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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 3.6246 g/cm3[1]
soluble
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 sulfuric acid. It is used in doping of semiconductors and in the production of explosives and fireworks.[1]

Structure

Solid antimony(III) sulfate has a three-dimensional structure: SbO6 octahedra share corners with SO4 tetrahedra.[4]

Chemical properties

Antimony sulfate is deliquescent, and soluble in acids. It can be prepared by dissolving antimony, antimony trioxide, antimony trisulfide or antimony oxychloride in hot, concentrated sulfuric acid.[1][5]

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

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.[1]

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. ^ a b c d Herbst, Karl Albert et al. (1985) Antimony and antimony compounds in Ullmann's Encyclopedia of Industrial Chemistry 5th ed., vol. A3, p. 70. ISBN 3-527-20103-3.
  2. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton, Florida: CRC Press. p. 4.64. ISBN 0-8493-0486-5.
  3. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Materials Data on Sb2(SO4)3 by Materials Project
  5. ^ Nicholas C. Norman (31 December 1997). Chemistry of arsenic, antimony, and bismuth. Springer. pp. 193–. 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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