltd. Freepatentsonline.com (2007-01-02). Retrieved on 2011-12-23.
  7. ^ Antimony(III) Sulfate Material Safety Data Sheet Archived 2012-04-26 at the Wayback Machine. Prochemonline.
  8. ^ "Klebelsbergite".
  9. ^ a b "List of Minerals". 21 March 2011.
  10. ^ "Coquandite".
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