Preparation of Iron (III) Sulfate
Naturally, iron sulfates are found in a variety of rare and commercially unimportant minerals. However, iron III sulfate is mainly found in minerals like pyrite and marcasite. In general, iron III sulfates are used as a solution that is generated from iron wastes. Although the actual specification is vague, its applications do not require high-purity materials.
On a large scale, iron III sulfates are prepared by treating sulfuric acid with a hot solution of iron(II) sulfate and an oxidizing agent. Hydrogen peroxide, chlorine, and nitric acid are some of the typical oxidizing agents used in the preparation of iron III sulfate.
2FeSO4 + H2SO4 + H2O2 → Fe2(SO4)3 + 2H2O
It can also be prepared industrially by injecting chlorine gas into an iron(II) sulfate solution, resulting in a mixture of iron(III) sulfate and iron(III) chloride.
3Cl2 + 6FeSO4 → 2Fe2(SO4)3 + 2FeCl3
Iron III Sulfate Formula
Iron(III) Sulfate is an inorganic compound that is also termed ferric sulfate. Its chemical formula is Fe2(SO4)3. In iron III sulfate, each iron atom has ionic bonds with the sulfate. A variety of hydrates of iron III sulfate are known, such as nonahydrate, anhydrous monohydrate, etc. In fact, they are the most commonly encountered form of “Iron III Sulfate”. It is slightly soluble in water and very hygroscopic. It is sparingly soluble in alcohol and negligibly soluble in acetone and ethyl acetate. It is not soluble in sulfuric acid and ammonia. As iron III sulfate is insoluble in sulfuric acid, it is used for producing iron III sulfate. It emits toxic fumes of iron and sulfur oxide when heated to decomposition. It is a threat to the environment and immediate steps should be taken to control its spread in the environment. It is used as a coagulant in water purification, as an astringent, and as a soil conditioner. It is corrosive to copper, copper alloys, mild steel, and galvanized steel.
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