Contents

Antimony(III) sulfate

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 Y
3D model (JSmol)	Interactive image
ChemSpider	22443 Y
ECHA InfoCard	100.028.370
EC Number	231-207-6
PubChem CID	24010
UNII	HN58C3HK0X Y
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 Y Key: MVMLTMBYNXHXFI-UHFFFAOYSA-H Y
SMILES [SbH3+3].[SbH3+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
Properties[2]
Chemical formula	Sb2(SO4)3
Molar mass	531.7078 g/mol
Density	3.94 g/cm3[1]
Solubility in water	Hydrolysis[1]
Structure[1]
Crystal structure	monoclinic
Space group	P21/c
Lattice constant	a = 13.12 Å, b = 4.75 Å, c = 17.55 Å α = 90°, β = 126.3°, γ = 90°
Lattice volume (V)	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). N (what is YN ?) Infobox references

Chemical compound

Antimony sulfate, Sb₂(SO₄)₃, is a hygroscopic salt formed by reacting antimony or its compounds with hot sulfuric acid. It is used in dopingofsemiconductors and in the production of explosives and fireworks.^[4]

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

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

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]

Owing to its solubility, antimony sulfate has uses in the doping of semiconductors.^[6] It is also used for coating anodesinelectrolysis and in the production of explosives and fireworks.^[4]

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

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]