## NaF (s) → Na+1 (aq) + F-1 (aq)

Back to reactions list

## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Na+1 (aq)) + 1ΔHf(F-1 (aq))] - [1ΔHf(NaF (s))]
[1(-240.1) + 1(-332.6)] - [1(-575.3)] = 2.59999999999991 kJ
2.60 kJ     (endothermic)

## Entropy Change

[1ΔSf(Na+1 (aq)) + 1ΔSf(F-1 (aq))] - [1ΔSf(NaF (s))]
[1(59) + 1(-13.8)] - [1(51.21)] = -6.01 J/K
-6.01 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Na+1 (aq)) + 1ΔGf(F-1 (aq))] - [1ΔGf(NaF (s))]
[1(-261.9) + 1(-278.8)] - [1(-545.18)] = 4.4799999999999 kJ
4.48 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.16409459813
This process is close to or at equilibrium at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.16409459813) will be used to calculate the equilibrium concentration for all species.

 NaF Na+1 F-1 Initial M 0 0 Change -x +x +x Equilibrium