Names | |
---|---|
IUPAC name
Antimony(III) sulfate
| |
Other names
Antimonous sulfate
Antimony trisulfate Diantimony trisulfate Diantimony tris(sulphate) | |
Identifiers | |
3D model (
JSmol)
|
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ChemSpider | |
ECHA InfoCard | 100.028.370 |
EC Number |
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PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
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Properties [2] | |
Sb2(SO4)3 | |
Molar mass | 531.7078 g/mol |
Density | 3.94 g/cm3 [1] |
Hydrolysis [1] | |
Structure [1] | |
monoclinic | |
P21/c | |
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).
|
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. [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]
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]
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 anodes in electrolysis 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]
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 |
EC Number |
|
PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties [2] | |
Sb2(SO4)3 | |
Molar mass | 531.7078 g/mol |
Density | 3.94 g/cm3 [1] |
Hydrolysis [1] | |
Structure [1] | |
monoclinic | |
P21/c | |
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).
|
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. [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]
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]
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 anodes in electrolysis 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]