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  • The cell potential for the following cell <img alt="\mathrm{Pt\left | H_{2}\left ( g \right )H^{+}(aq) \right |\left | Cu^{2+}\left ( 0.01\, M \right ) \right |Cu(s)}" src="https://entran

The cell potential for the following cell

\mathrm{Pt\left | H_{2}\left ( g \right )H^{+}(aq) \right |\left | Cu^{2+}\left ( 0.01\, M \right ) \right |Cu(s)}

is \mathrm{0.576\, V\: at\; 298\: K.} The \mathrm{pH} of the solution is _________ (Nearest integer)

(Given : \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{~V}$ and $\frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06 \mathrm{~V})
 

Option: 1

5


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

The cell reaction is

\mathrm{H}_{2}+\mathrm{Cu}^{2+} \longrightarrow 2 \mathrm{H^{+}}+\mathrm{Cu}

\mathrm{Now, E^{0}=0. 34-0=0.34 \mathrm{~V}}

Applying Nernst equation, we get

\mathrm{ E=E^{0}-\frac{0.06}{2} \, \log \, \frac{\left[H^{+}\right]^{2}}{0.01}}

\mathrm{ \Rightarrow 0.576=0. 34-0. 06\, \log \{10[H^{+}]\} }

\mathrm{ \Rightarrow 0.236 =0.06\{\mathrm{pH}-1\}}

\mathrm{ \Rightarrow \quad \mathrm{pH} =4. 93 \simeq 5 }

Hence, the answer is 5

Posted by

Divya Prakash Singh

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