Modified Nernst equation:
• ↓ E° → oxidation → anode
• ↑ E° → reduction → cathode
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e- and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 X 10-3 M and the cell emf is 0.660 V? Use the reduction potentials in Appendix E that are reported to three significant figures.
(a) 3.3 X 10-2 M
(b) 1.9 X 10-4 M
(c) 9.0 X 10-3 M
(d) 6.9 X 10-4 M
(e) 7.6 X 10-3 M
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