Question

1. Consider a cell in which the reaction is:

Pb (s) + 2 H+ (aq) 🡪 Pb2+ (aq) + H2 (g)

1. Calculate E◦ for this cell.
2. Chloride ions are added to the Pb|Pb2+ half-cell to precipitate PbCl2.  The voltage is measured to be +0.210 V.  Taking [H+] = 1.0 M and PH2 = 1.0 atm, calculate [Pb2+].
3. Taking [Cl-] in (b) to be 0.10 M, calculate Ksp of PbCl2.

Answer 1

Standard electrode potential of lead = -0.126V

E° cell = 0-(-0.126)

. E° cell = 0.126V