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Nernst Equation

The cell Pt...

Question

The cell $P t (H_{2}) (1 a t m) | H^{+} (p H = ?), I^{-} (a = 1) / A g l (s), A g h a s e m f, E_{298 K} = 0$ . The electrode potential for the reaction $A g l + e^{-} \to A g + I^{⊖} i s - 0.151$ volt. Calculate the $p H$ value :-

3.37

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5.26

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2.56

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4.62

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Solution

The correct option is A $2.56$
$\frac{1}{2} H_{2} + A g l ⟶ H^{+} + A g + I^{-} E = 0$
$\frac{1}{2} H_{2} ⟶ H^{+} + e^{-} E = 0.151$
$0.151 = - \frac{0.059}{1} log (H^{+}) = 0.059 \times p H$
$p H = \frac{0.151}{0.059} = 2.5$

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