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.[1]
Antimony(III) sulfate consists of interconnected SbO6 octahedra, which the corners are bonded to the sulfate ion.[2]
Antimony(III) sulfate was first produced in 1827 by the reaction of antimony(III) oxide and 18 molar sulfuric acid at 200 °C:
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:
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] [3]
Owing to its solubility, antimony sulfate has uses in the doping of semiconductors.[4] It is also used for coating anodes in electrolysis and in the production of explosives and fireworks.[1]
Antimony(III) sulfate causes irritation to the skin and mucous membranes.[5]
Natural analogue of the exact compound is yet unknown. However, basic hydrated Sb sulfates are known as the minerals klebelsbergite[6] [7] and coquandite.[8] [7]