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If E° of calomel electrode ClHg2Cl2Pt is 0.27V its potential when KCl=0.1M would be 

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a
0.25 V
b
0.26V
c
0.276 V
d
0.286 V

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detailed solution

Correct option is C

The reaction is 12Hg2Cl2(s)+eHg(l)+Cl(aq) 

Hence, E=ERTElnCl/c=0.27V(0.059V)log(0.1)=0.2759V

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