Zinc+Sulfate

Zinc sulfate is produced by treating zinc with aqueous [|sulfuric acid] : Zn + H2SO4 + 7 H2O → ZnSO4(H2O)7 + H2 Pharmaceutical grade zinc sulfate is produced from high purity [|zinc oxide] : ZnO + H2SO4 + 6 H2O → ZnSO4(H2O)7 In the laboratory, it can also be prepared by adding solid zinc to a [|copper(II) sulfate] solution: Zn + CuSO4 → ZnSO4 + Cu In aqueous solution, all forms of zinc sulfate behave identically. These aqueous solutions consist of the [|metal aquo complex] [Zn(H2O)6]2+and SO42- ions. [|Barium sulfate] forms when these solutions are treated with solutions of barium ions: ZnSO4 + BaCl2 → BaSO4 + ZnCl2 With a [|reduction potential] of -0.76, zinc(II) reduces only with difficulty. When heated over 680 C, zinc sulfate decomposes into [|sulfur dioxide] gas and [|zinc oxide] fume, both of which are hazardous. [|[]

__**Zinc sulfate**__ is the inorganic compound with the formula ZnSO4 as well as any of three hydrates. It was historically known as "white vitriol". It is a colorless solid that is a common source of soluble zinc ions.

The hydrates, especially the heptahydrate, are the primary forms used commercially. The main application is as a coagulant in the production of rayon. It is also a precursor to the pigment lithopone. Zinc sulfate is used to supply zinc in animal feeds, fertilizers, and agricultural sprays. Zinc sulfate, like many zinc compounds, can be used to control moss growth on roofs. It is used as in electrolytes for zinc plating, as a mordant in dyeing, as a preservative for skins and leather and in medicine as an astringent and emetic.