An aqueous electrolyte consists of the ions mentioned in the list , the ion which could be discharged most readily during electrolysis ?

Options

A. `Fe^(2+)`
B. `Cu^(2+)`
C. `Pb^(2+)`
D. `H^(+)`

Explanation

To determine which ion could be discharged most readily during electrolysis from an aqueous electrolyte, we need to consider the reduction potentials of the cations involved. Here’s a step-by-step solution:

### Step 1: Identify the Cations
First, identify the cations present in the aqueous electrolyte. For this example, let’s assume the cations are \( \text{Fe}^{2+}, \text{Pb}^{2+}, \text{H}^+, \text{Cu}^{2+} \).

### Step 2: Understand the Electrolysis Process
During electrolysis, cations migrate towards the cathode, where reduction occurs. The cation that is discharged most readily is the one that has the highest tendency to gain electrons (i.e., the one with the highest reduction potential).

### Step 3: Refer to the Electrochemical Series
Consult the electrochemical series to find the standard reduction potentials for the cations:
- \( \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \) (Standard reduction potential: -0.44 V)
- \( \text{Pb}^{2+} + 2e^- \rightarrow \text{Pb} \) (Standard reduction potential: -0.13 V)
- \( \text{H}^+ + e^- \rightarrow \frac{1}{2} \text{H}_2 \) (Standard reduction potential: 0.00 V)
- \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \) (Standard reduction potential: +0.34 V)

### Step 4: Compare the Reduction Potentials
Arrange the cations in order of their standard reduction potentials:
1. \( \text{Cu}^{2+} \) (0.34 V)
2. \( \text{H}^+ \) (0.00 V)
3. \( \text{Pb}^{2+} \) (-0.13 V)
4. \( \text{Fe}^{2+} \) (-0.44 V)

### Step 5: Identify the Ion Discharged Most Readily
From the comparison, \( \text{Cu}^{2+} \) has the highest reduction potential, indicating that it is discharged most readily at the cathode during electrolysis.

### Conclusion
Thus, the ion that could be discharged most readily during electrolysis is \( \text{Cu}^{2+} \).

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