`0.1` M copper sulphate solution in which copper electrode is dipped at `25^(@) C` . Calculate the electrode potential of copper .
`["Given ," E_(Cu^(2+)//Cu)^(0) = 0.34 V`].

Explanation

Given that
`[Cu^(2+)] = 0.1 M`
`E_(Cu^(2+)|Cu)^(0) = 0.34`
` E_("cell") `= ?
Cell reaction is
`Cu^(2+)(aq) + 2e^(-) to Cu(s)`
`E_("cell") = E^(0) - (0.0591)/n log . ([Cu])/([Cu^(2+)]) `
` = 0.34 - 0.0296`
` = 0.31 V`