The solubility product of AgCl is 2.0 x 10^-10 mol-2 dm-6. The maximum concentration of Ag+1 ions in the solution is:

Explanation

To find the maximum concentration of Ag+ ions in a solution of AgCl, we consider the dissolution process: AgCl(s) → Ag+(aq) + Cl-(aq). The solubility product expression is given by Ksp = [Ag+][Cl-]. Since the stoichiometry indicates that one mole of AgCl produces one mole of Ag+ and one mole of Cl-, we can denote their concentrations as [Ag+] = [Cl-] = s, where 's' represents solubility in mol dm-3. Thus, Ksp = s². Given Ksp = 2.0 x 10-10 mol2 dm-6, we can solve for 's': s² = 2.0 x 10-10, leading to s = √(2.0 x 10-10) ≈ 1.41 x 10-5 mol dm-3, which represents the maximum concentration of Ag+ ions.The other options are incorrect because they either stem from miscalculations or a misunderstanding of how to apply the Ksp expression and stoichiometry involved in the dissolution of AgCl.