You are titrating 45.0 mL of 0.0100 M Sn2+ in 1 M HCl with 0.0500 M Tl3+ resulting in the formation of Sn4+ and Tl+. A Ptindicator electrode and a saturated Ag|AgCl reference electrode are used to monitor the titration. What is the balanced titration reaction? titration reaction: ⟶ 1. Complete the two half‑reactions that occur at the Pt indicator electrode. Write the half-reactions as reductions. half-reaction: Sn+e−↽−−⇀ ∘=0.139 V half-reaction: Tl+e−↽−−⇀ ∘=0.77 V 2. Select the two equations that can be used to determine the cell voltage at different points in the titration. of the saturated Ag|AgCl reference electrode is 0.197 V. a. =0.139−0.05916log([Sn2+][Sn4+])−0.1 97 b. =0.139−0.05916log([Sn4+][Sn2+])−0.1 97 c. =0.139−0.059162log([Sn4+][Sn2+])−0. 197