A zinc electrode is dipped in a 0.1 M solution at $25^{0} C$ . Assuming that salt is dissociated to 20% at this dilution. Calculate the electrode potential. $E {^{0}}_{Z n^{2 +} / Z n} = - 0.76 V$ .

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The emf of a concentration cell consisting of two zinc electrode, one dipping into M/4 solution of zinc sulphate and the other into M/16 solution of the same salt at 250C :

The correct option is C 0.0178 VFor the given cell, the standard cell potential, E0cell=0.0V.The emf of the cell is Ecell=E0cell−0.05922log (M16)(M4)=0.0V+0.0296 log4=0.0178V.Option C is correct.

The emf of a concentration cell consisting of two zinc electrode, one dipping into M/4 solution of zinc sulphate and the other into M/16 solution of the same salt at 25 $^{0}$ C :

The correct option is C 0.0178 V
For the given cell, the standard cell potential, $E_{c e l l}^{0} = 0.0 V .$
The emf of the cell is $E_{c e l l} = E_{c e l l}^{0} - \frac{0.0592}{2} l o g \frac{(\frac{M}{16})}{(\frac{M}{4})} = 0.0 V + 0.0296 l o g 4 = 0.0178 V .$

Option C is correct.