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Antimony sulfate

Names
IUPAC name Antimony(III) sulfate
Other names 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-6Key: MVMLTMBYNXHXFI-UHFFFAOYSA-H
SMILES ..S(=O)(=O).S()(=O)=O.S()(=O)=O
Properties
Chemical formula	Sb2(SO4)3
Molar mass	531.7078 g/mol
Density	3.94 g/cm
Solubility in water	Hydrolysis
Structure
Crystal structure	monoclinic
Space group	P21/c
Lattice constant	a = 13.12 Å, b = 4.75 Å, c = 17.55 Åα = 90°, β = 126.3°, γ = 90°
Lattice volume (V)	881 Å
Hazards
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 0.5 mg/m (as Sb)
REL (Recommended)	TWA 0.5 mg/m (as Sb)
Safety data sheet (SDS)	MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). N (what is  ?) Infobox references

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.

Structure

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

Production

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

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:

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.

Uses

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

Safety

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

Natural occurrence

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

References

1. ^ R. Mercier; J. Douglade; J. Bernard (1976). "Structure cristalline de Sb₂O₃.3SO₃". Acta Crystallographica Section B (in French). 32 (10): 2787–2791. doi:10.1107/S0567740876008881.
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. ^ NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
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.
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. ^ "List of Minerals". 21 March 2011.
10. "Coquandite".

• Antimony(III) compounds
• Sulfates