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Q.

A current of 9.65 ampere is passed through 0.2 M,500 mL aqueous solution of CuSO₄ using Cu-electrode for 300 sec. than calculate [Cu²⁺] concentration in the resulting solution. If volume of solution remains constant:

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a

1 M

b

1.96 M

c

1.35 M

d

0.2 M

answer is D.

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Detailed Solution

$\begin{array}{l} E^{\circ} oxidation Cu |{Cu}^{2 +} > E^{\circ} H_{2} O| O_{2} \\ E_{R}^{\circ} {Cu}^{2 +} |Cu > E_{R}^{\circ} H_{2} O| H_{2} \end{array}$
So equivalent of Cu oxidised at anode = equivalent Cu²⁺ reduced at cathode. So [Cu²⁺] = constant

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