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gas and lose electrolyte. Water can be replaced in a conventional wet-acid battery. In a sealed or gel-cell battery, it cannot. As we have seen, charging regenerates the H2SO4 electrolyte. Pure H2SO4 is 1.83 times as dense as water. As the H2SO4 is generated, it tends to sink. Since it is the H2SO4 that makes the electrolyte conductive, its absence at the top of the cell limits the acceptance of charging current. In a conventional wet-acid battery, acceptance is slow until gassing begins. Rising gas bubbles then mix the electrolyte, and acceptance increases. Gelled-electrolyte batteries capture the electrolyte in a gel, preventing strati cation and increasing initial charge acceptance. Starved electrolyte batteries accomplish the same goal by limiting the electrolyte to just enough to saturate the porous separators. Most serious is the phenomenon of sulfation. If a battery is left in a discharged state (i.e., with much of its electrodes in the form of PbSO4), the initially ne, soft deposits grow into larger, harder crystals that clog the holes of the sponged electrodes. The battery becomes dif cult to charge and displays reduced capacity. Vigorous overcharging and bubbling (equalization) can break up and dislodge the crystals, resulting in recovery of much of the original capacity. However, each time it is done, the plates shed more material and get closer to the end of their useful lives. So you see that, although the basic chemistry of all lead-acid batteries is the same, there are enough variations in construction to allow battery company marketing departments a eld day. B i o p h y s i c s D e mys tifie D
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