Antimony sulfate

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.[2]

Antimony sulfate

Names
IUPAC name antimony(3+) trisulfate
Other names Antimony(III) sulfate Antimonous sulfate Antimony trisulfate Diantimony trisulfate Diantimony tris(sulphate)
Identifiers
CAS Number	7446-32-4
3D model (JSmol)	Interactive image
ChemSpider	22443
ECHA InfoCard	100.028.370
EC Number	231-207-6
PubChem CID	24010
UNII	HN58C3HK0X
CompTox Dashboard (EPA)	DTXSID10225469
InChI InChI=1S/3H2O4S.2Sb/c3*1-5(2,3)4;;/h3*(H2,1,2,3,4);;/q;;;2*+3/p-6 Key: MVMLTMBYNXHXFI-UHFFFAOYSA-H
SMILES [SbH3+3].[SbH3+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
Properties[1]
Chemical formula	Sb2(SO4)3
Molar mass	531.7078 g/mol
Density	3.6246 g/cm^3[2]
Solubility in water	soluble
Hazards
Safety data sheet	MSDS
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 0.5 mg/m^3 (as Sb)[3]
REL (Recommended)	TWA 0.5 mg/m^3 (as Sb)[3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

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 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]

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][11]

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. 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. 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. 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. https://www.mindat.org/min-2223.html
9. https://www.ima-mineralogy.org/Minlist.htm
10. https://www.mindat.org/min-1125.html
11. https://www.ima-mineralogy.org/Minlist.htm