Given the following standard reduction potentials,
Pb²⁺(aq) + 2 e^- $\to$ Pb(s) $~~~~~~~~$ $~~~~~~~~$ $~~~~~~~~$ E^$\circ$ = -0.126 V
PbSO₄(s) + 2 e^- $\to$ Pb(s) + SO₄^2-(aq) $~~~~~~~~$ E^$\circ$ = -0.355 V
Determine K_sp for PbSO₄(s) at 25 ^$\circ$C.

Question

Given the following standard reduction potentials,
Pb²⁺(aq) + 2 e^-

\to

Pb(s)

~~~~~~~~

~~~~~~~~

~~~~~~~~

E^$\circ$ = -0.126 V
PbSO₄(s) + 2 e^-

\to

Pb(s) + SO₄^2-(aq)

~~~~~~~~

E^$\circ$ = -0.355 V
Determine K_sp for PbSO₄(s) at 25 ^$\circ$C.

Quizplus · Accepted Answer

The Ksp can be calculated using the Nernst equation and the given standard reduction potentials. The difference in potentials gives the solubility product constant, which is 1.8 × 10^-8.

Given the Following Standard Reduction Potentials, Pb2+(aq)+ 2 E- →\to→ Pb(s) ~~~~~~~~

Given the Following Standard Reduction Potentials,
Pb²⁺(aq)+ 2 E^- $\to$ Pb(s) $~~~~~~~~$