Can you store copper sulphate solutions in a zinc pot?

Explanation

Zinc is more reactive than copper. Hence, it displaces copper sulphate solution as follows:
`Zn(s)+CuSO_(4)(aq) to ZnSO_(4)(aq)+Cu(s)`
Thus, zinc reacts with `CuSO_(4)` solution. Hence, we cannot store copper sulphate solution in a zinc pot.
Alternatively, `E_(Zn^(2+)//Zn)^(@)=-0.76V,E_(Cu^(2+)//Cu)^(@)=0.34V`
To check whether zinc reacts with `CuSO_(4)` solution i.e., whether the following reaction takes place or
not `Zn(s)+CuSO_(4)(aq) to ZnSO_(4)(aq)+Cu(s)`
Find the EMF of this cell reaction. the cell may be represented as:
> `Zn|Zn^(2+)||Cu^(2+)|Cu`
`E_(cell)^(@)=E^(@)(Cu^(2+)//Cu)-E^(@)(Zn^(2+)//Zn)`
`=0.34V-(-0.76V)=1.10V`
As `E_("cell")^(@)` is positive the reaction in the forward direction is spontaneous and as such we cannot store `CuSO_(4)` in zinc pot.