KF (s) → K+1 (aq) + F-1 (aq)

Back to reactions list

 

Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(K+1 (aq)) + 1ΔHf(F-1 (aq))] - [1ΔHf(KF (s))]
[1(-252.4) + 1(-332.6)] - [1(-568.61)] = -16.39 kJ
-16.39 kJ     (exothermic)

Entropy Change

[1ΔSf(K+1 (aq)) + 1ΔSf(F-1 (aq))] - [1ΔSf(KF (s))]
[1(102.5) + 1(-13.8)] - [1(66.57)] = 22.13 J/K
22.13 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(K+1 (aq)) + 1ΔGf(F-1 (aq))] - [1ΔGf(KF (s))]
[1(-283.3) + 1(-278.8)] - [1(-538.9)] = -23.2 kJ
-23.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-22.99 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

11606.20699
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (11606.20699) will be used to calculate the equilibrium concentration for all species.

KF K+1 F-1
Initial M   0 0
Change -x +x +x
Equilibrium