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 the concentration of sodium chloride is increased.

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

Answer 1

Increasing the concentration of sodium chloride in the reaction AgNO₃(aq) + NaCl(aq) -> AgCl (s) + NaNO₃(aq) will cause the equilibrium conditions to shift to the right.

Step-by-step explanation:

According to Le Chatelier's principle, if the concentration of sodium chloride in the reaction AgNO₃(aq) + NaCl(aq) -> AgCl (s) + NaNO₃(aq) is increased, the equilibrium conditions will shift to the right.

This means that more products, AgCl and NaNO₃, will be formed and the concentration of the reactants, AgNO₃ and NaCl, will decrease. Increasing the concentration of sodium chloride causes the system to shift in the direction that opposes the increase in concentration.