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:

B < D < C < A

The correct answer is option 3. B < D < C < A.

To arrange the species in increasing order of oxidizing agent strength, we need to consider their standard electrode potentials (\(E^\circ\)).

The greater the standard electrode potential (\(E^\circ\)), the stronger the oxidizing agent. This is because a higher \(E^\circ\) indicates a higher tendency to gain electrons, which is characteristic of strong oxidizing agents.

Let us look at each of the given species:

B. \(Zn^{2+}\) (-0.76 V): This species has the most negative standard electrode potential among the given options. A more negative standard electrode potential indicates a greater tendency to lose electrons, which means \(Zn^{2+}\) is the weakest oxidizing agent among the options provided. It's more likely to be reduced (gain electrons) rather than act as an oxidizing agent.

D. \(Pb^{2+}\) (-0.13 V): \(Pb^{2+}\) has a less negative standard electrode potential compared to \(Zn^{2+}\), indicating a lower tendency to gain electrons. Therefore, it is a stronger oxidizing agent than \(Zn^{2+}\), but weaker than the other options.

C. \(Cu^+\) (0.52 V): With a positive standard electrode potential, \(Cu^+\) has a higher tendency to gain electrons compared to \(Pb^{2+}\) and \(Zn^{2+}\). Therefore, it is a stronger oxidizing agent than both \(Pb^{2+}\) and \(Zn^{2+}\).

A. \(Ag^+\) (0.80 V): Among the given options, \(Ag^+\) has the most positive standard electrode potential. This indicates the highest tendency to gain electrons, making it the strongest oxidizing agent among the options provided.

Therefore, the correct order from weakest to strongest oxidizing agent is \(Zn^{2+} < Pb^{2+} < Cu^+ < Ag^+\), consistent with option 3: \(B < D < C < A\).