Final answer:
The volume increase through dilution of an equilibrium solution causes the system to react by shifting to the left, as the reaction seeks to restore the equilibrium constant.
Step-by-step explanation:
When the volume of an aqueous solution at equilibrium is increased through dilution, the system reacts by shifting to the left. This is because dilution decreases the concentration of the reactants and products, and according to Le Châtelier's principle, the equilibrium will adjust to counteract the change imposed upon it. In this case, the equilibrium shifts in the direction that tends to increase the concentration of the reactants and products back to their original state, which is the reverse reaction, or to the left. This shift ensures that the ratio of the concentrations of products to reactants approaches the equilibrium constant again.
When equilibrium is achieved, the reaction quotient Qc equals the equilibrium constant Kc, and concentrations of reactants and products remain constant. If the system is disturbed, the reaction will proceed in the direction that restores the equilibrium state, adjusting concentrations to ensure that Qc again equals Kc.