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For the reaction Ag+(aq) + Cl-(aq) -> AgCl(s), the standard free energies of formation are given as: ΔG°f(AgCl) = -109 kJ/mol, ΔG°f(Cl-) = -129 kJ/mol and ΔG°f(Ag+) = +77 kJ/mol. Using these data, what is the value of log10(Ksp) of AgCl at 298 K? (Take 2.303*R*T/F = 0.059 V)

1. -10
2. -5
3. +10
4. -12

Correct answer: -10

Solution

The combination reaction forming AgCl(s) is the reverse of the solubility equilibrium AgCl(s) -> Ag+ + Cl-. Its standard free energy gives the formation equilibrium constant, whose reciprocal is Ksp. A negative ΔG° (favourable precipitation) leads to a very small Ksp, hence a large negative log10(Ksp).

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