Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal ? Given that `E_(Ni^(-2)//Ni)=-0.25 ` volt and `E_(Cu^(-2)//Cu)^(@) =+0.34` volt

Explanation

In this problem we want to see whether the following reaction takes place or not ltbnr?gt `Ni+CuSO_(4) rarr NiSO_(4)+Cu, i.e NiCu^(2+) rarr Ni^(2+)+Cu`
By conventin the cell may be represented as `NiNi^(2+)||Cu^(2+)|Cu`
We given oxidation potential as `E_(Ni,Ni^(2))^(@)=+0.25` volt and `E_(Cu,Cu^(2))^(@)=-0.34` volt
Henc by reversing the sign of oixdation potential the reducitn potential s will
Thus EMF comes out to be positive this imlies that `CuSO_(4)` reacts with nickel hence `CuSO_(4)` solution connot be stroed in a nickel vessel
Alternatively since `E_(Ni^(2+),Ni)=-0.25` V is lower than `E_(Cu^(2+),Cu)^(@)=+0.34` V therefore Ni can easily lose electrons to `Cu^(2+)` ions in other words the following rection `Ni+Cu^(2+)rarrNi^(2+)+Cu`
Will occur thus `CuSO_(4)` solution cannot be stored in a nickel vessel