The single electrode potential of $0.1 M$ solution of $M^{+} / M$ ion is:
( $E^{o} = 2.36 V$ )

2.42 V

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2.30 V

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0.236 V

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0.230 V

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Solution

The correct option is C $2.30 V$
$E_{c e l l} = E_{c e l l}^{\circ} - \frac{0.059}{n} l o g (\frac{1}{M^{+}})$
Reaction:
$M^{+} + e^{-} \to M$
Now,
$∴ E_{c e l l} = 2.36 - \frac{0.059}{1} l o g (\frac{1}{0.1})$
$E_{c e l l} = 2.30 V$

Hence, the correct option is $B$ .

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Similar questions

The single electrode potential of metal $E$ of $0.1$ M solution of M $^{+} / M$ ions [ $E$ $^{0}$ $= - 2.36 V$ ] is nearly:

E

0.1

M^{+}

(E_{k p}^{o} = - 2.36 V)

0.1

M^{+} i o n s : (E_{R P} = - 2.36 V)

The name of equation showing relation between electrode potential (E)

standard electrode potential and concentration of ions in solution is

Z n S O_{4}

25^{o} C ? [E^{o} = 0.763 V]

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