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
Answers: 3
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You are titrating 45.0 mL of 0.0100 M Sn2+ in 1 M HCl with 0.0500 M Tl3+ resulting in the formation...
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