Question

Can you store copper sulphate solutions in a zinc pot?

Answer 1

Hint: The term related to this question is the standard reduction potential. If you can figure out how it can affect the reactivity of both of them.

Complete step by step answer:

The standard reduction potential is the reduction potential of a molecule under specific, standard conditions.
Standard reduction potentials can be useful in determining the directionality of a reaction. The reduction potential of a given species can be considered to be the negative of the oxidation potential.
The ${ E }^{ 0 }$ values of the copper and zinc electrodes are as follows :

${ Zn }^{ 2+ }(aq)+2{ e }^{ - }\quad \rightarrow \quad Zn(s),\quad { E }^{ 0 }=−0.76V$

${ Cu }^{ 2+ }(aq)+2{ e }^{ - }\quad \rightarrow \quad Cu(s),\quad { E }^{ 0 }=−0.34V$

This shows that zinc is a stronger reducing agent than copper. It will lose electrons to
${ Cu }^{ 2+ }$ ions and a redox reaction will immediately set in.

Copper is less reactive than zinc. Zinc will replace the copper from its salt solution. When the copper sulphate solution is stored in a zinc pot, copper is replaced by zinc, in the copper sulphate solution.
$Zn\quad +\quad { CuSO }_{ 4 }\quad \rightarrow\quad { ZnSO }_{ 4 }\quad +\quad Cu$
So copper sulphate solution cannot be stored in a zinc pot.

Note: Sometimes, the direction of a redox reaction can be determined by estimating the relative strengths of the reductants and oxidants.
In situations where an electrochemical series is not sufficient to absolutely determine the direction of a redox reaction, the standard electrode potential, ${ E }^{ 0 }$, can be used.
A negative value of cell potential indicates a reducing environment, while a positive value indicates an oxidizing environment.