🤓 Based on our data, we think this question is relevant for Professor Vines' class at PITT.

Solution: Given the measured cell potential, Ecell, is -0.3641 V at 25 °C in the following cell, calculate the H+ concentration Pt (s) | H2(g, 0.769 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 2H+(aq) + 2e- → H2(g)                  E° = 0.00 V Cd2+ (aq) + 2e- → Cd(s)               E° = -0.403 V

Problem

Given the measured cell potential, Ecell, is -0.3641 V at 25 °C in the following cell, calculate the H+ concentration 

Pt (s) | H2(g, 0.769 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) 

The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 

2H+(aq) + 2e- → H2(g)                  E° = 0.00 V 

Cd2+ (aq) + 2e- → Cd(s)               E° = -0.403 V


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