LiOH (s) → Li+1 (aq) + OH-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Li+1 (aq)) + 1ΔHf(OH-1 (aq))] - [1ΔHf(LiOH (s))]
[1(-278.5) + 1(-229.99)] - [1(-484.93)] = -23.56 kJ
-23.56 kJ     (exothermic)

Entropy Change

[1ΔSf(Li+1 (aq)) + 1ΔSf(OH-1 (aq))] - [1ΔSf(LiOH (s))]
[1(13.4) + 1(-10.75)] - [1(42.8)] = -40.15 J/K
-40.15 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Li+1 (aq)) + 1ΔGf(OH-1 (aq))] - [1ΔGf(LiOH (s))]
[1(-293.3) + 1(-157.28)] - [1(-438.9)] = -11.6800000000001 kJ
-11.68 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-11.59 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

111.26570635
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (111.26570635) will be used to calculate the equilibrium concentration for all species.

LiOH Li+1 OH-1
Initial M   0 0
Change -x +x +x
Equilibrium

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 226.

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