Can 1 M `ZnSO_(4)` be stored in a vessel made up of copper ?
Given : `E_(Zn^(2+)//Zn)^(@)=-0.76 " and "E_(Cu^(2+)//Cu)^(@)=+0.34" V"`?

Explanation

Since the standard reduction potential of Zn is less than that of copper, hence zinc metal will reduce `Cu^(+2)` ions present in aqueous solution of copper sulphate. Thus, we can not store copper sulphate solution in a vessel of zinc.
`Zn(s) + CuSO_(4)(aq) rArr ZnSO_(4)(aq) + Cu`
`E_("Redux process")^(@) = E_("Reduced pieces")^(@) - E_("Oxidised pecies")^(@)`
`=+0.34 -(-0.76) =+1.10 V`
Positive value of `E^(@)` confirms that above redux process is spontaneous and hence we cannot share copper sulphate solution in a vessel of zinc.