Ga(OH)3 - GALLIUM (III) HYDROXIDE

Properties of gallium (III) hydroxide:

White, amorphous, when heated it is decomposes. Not soluble in water, precipitated from the solution in weak acidic and alkalescent environment. Shows amphoteric properties; it is transferred to solution by acids, alkalis and concentrated ammonium hydroxide.


Molar mass g/mol 120.74

Methods for preparation of gallium (III) hydroxide:

2Ga + 6H2O(hot) = 2Ga(OH)3↓ + 3H2↑,

2Ga + 4H2O(vapor) = 2GaO(OH) + 3H2 (350° C).

Ga(NO3)3 + 3NaOH(diluted) = Ga(OH)3↓ + 3NaNO3,

Ga(NO3)3 + 4NaOH(conc., hot) = Na[Ga(OH)4] + 3NaNO3.

Ga(NO3)3 + 3(NH3 • H2O)[diluted] = Ga(OH)3↓ + 3NH4NO3,

Ga(NO3)3 + 4(NH3 • H2O)[conc., cold] = NH4[Ga(OH)4] + 3NH4NO3.

2Ga(NO3)3 + 6HO + 3Na2S = 2Ga(OH)3↓ + 3H2S↑ + 6NaNO3.

Ga2(SO4)3 + 6NaOH(diluted) = 2Ga(OH)3↓ + 3Na2SO4,

Ga2(SO4)3 + 8NaOH(conc., hot) = 2Na[Ga(OH)4] + 3Na2SO4.

Ga2(SO4)3 + 6(NH3 • H2O)[diluted] = 2Ga(OH)3↓ + 3(NH4)2SO4,

Ga2(SO4)3 + 8(NH3 • H2O)[conc., cold] = 2NH4[Ga(OH)4] + 3(NH4)2SO4.

GaCl3 + 3NaOH(diluted) = Ga(OH)3↓ + 3NaCl,

GaCl3 + 4NaOH(conc., hot) = Na[Ga(OH)4] + 3NaCl.

GaCl3 + 3(NH3 • H2O)[diluted] = Ga(OH)3↓ + 3NH4Cl,

GaCl3 + 4(NH3 • H2O)[conc., cold] = NH4[Ga(OH)4] + 3NH4Cl.

Ga2S3 + 6H2O = 2Ga(OH)3↓ + 3H2S↑.


Chemical reactions with gallium (III) hydroxide:

Ga(OH)3 = GaO(OH) + H2O (80-400° C),

2Ga(OH)3 = Ga2O3 + 3H2O (540-600° C).

Ga(OH)3(solid) + 6H2O = [Ga(H2O)6](3+) + 3OH(-),

Ga(OH)3(solid) + 4H2O = [Ga(H2O)2(OH)4](-) + H3O(+).

Ga(OH)3 + 3HCl(diluted) = GaCl3 + 3H2O.

Ga(OH)3 + NaOH(conc., hot) = Na[Ga(OH)4],

Ga(OH)3 + NaOH = NaGaO2 + 2H2O (above 150° C).

Ga(OH)3 + NH3 • H2O(conc., cold) = NH4[Ga(OH)4].


 

Did you know?

Empirical formulas show the simplest whole number ratio of atoms in a formula.