What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.59 V at standard temperature and pressure?

Class 12th Chemistry, Question -What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.59 V at standard temperature and pressure?

By
Komal Kohli
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Question 34:What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.59 V at standard temperature and pressure?

The correct answer is – The standard reduction potential of the hydrogen electrode is 0 V. At standard temperature and pressure, the potential of the hydrogen gas electrode is related to the pH of the solution by the Nernst equation:

E = E° – (0.0592 V / n) log([H+])

where E° is the standard reduction potential of the hydrogen electrode, n is the number of electrons transferred (which is 2 in this case), [H+] is the hydrogen ion concentration, and E is the electrode potential.

Substituting the values given:

-0.59 V = 0 V – (0.0592 V / 2) log([H+])

Solving for [H+]:

log([H+]) = -0.59 V / (0.0592 V) x 2

log([H+]) = -9.966

[H+] = 10^(-9.966)

[H+] = 1.18 x 10^(-10) M

Therefore, the pH of the HCl solution is:

pH = -log[H+] pH = -log(1.18 x 10^(-10)) pH = 9.93

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