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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?
Solution
Given, the potential of hydrogen gas electrode = −0.59 V
Electrode reaction: \[\ce{H^{+} + e^{-} -> 0.5 H2}\]
Applying the Nernst equation,
E(H+/H2) = Eo(H+/H2) − `0.059/"n" log ([H_2]^(1/2))/([H^+])`
Eo(H+/H2) = 0 V
E(H+/H2) = −0.59 V
n = 1
[H2] = 1 bar
−0.59 = 0 − 0.059 (− log [H+])
−0.59 = −0.059 pH
∴ pH = 10
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