Calculations determine the pH corresponding to a hydrogen electrode potential of 0.059 V using the Nernst equation, linking electrode potential with hydrogen ion concentration. The analysis explains how molar conductivity increases with dilution and contrasts the behavior of strong and weak electrolytes through a conceptual graph. Methods for evaluating the electromotive force of cells are detailed, including computations based on silver electrode reactions and electron transfer numbers. The discussion concludes with practical electrolysis challenges such as calculating the mass of deposited metals and examining the construction and performance of lead storage, nickel-cadmium, and fuel cells.