Can you store `CuSO_(4)` solution in `Zn` pot ?

Explanation

No, it is not possible. The `E^(@)` values of the copper and zinc electrodes are as follows :
`Zn^(2+)(aq)+2e^(-)toZn(s) , E^(@)=-0.76" V"`
`Cu^(2+)(aq)+2e^(-) to Cu(s) , E^(@)=-0.34" V"`
This shows that zinc is a stronger reducing agent than copper. It will lose electrons to `Cu^(2+)` ions and redox reaction will immediately set in.
`Zn(s)+Cu^(2+)(aq)toZn^(2+)(aq)+Cu(s)`
Thus, copper sulphate solution cannot be stored in zinc pot.