The solubility of AgCl in a NaCl solution can be explained using the solubility product constant Ksp and Le Chatelier's principle. First, let's consider the solubility equilibrium of AgCl:AgCl s Ag+ aq + Cl- aq The solubility product constant Ksp for this reaction is given by:Ksp = [Ag+] [Cl-]Now, let's consider the effect of changing the concentration of NaCl solution. When NaCl is dissolved in water, it dissociates into Na+ and Cl- ions:NaCl s Na+ aq + Cl- aq As the concentration of NaCl increases, the concentration of Cl- ions in the solution also increases. According to Le Chatelier's principle, when a change is made to a system in equilibrium, the system will adjust to counteract that change and re-establish equilibrium. In this case, the increase in Cl- ion concentration will shift the equilibrium of the AgCl solubility reaction to the left, favoring the formation of solid AgCl and decreasing its solubility in the solution.This can also be explained using the solubility product constant Ksp . Since Ksp is a constant value for a given temperature, if the concentration of Cl- ions increases, the concentration of Ag+ ions must decrease to maintain the constant Ksp value. As a result, the solubility of AgCl decreases.In conclusion, increasing the concentration of NaCl solution will decrease the solubility of AgCl due to the increase in Cl- ion concentration, which shifts the AgCl solubility equilibrium to the left, favoring the formation of solid AgCl. This is supported by both Le Chatelier's principle and the solubility product constant Ksp .