The solubility of AgCl in water is affected by the common ion effect due to the presence of NaCl. The common ion effect states that the solubility of a sparingly soluble salt is decreased in the presence of a common ion.AgCl is a sparingly soluble salt that dissociates in water as follows:AgCl s Ag aq + Cl aq The solubility product constant Ksp for AgCl is 1.77 x 10 at 25C.Ksp = [Ag][Cl]When NaCl is added to the solution, it dissociates completely into Na and Cl ions:NaCl s Na aq + Cl aq Since the concentration of Cl ions increases due to the addition of NaCl, the equilibrium of AgCl shifts to the left, according to Le Chatelier's principle, to counteract the change. This results in a decrease in the solubility of AgCl.To calculate the impact of increasing the concentration of NaCl on the solubility of AgCl, let's assume we have a 0.1 M NaCl solution.The dissociation of NaCl will result in [Cl] = 0.1 M. Now, let's find the concentration of Ag ions at equilibrium:Ksp = [Ag][Cl] = [Ag] 0.1 [Ag] = Ksp / [Cl] = 1.77 x 10 / 0.1 = 1.77 x 10 MThe solubility of AgCl in pure water is approximately 1.3 x 10 M. In the presence of 0.1 M NaCl, the solubility of AgCl decreases to 1.77 x 10 M. This demonstrates that increasing the concentration of NaCl significantly reduces the solubility of AgCl in water.