## Ga(OH)3 (s) → Ga+3 (aq) + 3 OH-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ga+3 (aq)) + 3ΔHf(OH-1 (aq))] - [1ΔHf(Ga(OH)3 (s))]
[1(-211.7) + 3(-229.99)] - [1(-964.41)] = 62.7399999999999 kJ
62.74 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ga+3 (aq)) + 3ΔSf(OH-1 (aq))] - [1ΔSf(Ga(OH)3 (s))]
[1(-331) + 3(-10.75)] - [1(100.42)] = -463.67 J/K
-463.67 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ga+3 (aq)) + 3ΔGf(OH-1 (aq))] - [1ΔGf(Ga(OH)3 (s))]
[1(-159) + 3(-157.28)] - [1(-831.36)] = 200.52 kJ
200.52 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
200.98 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

7.3868818211e-036
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (7.3868818211e-036) will be used to calculate the equilibrium concentration for all species.

 Ga(OH)3 Ga+3 OH-1 Initial M 0 0 Change -x +x +3x Equilibrium