Titrating 100.0 mL of 0.0400 M Fe2 in 1 M HClO4 with 0.100 M Ce4 to give Fe3 and Ce3 using Pt and calomel electrodes to find the endpoint.

(a) Write the balanced titration reaction.

(b) Complete the two half reactions for the Pt electrode.
Ce + e- equilibrium ??? E potential= 1.70 v
Fe + e- equilibrium ??? E potential= 0.767

c) Write 2 Nernst equations for the cell. Each applying at different points in the titration.) E potential of the calomel electrode is 0.241 V.

d) Calculate the values of E for the cell when the following volumes of the ce4+ titrant hav been added:(Activity coefficients may be ignored as they tend to cancel when calculating concentration ratios). 1.50 ml 20.0 ml 39.0 ml 40.0 ml 44.0 ml 80.0 ml