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E^(@) values of Ni^(2+), Ni and Cl(2), ...

`E^(@)` values of `Ni^(2+)`, Ni and `Cl_(2), Cl^(-)` are respectively `-0.25V` and `+1.37V`. Calculate the EMF of the cell `Ni, Ni^(2+) (0.01M)//Cl^(-)(0.1M), Cl_(2)`, pt. Potential of nickel electrode is given as,

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`E =E^(@) + 0.0295 log [Ni^(2+)]= -0.25+0.0295log 10^(-2)`
`= -0.25 + 0.0295(-2) = -0.305 V`
Potential of chlorine electrode is given as,
`E =E^(@)-0.059log [Cl^(-)]=+1.37-0.059log 10^(-1) = 1.43V`
EMF of cell `=1.43-(-0.305) = 1.735` V.
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