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

Explanation

Given that
`[Cu^(2+)]=01M`
`E_(Cu^(2+)"|"Cu)^(@)=0.34`
`E_("cell")=?`
Cell reaction is `Cu^(2+)(aq)+2e^(-) to Cu(s)`
`E_("cell")=E^(@)-(0.0591)/(n)"log"([Cu])/([Cu^(2+)])=0.34-(0.0591)/(2)"log"(1)/(0.1)`
`=0.34-0.0296=0.31V`