In a Lead Storage Battery, the anode consists of lead ($Pb$) and the electrolyte is $38\%H_{2}S{O}_4$.

• During Discharge (acting as a galvanic cell):

1. At Anode (Oxidation): Lead is oxidized. However, because $S{O}_4^{2-}$ ions are present, the $P{b}^{2+}$ ions immediately precipitate as insoluble lead sulfate. $Pb(s)+S{O}_4^{2-}(aq)\to PbS{O}_4(s)+2e^{-}$
2. At Cathode (Reduction): $Pb{O}_2$ is reduced. $Pb{O}_2+S{O}_4^{2-}+4H^{+}+2e^{-}\to PbS{O}_4+2H_{2}O$

• Note that both reactions consume sulfuric acid and produce $PbS{O}_4$.