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Problem- Calculate the cell voltage using the following half - reactions, standard reduction potentials and Ksp values for AgCl and PbF2 The concentrations of NaF and KCl are .10M in each half cell

Anode has Pb (s) + PbF2 + F^-

Cathode has Cl^- + AgCl(s) + Ag(a)

2 Ag+ + 2e yields 2 Ag(s) E = .7993 (occurs at cathode)

Pb^+2 yields Pb(s) E = -.126 (occurs at anode)

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