Answer:
A solution of an electrolyte can be
stored in a particular vessel only in case there is no chemical reaction taking
place with the material of the
vessel.
Now if silver nitrate solution is to be
kept in copper vessel, the probable reaction will be:
\[Cu(s)+2A{{g}^{+}}(aq)\xrightarrow{\,}\,C{{u}^{2+}}(aq)+2Ag(s)\]
Since copper is placed below
silver in the activity series, this means that it is a stronger reducing agent
and can lose electrons to \[A{{g}^{+}}\] ions and the chemical reaction will
occur. Therefore, silver nitrate is a stronger reducing agent and solution
cannot be kept in copper vessel. Now, when copper sulphate solution is placed
in silver vessel, the likely chemical reaction is:
\[2Ag(s)+C{{u}^{2+}}(aq)\xrightarrow{\,}\,Cu(s)+2A{{g}^{+}}(aq)\]
Since Ag is placed above copper
in the activity series, the chemical reaction will not take place. As a result,
copper sulphate can be easily stored in silver vessel.
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