A solution prepared by mixing 51.4 mL of 0.340 M AgNO3 and 51.4 mL of 0.340 M TlNO3 was titrated with 0.680 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TlBr is Ksp = 3.6 × 10–6 and the solubility constant of AgBr is Ksp = 5.0 × 10–13.
I know how to do a regular titration with Ag. I am thrown off by the NaBr. How does that fit in with the calculations?
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What is the cell voltage when the following volumes of 0.680 M NaBr have been added? (b) 1.0 mL (c) 13.2 mL (d) 24.7 mL (e) 25.6 mL (f) 26.0 mL (g) 38.9 mL (h) 51.4 mL (i) 52.0 mL
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