BaSO4 (s) → Ba+2 (aq) + SO4-2 (aq)

Back to reactions list

 

Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(BaSO4 (s))]
[1(-537.6) + 1(-909.27)] - [1(-1473.19)] = 26.3200000000002 kJ
26.32 kJ     (endothermic)

Entropy Change

[1ΔSf(Ba+2 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(BaSO4 (s))]
[1(9.6) + 1(20.08)] - [1(132.21)] = -102.53 J/K
-102.53 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(BaSO4 (s))]
[1(-560.8) + 1(-744.63)] - [1(-1362.31)] = 56.8800000000001 kJ
56.88 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.0826813347e-010
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.0826813347e-010) will be used to calculate the equilibrium concentration for all species.

BaSO4 Ba+2 SO4-2
Initial M   0 0
Change -x +x +x
Equilibrium