The standard reduction potentials for a reaction are as follows: Pb²⁺(aq) + 2 e^- → Pb(s)
E° = -0.126 V
PbSO₄(s) + 2 e^- → Pb(s) + SO₄^2-(aq)
E° = -0.355 V
Calculate the K_sp for lead(II) sulfate (PbSO₄) at 25 °C.

Question

Quizplus · Accepted Answer

The difference in standard reduction potentials (ΔE°) is used to calculate the equilibrium constant (K) for the dissolution of PbSO₄. ΔE° = E°(Pb²⁺/Pb) - E°(PbSO₄/Pb) = -0.126 V - (-0.355 V) = 0.229 V. Using the Nernst equation, K = 10^(nFΔE°/RT), where n = 2, F = 96485 C/mol, R = 8.314 J/mol·K, and T = 298 K. This gives K ≈ 1.8 × 10⁻⁸.

The Standard Reduction Potentials for a Reaction Are as Follows