During discharging of a lead storage battery

Options

A. `Pb` is oxidized to `PbSO_(4)` at the anode
B. `PbO_(2)` is reduced to `PbSO_(4)` at the cathode
C. Both electrodes are immersed in the same aqueous solution of `H_(2)SO_(4)`
D. All of the above are true.

Explanation

**Step-by-Step Solution:**

1. **Understanding the Lead Storage Battery:**
- A lead storage battery consists of two electrodes: lead (Pb) and lead dioxide (PbO2), immersed in an electrolyte solution of sulfuric acid (H2SO4). During discharging, chemical reactions occur at both electrodes.

2. **Identifying the Oxidation Reaction:**
- At the anode, oxidation occurs. The oxidation half-reaction can be written as:
\[ \text{Pb (s)} + \text{SO}_4^{2-} \rightarrow \text{PbSO}_4 (s) + 2 \text{e}^- \]
- This indicates that solid lead (Pb) is oxidized to lead sulfate (PbSO4) while releasing two electrons.

3. **Identifying the Reduction Reaction:**
- At the cathode, reduction occurs. The reduction half-reaction can be written as:
\[ \text{PbO}_2 (s) + 4 \text{H}^+ (aq) + \text{SO}_4^{2-} (aq) + 2 \text{e}^- \rightarrow \text{PbSO}_4 (s) + 2 \text{H}_2\text{O} (l) \]
- This indicates that lead dioxide (PbO2) is reduced to lead sulfate (PbSO4) while consuming four protons and two electrons.

4. **Analyzing the Electrolyte:**
- Both electrodes are immersed in the same aqueous solution of sulfuric acid (H2SO4), which provides the necessary sulfate ions (SO4^2-) for the reactions.

5. **Conclusion:**
- Based on the reactions at the anode and cathode, as well as the electrolyte used, we can conclude:
- Option 1: Pb is oxidized to PbSO4 at the anode (True)
- Option 2: PbO2 is reduced to PbSO4 at the cathode (True)
- Option 3: Both electrodes are immersed in the same aqueous solution of H2SO4 (True)
- Therefore, Option 4: All the above are true (Correct)

**Final Answer:**
- The correct answer is **Option 4: All the above are true.**

---