If the $0.05$ molar solution of $M^{+}$ is replaced by a $0.0025$ molar $M^{+}$ solution, then the magnitude of the cell potential would be__________.

35 m V

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70 m V

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140 m V

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700 m V

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Solution

The correct option is D $140 m V$
$E_{c e l l}^{\circ} = 0$ , for every concentration cell
$E = 0 - \frac{0.059}{n} log \frac{[M^{+}]_{a n o d e}}{[M^{+}]_{c a t h o d e}}$
$= - \frac{0.059}{1} log [0.0025]$
$= + 153 m V$
It is close to $140 m V$ .

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Similar questions

Q. If the 0.05 molar solution of

M^{+}

is replaced by 0.0025 molar

M^{+}

solution, then the magnitude of the cell potential would be:

Q. If the 0.05 M solution of M

^{+}

is replaced by a 0.0025 M solution of M

^{+}

, then the magnitude of the cell potential would be:

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is:
$M (s) | M^{+} (a q; 0.05 m o l a r) | | M^{+} (a q; 1 m o l a r) | M (s)$
For the above electrolytic cell the magnitude of the cell potential $| E_{c e l l} | = 70 m V$ .

If the 0.05 molar solution of $M^{+}$ is replaced by a 0.0025 molar $M^{+}$ solution, then the magnitude of the cell potential would be

100 {cm}^{3}

of a 0.1 M

H C l

solution is mixed with

100 {cm}^{3}

of a 0.2 N

N a O H

solution. The concentration of excess reagent left and the nature of resulting solution is:

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is:
$M (s) | M^{+}$ (aq;0.05 molar)|| $M^{+}$ (aq;1 molar)|M(s)
For the above electrolytic cell the magnitude of the cell potential $| E_{c e l l} | = 70 m V$ .

For the above cell

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If the 0.05 molar solution of M+ is replaced by a 0.0025 molar M+ solution, then the magnitude of the cell potential would be__________.

The correct option is D 140 mVE∘cell=0, for every concentration cellE=0−0.059nlog[M+]anode[M+]cathode=−0.0591log[0.0025]=+153 mVIt is close to 140 mV.

If the $0.05$ molar solution of $M^{+}$ is replaced by a $0.0025$ molar $M^{+}$ solution, then the magnitude of the cell potential would be__________.

The correct option is D $140 m V$
$E_{c e l l}^{\circ} = 0$ , for every concentration cell
$E = 0 - \frac{0.059}{n} log \frac{[M^{+}]_{a n o d e}}{[M^{+}]_{c a t h o d e}}$
$= - \frac{0.059}{1} log [0.0025]$
$= + 153 m V$
It is close to $140 m V$ .