The standard electrode potentials at \(298 K\) are given. Arrange the following in the increasing strength of oxidizing agent
A. \(Ag^+ = 0.80 V\)
B. \(Zn^{2+} = -0.76 V\)
C. \(Cu^+ = 0.52 V\)
D. \(Pb^{2+} = -0.13 V\)
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 3
The correct answer is Option (3) → B < D < C < A
A standard electrode potential is a reduction potential. The higher (more positive) the E° of Mn+/M, the greater the tendency of the ion Mn+ to take electrons and be reduced, so the stronger it is as an oxidising agent. A more negative E° means a weaker oxidising agent.
Placing each ion by its E°, weakest oxidising agent first:
B. \( \ce{Zn^2+} \) (−0.76 V) — first. The most negative potential, the weakest oxidising agent.
D. \( \ce{Pb^2+} \) (−0.13 V) — second.
C. \( \ce{Cu+} \) (0.52 V) — third.
A. \( \ce{Ag+} \) (0.80 V) — last. The most positive potential, the strongest oxidising agent.
NCERT (2026-27 edition):
Measurement of Electrode Potential – …
