# 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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80% (386 ratings) ###### Problem Details

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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.

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