Pb2+ + 2 e‒ ⇌ Zn E° = ‒0.1262 V
Cd2+ + 2 e‒ ⇌ Cd E° = ‒0.4030 V
• ↓ E° → oxidation
Loss Electrons → Oxidation → Reducing Agent
• ↑ E° → reduction → cathode
Gain Electrons → Reduction → Oxidizing Agent
can be oxidized with a Pb2+ solution but not with a Cd2+ solution
Cr2+ + 2 e‒ ⇌ Cr E° = ‒0.913 V
• lower E° than Pb2+/Pb and Cd2+/Cd
• Cr → can be oxidized by both Pb2+ and Cd2+
Ni2+ + 2 e‒ ⇌ Ni E° = ‒0.257 V
• higher E° than Cd2+/Cd but lower than Pb2+/Pb
• Ni → can be oxidized by Pb2+ but not by Cd2+
Which metal(s) can be oxidized with a Pb2+ solution but not with a Cd2+ solution? (Hint: The reactions are occurring under standard conditions.)
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