A cell based on the reaction below has a standard potential of +0.42 V at 25°C.If all of the species are at standard conditions except [H⁺],at what pH will the cell have a potential of zero? H₂O₂(aq)+ 2 H⁺(aq)+ 2 Cl^-(aq)→ Cl₂(aq)+ 2 H₂O(l) A)3.55 B)7.09 C)10.6 D)14.2

Question

Quizplus · Accepted Answer

To find the pH at which the cell potential is zero, we need to find the concentration of [H⁺]/[H₂O] that will make the cell potential equal to zero. At standard conditions, the Nernst equation can be written as: E° = 0.42 V = (0.0592 V/pH) log([H⁺]/[H₂O]) Solving for pH, we get: pH = 7.09

A Cell Based on the Reaction Below Has a Standard