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Nernst Equation

The EMF of th...

Question

The EMF of the cell $p t, H_{2} (1 a t m) | H^{\oplus} (c) | | K C l (s a t u r a t e d) | H g_{2} C l_{2} | H g (s)$ is $0.36$ V. The RHE is know as calomel electrode and its standard electrode potential is + $0.242$ V. Find the $H^{\oplus}$ ions concentration in LHE and hence find the pH of LHE.

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Solution

$E_{c e l l} = 0.36 V$
$E_{c e l l}^{⊖} = E_{(C l^{⊖} | H g_{2} C l_{2} | | H g)}^{⊖} - 0 = 0.242 V$
$\Rightarrow 0.36 = 0.242 - \frac{0.059}{1} l o g \frac{[H^{\oplus}]}{[p_{H_{2}]}^{1 / 2}}$
$\Rightarrow 0.118 = - 0.118 = - 0.059 l o g [H^{\oplus}]$
$\Rightarrow - l o g [H^{\oplus}] = p H \frac{0.118}{0.059} = 2$
pH = 2

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