Answer: The equilibrium will shift to the right and the concentration of Ag+ (aq) will decrease, and the amount of AgCl(s) will increase.
Explanation: In the equilibrium equation AgCl(s) <--> Ag^+(aq) + Cl^-(aq) represents a system where AgCl is in equilibrium with its dissociated ions Ag+ and Cl- in aqueous solution. The equilibrium is established by the forward and reverse reactions, AgCl(s) dissociating into Ag+(aq) and Cl-(aq) and Ag+(aq) and Cl-(aq) recombining to form AgCl(s).
When the concentration of Cl- (aq) is increased, the equilibrium system will shift to the right to consume some of the added Cl-. This is known as Le Chatelier's principle, which states that if a stress is applied to a system at equilibrium, the system will shift in the direction that will tend to relieve that stress. In this case, the added Cl- ions will react with the Ag+ ions to form more AgCl(s) and decrease the concentration of Ag+ ions.
It's important to note that the other options provided are not related to the reaction given and are not accurate.