The cell potential for the following cell $Pt$ \left|{H}_{2} $\left(g\right)\right|{H}^{+}\left(aq\right) | | {Cu}^{2 +}\left(0 .01 M\right)|Cu\left(s\right)$ is $0 . 576V$ at $298K$ . The $pH$ of the solution is (Nearest integer)
(Given : ${E}_{{Cu}^{2 +} / Cu}^{o} = 0 . 34V$ and $\dfrac{2 . 303RT}{F} = 0 . 06V$ )

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The cell potential for the following cell $Pt$ \left|{H}_{2} $\left(g\right)\right|{H}^{+}\left(aq\right) | | {Cu}^{2 +}\left(0 .01 M\right)|Cu\left(s\right)$ is $0 . 576V$ at $298K$ . The $pH$ of the solution is (Nearest integer)

(Given : ${E}_{{Cu}^{2 +} / Cu}^{o} = 0 . 34V$ and $\dfrac{2 . 303RT}{F} = 0 . 06V$ )

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Correct answer: 0

Anode ⇒ H _ 2 (g) ⟶ 2 H ^ + (aq) + 2 e ^ - Cathode ⇒ Cu ^ 2 + (aq) + 2 e ^ - ⟶ Cu(s) Overall ⇒ H _ 2 (q) + Cu ^ 2 + (aq) ⟶ 2 H ^ + (aq) + Cu(s) _ ¯ E _ cell ^ ° = E _ Cu ^ 2 + Cu ^ ° - E _ H ^ + H _ 2 ^ ° = 0 . 34V E _ cell = E _ cell ^ ° - (0 . 06)/(2)log [ H ^ + ] ^ 2 [ Cu ^ 2 + ] 0 . 576 = 0 . 34 + 0 . 03[- log [ H ^ + ] ^ 2 + [ Cu ^ 2 + ]) 0 . 576 = 0 . 34 + 0 . 03[2pH + [ Cu ^ 2 + ]] 0 . 236 = 0 . 03[2pH - 2] 7 . 866 = 2pH - 2 pH = 4 . 93 5

The cell potential for the following cell Pt | H _ 2 (g)| H ^ +...

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