LITHIUM HYDROXIDE LiOH

White, melts without decomposition, further heating is decomposed in an atmosphere of H2. It is readily soluble in water. Exhibits the properties of the basic hydroxide (alkali), reacts with acids, acid oxides, absorbs CO2 from the air.


Molar mass g/mol 23.95
Density g/cm3 1.46
Melting point °C 471

Obtaining lithium hydroxide LiOH:

2 Li + 2 H2O = 2 LiOH + H2↑.

LiH + H2O = LiOH + H2↑.

2 LiH + O2 = 2 LiOH (t> 500°C).

Li2O + H2O = 2 LiOH.

Li2CO3 + Ca(OH)2 = 2 LiOH + CaCO3 (to 600°C).

Li2SO4 + Ba(OH)2 = BaSO4 ↓ + 2LiOH.

2 LiCl + 2 H2O → Electrolysis 2 LiOH + H2↑ (cathode) + Cl2 (anode).


Reactions with lithium hydroxide LiOH:

2 LiOH = Li2O + H2O (800-1000°C, in the atm. H2).

LiOH-H2O = LiOH + H2O (500°C, in the atm. H2).

LiOH (dilute) + 4 H2O = [Li(H2O)4]+ + OH-.

LiOH + HCl (dilute.) = LiCl + H2O.

2 LiOH (conc.) + CO2 = Li2CO3 ↓ + H2O (norm. temp).

4 LiOH (dilute) + SiO2 (solid) ↔ Li4SiO4 (solution) + 2H2O (norm. temp).

2 LiOH (saturated) + SO2 = Li2SO3 + H2O.

2 LiOH + H2O + 2H2O2 (hot) = Li2O2-H2O2-3H2O↓ (in ethanol),

Li2O2-H2O2-3H2O = Li2O2 + H2O2 + 3H2O (over P4O10, vacuum).

2 LiOH (cold) + Cl2 = LiClO + LiCl + H2O,

6 LiOH (cold) + 3 Cl2 = LiClO3 + 5 LiCl + 3H2O.