You are titrating 40.0 mL of 0.0100 M Sn2+ in 1 M HCl with 0.0500 M Tl3+ resulting in the formation of Sn4 and Tl. A Pt indicator electrode and a saturated Ag | AgCl reference electrode are used to monitor the titration. What is the balanced titration reaction? Complete the two half-reactions that occur at the Pt indicator electrode, Write the half-reactions as reductions,
half-reaction: Sn + e - → E0 = 139 V
half reaction: TI + e- → E0 = 0.77 V
Select the two equations that can be used to determine the cell voltage at different points in the titration. E of the saturated Ag l AgCI reference electrode is 0.197 V.
a. E = 0.139 - 0.05916log ([Sn2+] [Sn4+]) - 0.197
b. E = 0.139 - 0.05916log ([Sn4+]/[Sn2+]) - 0.197
c. E = 0.139 - 0.05916/2log ([Sn4+]/[Sn2+]) - 0.197
d. E = 0.139 - 0.05916 2log ([Sn2+] [Sn4+]) - 0.197
e. E = 0.139 - 0.05916log ([TI+] [TI3+]) - 0.197
f. E = 0.77 - 0.05916log ([TI3+]/[TI+] - 1 0.197
g. E = 0.77 - 0.05916 2log ([TI+] [TI3+]) - 0.197
Calculate the cell potential (E) after each of the given volumes of the Ti3+ titrant have been added.