Ferric hydroxide 3

Inorganic compound, iron hydroxide 3 has the chemical formula Fe (OH) 2. It belongs to a series of amphoteric iron compounds, in which the properties characteristic of bases predominate. In appearance, this substance is a crystal of white color, which with a long stay in the open air gradually darkens. There are variants of crystals of a greenish shade. In everyday life, the substance can be observed each in the form of a greenish coating on the metal surfaces, which indicates the beginning of the rusting process - iron hydroxide 3 acts as one of the intermediate stages of this process.

In nature, the compound is in the form of amakinite. This crystalline mineral, in addition to the iron proper, contains still impurities of magnesium and manganese, all these substances give amakinite different shades - from yellow-green to pale-green, depending on the percentage of this or that element. The hardness of the mineral is 3.5-4 units on the Mohs scale, and the density is approximately 3 g / cm³.

The physical properties of the substance should also include its extremely weak solubility. In the case where the hydroxide of iron 3 is heated, it decomposes.

This substance is very active and interacts with many other substances and compounds. So, for example, having the properties of the base, it enters a neutralization reaction with various acids. In particular, sulfuric acid, iron hydroxide 3 during the reaction lead to the production of ferric sulfate . Since this reaction can take place by means of conventional calcination in the open air, such an inexpensive method of producing sulphate is used both in laboratory and industrial conditions.

During the reaction with hydrochloric acid, its result is the formation of iron (II) chloride.

In some cases, iron hydroxide 3 can also exhibit acidic properties. So, for example, when interacting with a highly concentrated (concentration should be not less than 50%) sodium hydroxide solution, sodium tetrahydroxoferrate (II) is obtained, precipitating as a precipitate. True, for the flow of such a reaction it is necessary to provide rather complicated conditions: the reaction must take place under the boiling point of the solution in a nitrogen atmospheric medium.

As already mentioned, the substance decomposes on heating. The result of this decomposition is iron (II) oxide , and, in addition, metallic iron and its derivatives are obtained as impurities: Dicelose (III) oxide, whose chemical formula is Fe3O4.

How to produce iron hydroxide 3, the production of which is associated with its ability to react with acids? Before starting the experiment, it is necessary to recall the safety rules for conducting such experiments. These rules are applicable for all cases of handling acid-base solutions. The main thing here is to provide reliable protection and to avoid getting drops of solutions on mucous membranes and skin.

Thus, it is possible to obtain hydroxide during the reaction in which ferric chloride and hydroxide are reacted. This method is the most common method for the formation of insoluble bases. When these substances interact, the usual exchange reaction proceeds, resulting in a brown precipitate. This precipitate is the desired substance.

The use of iron hydroxide in industrial production is quite widespread. The most common is its use as an active substance in iron-nickel-type accumulators. In addition, the compound is used in metallurgy for the production of various metal alloys, as well as in galvanic production, and automotive engineering.