Zinc sulfate, with the chemical formula ZnSO4, is an inorganic compound that exists in various hydrated forms, the most common being the heptahydrate, ZnSO4·7H2O. All these forms are colorless solids, though it is often encountered as a white crystalline powder. Understanding its chemical properties is fundamental to appreciating its diverse applications, from laboratory reagents to industrial synthesis.

In aqueous solutions, zinc sulfate dissociates into zinc ions ([Zn(H2O)6]2+) and sulfate ions (SO42−). This behavior is key to its role in electroplating and as a source of zinc in biochemical reactions. The production of zinc sulfate typically involves reacting zinc-containing materials, such as zinc metal or zinc oxide, with sulfuric acid. For instance, the reaction of zinc oxide with sulfuric acid yields zinc sulfate heptahydrate and water: ZnO + H2SO4 + 6 H2O → ZnSO4·7H2O.

The compound exhibits a relatively high melting point for its anhydrous form, decomposing at around 680°C. The heptahydrate form decomposes at a much lower temperature, around 100°C. Zinc sulfate is soluble in water, with solubility varying depending on temperature and the specific hydrate form. Its interaction with other ions, such as barium ions to form insoluble barium sulfate, is a common reaction utilized in analytical chemistry.

In scientific research, zinc sulfate solutions are used in various experimental setups, often serving as a cofactor for enzymes or as a means to introduce zinc ions into cellular systems. The purity of zinc sulfate is critical for sensitive applications, and manufacturers often provide detailed certificates of analysis to confirm its specifications. For those looking to buy zinc sulfate for research or industrial purposes, understanding its chemical characteristics ensures the selection of the appropriate grade and form.