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formula for iron ii sulfate heptahydrate

One of the most common simple sulfates is the blue-green crystalline ferrous sulfate. This is a mildly reducing agent and is commonly used in organic synthesis. It also occurs naturally as a minor component of the soil and is found in a variety of iron-containing minerals.

It is soluble in water and slightly acidic, making it an ideal source of the iron metal for uses compatible with sulfates such as chelating agents, pH indicators, antibacterials, disinfectants, and enzyme inhibitors. It can also be incorporated into a range of organic molecules as a precursor for the synthesis of other metals and other organic compounds.

The most enticing aspect of this compound is that it can be manipulated into all sorts of different forms and sizes. The most interesting form is the heptahydrate. The heptahydrate is the product of three iron ions joined by two sulfate ions, each of which is 3+. The resulting compound has the best ion-to-ion dilution ratio of any hydrate.

Aside from the usual oxidation/reduction reactions, the iron sulfate heptahydrate is also notable for its ability to suck in water of crystallisation. In fact, it is capable of doing so in a manner not unlike the ancient process by which oak galls and copperas were produced.

In modern times, ferrous sulfate is often used in the manufacture of ink and a lawn conditioner. It is also a popular mordant for wool dyeing and a key ingredient in the manufacture of the famous China blue textile dye. It is also a reducing agent and an important part of the chemistry behind the production of titanium dioxide from ilmenite.