The solubility of AgCl will be maximum in which of the following?

<p>The solubility of AgCl will be maximum in deionized water.</p> <p>Silver chloride (AgCl) is a sparingly soluble salt. Its solubility in water can be represented by the equilibrium:</p> <p>$\text{AgCl (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^- (aq)$</p> <p>In the presence of a common ion, the solubility of AgCl decreases due to the common ion effect, which is explained by Le Chatelier's Principle. Here's an analysis of each option:</p> <p><p><strong>Option A: 0.01 M KCl</strong> </p> <p>The presence of additional chloride ions ($\text{Cl}^-$) from KCl will shift the equilibrium to the left, reducing the solubility of AgCl.</p></p> <p><p><strong>Option B: 0.01 M HCl</strong> </p> <p>Similar to KCl, HCl also provides more chloride ions, which will decrease the solubility of AgCl due to the common ion effect.</p></p> <p><p><strong>Option C: 0.01 M AgNO$_3$</strong> </p> <p>AgNO$_3$ introduces additional silver ions ($\text{Ag}^+$) into the solution, also shifting the equilibrium to the left, hence decreasing the solubility of AgCl.</p></p> <p><p><strong>Option D: Deionized water</strong> </p> <p>This option does not introduce additional ions that impact the equilibrium, so there are no additional silver or chloride ions to shift the equilibrium. As a result, the solubility of AgCl will be highest in deionized water, as there is no common ion effect.</p></p> <p>Therefore, the solubility of AgCl is highest in deionized water.</p>