Question

Given,\[AgCl\] is more soluble in aqueous sodium chloride than in pure water.
True or False

Answer 1

Hint: We need to remember that the silver chloride, \[AgCl\] is a white crystalline solid which is well known for its low solubility in water. If several salts are present in a system, they all ionize in the solution. If the salts contain a common cation or anion, these salts contribute to the concentration of the common ion. Contributions from all salts must be included in the calculation of concentration of the common ion.

Complete answer:
Silver chloride dissociates into silver and chloride ions while sodium chloride dissociates to give sodium and chloride ions.
\[AgCl \rightleftarrows A{g^ + } + C{l^ - }\]
\[NaCl \to N{a^ + } + C{l^ - }\]
Sodium chloride is a strong electrolyte and is completely dissociated. This increases the chloride ion concentration in solution and suppresses the ionization of \[AgCl\]. Hence, the solubility of \[AgCl\] decreases. Lesser the lattice energy and greater the hydration enthalpy, more is the solubility. Hydration in turn depends upon the charge to radius ratio of the ions… this ratio for sodium chloride is more than \[AgCl\] so it is more soluble.
\[AgCl\] will be more soluble in water. Presence of sodium chloride in the solution will lower the dissociation of \[AgCl\] due to common ion effect. However, Silver Chloride is more soluble in a very concentrated sodium chloride solution than in pure water. The pH of a buffer solution does not change on the addition of a small amount of an acid or a base.

Note:
As we know that there exists an electronegativity difference between Salt which gives polarity to the molecule. Thus salt is a polar molecule. As sodium chloride is a polar molecule it will be soluble in polar solvents like water. And insoluble in kerosene.