## Ba(IO3)2 (s) → Ba+2 (aq) + 2 IO3-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(IO3-1 (aq))] - [1ΔHf(Ba(IO3)2 (s))]
[1(-537.6) + 2(-221.33)] - [1(-1027.17)] = 46.9100000000001 kJ
46.91 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(IO3-1 (aq))] - [1ΔSf(Ba(IO3)2 (s))]
[1(9.6) + 2(118.41)] - [1(249.37)] = -2.95000000000002 J/K
-2.95 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(IO3-1 (aq))] - [1ΔGf(Ba(IO3)2 (s))]
[1(-560.8) + 2(-128.03)] - [1(-864.83)] = 47.9700000000001 kJ
47.97 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

3.9405058079e-009
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.9405058079e-009) will be used to calculate the equilibrium concentration for all species.

 Ba(IO3)2 Ba+2 IO3-1 Initial M 0 0 Change -x +x +2x Equilibrium