Question

For a beaker containing the reaction below that is at equilibrium, using LeChatelier's principle, predict which way the equilibrium conditions will shift if silver chloride was added to a beaker.

AgNO₃(aq) + NaCl(aq) AgCl (s) + NaNO₃(aq)
a. left
b. right
c. no change

Answer 1

Adding silver chloride to the reaction at equilibrium will cause the equilibrium to shift to the left, according to Le Chatelier's principle, in order to consume some of the added AgCl and restore equilibrium.

Step-by-step explanation:

According to Le Chatelier's principle, the equilibrium of a reaction will shift to counteract any change in conditions. When silver chloride (AgCl) is added to the equilibrium reaction AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq), more Ag+ and Cl− ions are introduced into the system.

Since silver chloride is a product of the presented reaction, adding more will effectively increase the concentration of one of the products. This perturbation will cause the equilibrium to shift to the left to consume some of the added AgCl by forming more AgNO₃(aq) and NaCl(aq) and thus reduce the disturbance.