Consider the cell: Ag(s), AgCl(s) \| KCl (0.1 M) \| Hg2Cl2(s), Hg(l). The cell potential — Electrochemistry Chemistry Question

💡 Solution & Explanation

The anode half-reaction is Ag(s) + Cl^–(aq) -> AgCl(s) + e^–. The cathode half-reaction is 1/2 Hg2Cl2(s) + e^– -> Hg(l) + Cl^–(aq). Adding these gives the overall net cell reaction: Ag(s) + 1/2 Hg2Cl2(s) -> AgCl(s) + Hg(l). Because Cl^–(aq) is both consumed and produced in equal amounts, it does not appear in the overall reaction. Thus, the cell potential is independent of the Cl^– concentration. Additionally, the potential of a cell is independent of the physical amounts of solid substances present. Therefore, correct answer is C,D.