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| IUPAC name
| Other names
|Molar mass|| 161.47 g/mol (anhydrous)|
179.47 g/mol (monohydrate)
287.53 g/mol (heptahydrate)
|Density|| 3.54 g/cm3 (anhydrous)|
2.072 g/cm3 (hexahydrate)
|Melting point|| 680 °C (1,256 °F; 953 K) decomposes (anhydrous)|
100 °C (212 °F; 373 K) (heptahydrate)
70 °C (158 °F; 343 K) decomposes (hexahydrate)
|Boiling point|| 740 °C (1,360 °F; 1,010 K) (anhydrous)|
280 °C (536 °F; 553 K), decomposes (heptahydrate)
57.7 g/100 mL (25 °C)
101 g/100 ml (70 °C)
|Solubility||Insoluble in ethanol, toluene|
|Safety data sheet||LabChem (heptahydrate)|
| Cadmium sulfate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Zinc sulfate is a white hygroscopic solid. It is soluble in water and some alcohols. It forms three hydrates.
Zinc sulfate heptahydrate can be found in nature as the mineral known as goslarite.
Zinc supplements generally contain zinc sulfate, usually mixed with vitamins or sweeteners and are available at pharmacies.
Lastly, it can also be bought from chemical suppliers.
Zinc sulfate can be prepared by adding zinc metal to a solution of copper(II) sulfate. Metallic copper sponge will precipitate (with small amounts of copper(II) oxide and copper(I) oxide) and the solution will become colorless when the reaction stops. The filtered solution can be boiled to crystallize the zinc sulfate from the solution.
Zinc sulfate has low toxicity and is also sold as a supplement. It's best to avoid consuming lab-grade ZnSO4 though, as it may contain traces of heavy metals (cadmium e.g.). Anhydrous zinc sulfate may cause irritations.
The anhydrous form should be stored in closed bottles to prevent hydration. Otherwise there are no special procedures needed.
It may be recovered a zinc metal through electrolysis.