Standard reducation potential at `25^(@)C` of `Li^(+)//Li`, `Ba^(2+)//Ba, Na^(+)//Na` and `Mg^(+)//Mg` are `-3.05, -2.90, -2.71` and `-2.37` volt respectively. Which one of the following is the strongest oxidising agent ?

Options

A. `Mg^(2+)`
B. `Ba^(2+)`
C. `Na^(+)`
D. `Li^(+)`

Explanation

To determine which of the given species is the strongest oxidizing agent based on their standard reduction potentials, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Standard Reduction Potential**:
The standard reduction potential (SRP) indicates how readily a species gains electrons (is reduced). A higher (or less negative) SRP means that the species is more likely to be reduced and thus is a stronger oxidizing agent.

2. **List the Given Standard Reduction Potentials**:
- \( \text{Li}^+ + e^- \rightarrow \text{Li} \): \( E^\circ = -3.05 \, \text{V} \)
- \( \text{Ba}^{2+} + 2e^- \rightarrow \text{Ba} \): \( E^\circ = -2.90 \, \text{V} \)
- \( \text{Na}^+ + e^- \rightarrow \text{Na} \): \( E^\circ = -2.71 \, \text{V} \)
- \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} \): \( E^\circ = -2.37 \, \text{V} \)

3. **Compare the SRP Values**:
The higher the SRP value, the stronger the oxidizing agent. We compare the given values:
- \( -3.05 \, \text{V} \) (Li)
- \( -2.90 \, \text{V} \) (Ba)
- \( -2.71 \, \text{V} \) (Na)
- \( -2.37 \, \text{V} \) (Mg)

4. **Identify the Highest SRP**:
Among the given values, \( -2.37 \, \text{V} \) (for Mg) is the highest (least negative) value.

5. **Conclusion**:
Since magnesium has the highest standard reduction potential, it is the strongest oxidizing agent among the given options.

### Final Answer:
**The strongest oxidizing agent is \( \text{Mg}^{2+} \) (Magnesium).**