Antimony sulfate

Antimony sulfate
Names
IUPAC name
antimony(3+) trisulfate
Other names
Antimony(III) sulfate
Antimonous sulfate
Antimony trisulfate
Diantimony trisulfate
Diantimony tris(sulphate)
Identifiers
7446-32-4 N[yes]
3D model (Jmol) Interactive image
ChemSpider 22443 YesY
ECHA InfoCard 100.028.370
EC Number 231-207-6
PubChem 24010
Properties[1]
Sb2(SO4)3
Molar mass 531.7078 g/mol
Density 3.6246 g/cm3[2]
soluble
Hazards
Safety data sheet MSDS
US health exposure limits (NIOSH):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[3]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N (what is YesYN ?)
Infobox references

Antimony sulfate, Sb2(SO4)3, is a hygroscopic material is 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.[2]

Structure

Solid antimony sulfate contains infinite ladders of SO4 tetrahedra and SbO3 pyramids sharing corners. It is often described as a mixed oxide, Sb2O3.3SO3.[4]

Chemical properties

Antimony sulfate is sometimes called a "salt" as it can be produced from the reaction of antimony and sulfuric acid, but it should be noted that antimony does not form a nitrate when dissolved in nitric acid, (an oxidising acid) but produces a mixture of antimony oxides, and this contrasts with bismuth which dissolves in both acids to form salts.[5] It 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.[2][5]

2 Sb (s) + 6 H2SO4 → Sb2(SO4)3 + 3SO2 + 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.[2]

Safety

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

References

  1. ↑ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. p. 4.64. ISBN 0-8493-0486-5.
  2. 1 2 3 4 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.
  3. 1 2 "NIOSH Pocket Guide to Chemical Hazards #0036". National Institute for Occupational Safety and Health (NIOSH).
  4. ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  5. 1 2 Nicholas C. Norman. 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. Prochemonline.
This article is issued from Wikipedia - version of the 11/2/2016. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.