1. The problem statement, all variables and given/known data Given the following half-reactions: Ce4+ + e− → Ce3+ E° = 1.72 V Fe3+ + e− → Fe2+ E° = 0.771 V A solution is prepared by mixing 9.0 mL of 0.30 M Fe2+ with 7.0 mL of 0.11 M Ce4+. 1. What is the potential of a platinum electrode dipped into the resulting, equilibrated, solution (relative to SHE)? 2. Calculate Keq for the reaction Ce4+ + Fe2+ ⇌ Ce3+ + Fe3+ 3. Calculate [Ce4+] in the solution. 2. Relevant equations Nernst equation 3. The attempt at a solution I got question 2 since its K = 10^(nEo/0.05916), K= 10^(1(1.72-0.771))/0.05916)=1.1*10^16 I tried and can't seem to get #1 correct. #3 I used ICE table method but cannot get a answer that makes sense. Any help is appreciated. Thanks.