The solubility of silver chloride AgCl in water is affected by the presence of other ions in the solution, such as sodium chloride NaCl . This phenomenon can be explained using the common ion effect, which states that the solubility of a sparingly soluble salt decreases in the presence of a common ion.Silver chloride has low solubility in water and dissociates into silver ions Ag and chloride ions Cl according to the following equilibrium reaction:AgCl s Ag aq + Cl aq The solubility product constant Ksp for this reaction is given by:Ksp = [Ag][Cl]When sodium chloride is added to the solution, it dissociates completely into sodium ions Na and chloride ions Cl :NaCl s Na aq + Cl aq As the concentration of sodium chloride increases, the concentration of chloride ions in the solution also increases. According to Le Chatelier's principle, the equilibrium will shift to counteract this change, in this case by shifting the AgCl equilibrium to the left favoring the formation of solid AgCl . This results in a decrease in the solubility of silver chloride.To illustrate this effect, we can perform calculations using the solubility product constant for silver chloride Ksp = 1.77 x 10 and the concentration of sodium chloride.Let's assume the initial concentration of sodium chloride is 0.1 M. The equilibrium concentrations of Ag and Cl ions can be represented as:[Ag] = x[Cl] = 0.1 + xSince Ksp = [Ag][Cl], we can substitute the equilibrium concentrations:1.77 x 10 = x 0.1 + x Solving for x, we find that x 1.76 x 10 M, which represents the solubility of AgCl in the presence of 0.1 M NaCl.Now, let's increase the concentration of sodium chloride to 0.5 M and repeat the calculation:[Ag] = x[Cl] = 0.5 + x1.77 x 10 = x 0.5 + x Solving for x, we find that x 3.53 x 10 M, which represents the solubility of AgCl in the presence of 0.5 M NaCl.As the calculations show, the solubility of silver chloride decreases as the concentration of sodium chloride increases.To represent this graphically, we can plot the solubility of AgCl y-axis against the concentration of NaCl x-axis . The graph will show a downward trend, indicating that the solubility of AgCl decreases as the concentration of NaCl increases.