You are provided with two containers made of copper and aluminium. You are also provided with solutions of dilute $HCl$,dilute $HNO_{3}$,$ZnCl_{2}$,and $H_{2}O$. In which of the above containers can these solutions be kept?

(A-D) When solutions are kept in a copper container:
$(a)$ Dilute $HCl$: Copper does not react with dilute $HCl$,so it can be kept.
$(b)$ Dilute $HNO_{3}$: Nitric acid is a strong oxidizing agent and reacts with copper,so it cannot be kept.
$(c)$ $ZnCl_{2}$: Zinc is more reactive than copper,so no displacement reaction occurs; it can be kept.
$(d)$ $H_{2}O$: Copper does not react with water,so it can be kept.
$(B)$ When solutions are kept in an aluminium container:
$(a)$ Dilute $HCl$: Aluminium reacts with dilute $HCl$ to form $AlCl_{3}$ and $H_{2}$ gas,so it cannot be kept. Reaction: $2Al + 6HCl \rightarrow 2AlCl_{3} + 3H_{2}$.
$(b)$ Dilute $HNO_{3}$: Aluminium forms a protective oxide layer $(Al_{2}O_{3})$ with dilute $HNO_{3}$,which prevents further reaction,so it can be kept.
$(c)$ $ZnCl_{2}$: Aluminium is more reactive than zinc and will displace zinc from the solution,so it cannot be kept. Reaction: $2Al + 3ZnCl_{2} \rightarrow 2AlCl_{3} + 3Zn$.
$(d)$ $H_{2}O$: Aluminium does not react with cold or hot water,so it can be kept.