SrF2 (s) → Sr+2 (aq) + 2 F-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 2ΔHf(F-1 (aq))] - [1ΔHf(SrF2 (s))]
[1(-545.8) + 2(-332.6)] - [1(-1217.13)] = 6.13000000000011 kJ
6.13 kJ     (endothermic)

Entropy Change

[1ΔSf(Sr+2 (aq)) + 2ΔSf(F-1 (aq))] - [1ΔSf(SrF2 (s))]
[1(-32.6) + 2(-13.8)] - [1(82.13)] = -142.33 J/K
-142.33 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 2ΔGf(F-1 (aq))] - [1ΔGf(SrF2 (s))]
[1(-559.5) + 2(-278.8)] - [1(-1165.58)] = 48.48 kJ
48.48 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

3.20773783e-009
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.20773783e-009) will be used to calculate the equilibrium concentration for all species.

SrF2 Sr+2 F-1
Initial M   0 0
Change -x +x +2x
Equilibrium