Final answer:
Adding solid AgCl to a saturated solution of silver chloride will not change the concentration of Ag+ and Cl– ions due to the solubility equilibrium. The system is governed by Le Chatelier's principle, ensuring the concentrations of the ions in a saturated solution remain constant despite the addition of more solid.
Step-by-step explanation:
When solid AgCl is added to a saturated solution of silver chloride, the concentration of Ag+ and Cl– ions in solution will not change because the solution is already at equilibrium. This scenario is dictated by Le Chatelier's principle, which states that if a system at equilibrium is disturbed, the system will adjust itself to diminish the change. Adding more AgCl solid does not increase the ions in solution because the solubility equilibrium between the dissolved ions and the solid AgCl has already been established.
The equilibrium can be represented by the following equation:
AgCl(s) ⇌ Ag+ (aq) + Cl– (aq)
This equation indicates that solid silver chloride is in a dynamic equilibrium with its ions in solution. Any excess of solid AgCl will simply remain undissolved until more ions are needed to maintain equilibrium, for instance if some of the aqueous Ag+ or Cl– ions were removed.
Therefore, adding more solid AgCl will not increase the concentration of the ions due to the precipitation of AgCl from the aqueous ions at the same rate as its dissolution into ions.