Question

For the cell shown, the measured cell potential, Eₑₗₗ, is -0.3517 V at 25 °C.

Pt(s) | H₂(g, 0.847 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
2 H⁺(aq) + 2 e- → H₂(g) E° = 0.00 V
Cd²⁺(aq) + 2e- → Cd(s) E° = -0.403 V
Calculate the H⁺ concentration.
[H⁺] = ..... M

Answer 1

To calculate the H⁺ concentration in the cell, we can use the Nernst equation. By substituting the given values into the equation and solving for [H⁺], we find that the H⁺ concentration is approximately 6.07 x 10^11 M.

Step-by-step explanation:

To calculate the H⁺ concentration, we can use the Nernst equation:

E = E° - (0.0592/n) * log[H⁺]

Given the measured cell potential, Eₑₗₗ, and the standard reduction potential, E°, we can substitute these values into the equation:

-0.3517 V = 0.00 V - (0.0592/2) * log[H⁺]

Simplifying the equation, we have:

0.3517 V = (0.0592/2) * log[H⁺]

Now, we can solve for the H⁺ concentration:

log[H⁺] = (0.3517 V * 2) / 0.0592

log[H⁺] = 11.72

[H⁺] = 10^11.72 M

Therefore, the H⁺ concentration is approximately 6.07 x 10^11 M.