What is the reduction potential of a hydrogen electrode that is still at standard pressure, but has ph = 5.65 , relative to the she?

Explanation:

We must use the Nernst equation

1. Write the equation for the cell reaction

If you want the reduction potential, the pH 5.65 solution is the cathode, and the cell reaction is

                                                                      E°/V

  Anode: H₂(1 bar) ⇌ 2H⁺(1 mol·L⁻¹) + 2e⁻;     0

Cathode: 2H⁺(pH 5.65) + 2e⁻ ⇌ H₂(1 bar);     0

 Overall: 2H⁺ (pH 5.65) ⇌ 2H⁺(1 mol·L⁻¹);      0

Step 2. Calculate E°

(a) Data

   E° = 0

   R = 8.314 J·K⁻¹mol⁻¹

   T = 25 °C

   n = 2

   F = 96 485 C/mol

pH = 5.65

Calculations:  

T = 25 + 273.15 = 298.15 K

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