Consider the equilibrium that is established in a saturated solution of silver c

Question

Consider the equilibrium that is established in a saturated solution of silver chloride, Ag+(aq) + Cl(aq) AgCl(s). If solid AgCl is added to this solution what will happen to the concentration of Ag+ and Cl ions in solution?

Consider the equilibrium that is established in a saturated solution of silver chloride, . If solid  is added to this solution what will happen to the concentration of  and  ions in solution?

[Ag+] will increase and [Cl] will decrease [Ag+] and [Cl] will both increase [Ag+] will decrease and [Cl] will increase [Ag+] and [Cl] will both decrease neither [Ag+] nor [Cl] will change

Explanation / Answer

neither [Ag+] nor [Cl-] will change

Since the solution is already saturated. No more ions can be formed since
Ksp = [Ag+] [Cl-] is constant

le chatellier's priciple would have worked if the solution was not saturated

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