Iron(III) sulfate
Iron sulfate or ferric sulfate is a family of inorganic compounds with the formula Fe23n. A variety of hydrates are known, including the most commonly encountered form of "ferric sulfate". Solutions are used in dyeing as a mordant and as a coagulant for industrial wastes. Solutions of ferric sulfate are also used in the processing of aluminum and steel.
Speciation
The various crystalline forms of Fe23n are well-defined, often by X-ray crystallography. The nature of the aqueous solutions is often less certain, but aquo-hydroxo complexes such as 3+ and 2+ are often assumed. Regardless, all such solids and solutions feature ferric ions, each with five unpaired electrons. By virtue of this high-spin d5 electronic configuration, these ions are paramagnetic and are weak chromophores.
Production
Ferric sulfate solutions are usually generated from iron wastes. The actual identity of the iron species is often vague, but many applications do not demand high-purity materials. It is produced on a large scale by treating sulfuric acid, a hot solution of ferrous sulfate, and an oxidizing agent. Typical oxidizing agents include chlorine, nitric acid, and hydrogen peroxide.
Natural occurrences
Iron sulfates occur as a variety of rare commercially unimportant minerals. The mineralogical form of iron sulfate, mikasaite, is a mixed iron-aluminium sulfate with the chemical formula 23. This anhydrous form occurs very rarely and is connected with coal fires. The hydrates are more common, with coquimbite as probably the most often met among them. Paracoquimbite is the other, rarely encountered natural nonahydrate. Kornelite and quenstedtite are rarely found. Andradite garnet is a yellow-green example found in Italy. Lausenite is a doubtful species. All the mentioned natural hydrates are unstable connected with the weathering of Fe-bearing primary minerals.