BaF2 (s) → Ba+2 (aq) + 2 F-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(F-1 (aq))] - [1ΔHf(BaF2 (s))]
[1(-537.6) + 2(-332.6)] - [1(-1208.76)] = 5.95999999999981 kJ
5.96 kJ     (endothermic)

Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(F-1 (aq))] - [1ΔSf(BaF2 (s))]
[1(9.6) + 2(-13.8)] - [1(96.4)] = -114.4 J/K
-114.40 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(F-1 (aq))] - [1ΔGf(BaF2 (s))]
[1(-560.8) + 2(-278.8)] - [1(-1158.55)] = 40.1499999999999 kJ
40.15 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

9.2391694103e-008
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (9.2391694103e-008) will be used to calculate the equilibrium concentration for all species.

BaF2 Ba+2 F-1
Initial M   0 0
Change -x +x +2x
Equilibrium