Is it possible to store:
(i) Copper sulphate solution in a zinc vessel?
(ii) Copper sulphate solution in a silver vessel?
(iii) Copper sulphate solution in a gold vessel?
Given: `E_(Cu^(2+)| Cu )^(0)` = + 0.34 volt and `E_(Ag^(2+)| Ag )^(0)` = 0.80 volt and `E_(Au^(2+)| Au )^(0)` = +1.50 volt

Explanation

(i) We cannot `SuSO_(4)` soluton in a zinc vessel if the following redox reaction occurs
`Zn+CuSO_(4)rarrZnSO_(4)+Cu` or `Zn+Cu^(2+)rarrZn^(2+)+Cu`
By convention the cell may be represented as `Zn|Zn^(2+)||Cu^(2+)|Cu`
By convention the cell of the above redox reaction may be represented as
`Ag|Ag^(+)||Cu^(2+)|Cu` and `E_(cell)^(@)=E_(Cu^(2+),Cu)^(@)-E_(Ag^(+),Ag)^(@)=0.34-0.80 =-0.56 V`
since the EMF of the cell is -ve therefore `CuSO_(4)` does not react with silver in other wods `CuSO_(4)` solution can be stroed in a silver vessel
(iii) we cannot stroe `CuSO_(4)` solution in a gold vessel if the following redox reaction occurs
`2 Au+3Cu^(2+) rarr2 Au^(3+)+3Cu`
The cell corresponding to the above redox reaction may be represented as
`Au|Au^(3+)||Cu^(2)|Cu` and `E_(Cu^(2+),Cu)^(@)-E_(Au^(3+),Au)^(@)=0.34 -1.50 =-1.26 V`
since the EMF of the above cell reaction is -ve therefore `CuSO_(4)` solution does not react with gold in other words `CuSO_(4)` solutoin can be stored in a gold vessel