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Question

In a lead storage battery during discharge, the reaction at anode is:

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In a **Lead Storage Battery**, the anode consists of lead ($Pb$) and the electrolyte is $38\% H_2SO_4$.
- **During Discharge** (acting as a galvanic cell):
1. **At Anode** (Oxidation): Lead is oxidized. However, because $SO_4^{2-}$ ions are present, the $Pb^{2+}$ ions immediately precipitate as insoluble lead sulfate.
   $Pb(s) + SO_4^{2-}(aq) 	o PbSO_4(s) + 2e^-$
2. **At Cathode** (Reduction): $PbO_2$ is reduced.
   $PbO_2 + SO_4^{2-} + 4H^+ + 2e^- 	o PbSO_4 + 2H_2O$
- Note that both reactions consume sulfuric acid and produce $PbSO_4$.

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