Lithium hydroxide

• Ätzlithion
• Ätzlithium
• Lithiumoxidhydrat

White solid

Fixed

1.46 g · cm -3

450 ° C.

924 ° C

Moderately soluble in water ( 128 g · l-1 solution at 20 ° C)

Risk

210 mg · kg -1 ( LD50, rat, oral)

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Lithium hydroxide LiOH, lithium hydroxide, is a true strong in water but only moderately soluble base.

Synthesis

Pure lithium oxide Li2O reacts with water to form lithium hydroxide.

The industrial production is carried out by reacting lithium carbonate with calcium hydroxide:

Pure lithium hydroxide can be prepared by reaction of lithium sulfate with barium hydroxide octahydrate. The resulting monohydrate may be reacted with P4O10 in vacuo for anhydrate.

Properties

Lithium hydroxide is a white, translucent solid with a crystal structure of PbO - type (space group P4/mm, a = 3.549, c = 4.334 Å). It is a strong base and, as such, reacts with acids. In addition, lithium is able to bind carbon dioxide (1 g of anhydrous lithium hydroxide binds 450 ml CO2).

Use

Most of the lithium hydroxide is required for the production of Lithiumstearaten which are important lubricating greases for cars or airplanes. It is also used due to its carbon dioxide -binding effect as an air cleaner. This plays a role, especially in the aerospace, submarine- and pendulum - breathing diving apparatus ( rebreathers ). Lithium hydroxide, cement may be added to and is able to suppress the alkali -silica reaction. Furthermore, lithium is a possible additive in nickel-iron batteries.

In pressurized water reactors of lithium hydroxide is added to the primary circuit in order to neutralize and boric acid to attain a pH of about 7.2.

Other applications include photo developer, ceramic products and the production of borates.