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  4. Calculate the pH of a buffer when the reduction potential of hydrogen electrode placed in the buffer solution is found to be -0.413V .

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Q. Calculate the $pH$ of a buffer when the reduction potential of hydrogen electrode placed in the buffer solution is found to be $-0.413V$ .

NTA AbhyasNTA Abhyas 2020Electrochemistry

Solution:

Apply Nernst Equation on the given reduction reaction of hydrogen.

$H^{+}\left(aq\right)+e^{-} \rightarrow \frac{1}{2}H_{2}\left(g\right)$

$E_{cell}=E_{cell}^{^\circ }-\frac{0 . 059}{n}log\frac{1}{\left[H^{+}\right]}$

Where $E_{H^{+} / H_{2}}^{^\circ }=0V$ and $n=1$

$-0.413=-0.059log\frac{1}{\left[H^{+}\right]}$ or $\frac{0 . 414}{0 . 059}=-log\left[H^{+}\right]=pH$

$pH=7$