NCERT chemistry 12th - electrochemistry - intext question 3.4 - Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10 ?

Question

Answer

Calculation of potential of hydrogen electrode in contact with pH 10 solution

Step 1: Write the half-reaction of the hydrogen electrode

2H+ + 2e- → H2

Step 2: Determine the standard electrode potential of the hydrogen electrode

The standard electrode potential of the hydrogen electrode is 0.00 V at 25°C and 1 atm H2 pressure.

Step 3: Calculate the activity of H+ ions from the given pH value

pH = -log [H+]

[H+] = 10^-pH = 10^-10

Step 4: Calculate the activity of electrons from the Nernst equation

E = E° - (RT/nF) ln Q

At 25°C, R = 8.314 J/K mol, F = 96485 C/mol, n = 2 (since 2 electrons are involved in the half-reaction)

Q = [H+]^2/P(H2), where P(H2) is the pressure of H2 gas (which is 1 atm in this case)

Q = [H+]^2

E = 0.00 - (8.314*298/2*96485) ln (10^-10)^2 = 0.414 V

Step 5: Conclusion

The potential of the hydrogen electrode in contact with a solution whose pH is 10 is 0.414 V. This means that the hydrogen electrode is a reducing agent and has a tendency to donate electrons. It can be used as a reference electrode to measure the potential of other electrodes.

Answer

0.06×ph=potential ans 0.6

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