Increasing the pH of a solution means that the concentration of hydroxide ions OH- is increasing, making the solution more basic. To understand how this affects the equilibrium position of a weak acid and its conjugate base, let's consider the following general equation for the dissociation of a weak acid HA in water:HA + H2O H3O+ + A-In this equation, HA represents the weak acid, H2O is water, H3O+ is the hydronium ion, and A- is the conjugate base of the weak acid. The equilibrium constant expression for this reaction is given by:Ka = [H3O+][A-] / [HA]Now, let's consider what happens when the pH of the solution is increased, which means the concentration of OH- ions is increased. The OH- ions will react with the H3O+ ions present in the solution, forming water:OH- + H3O+ 2H2OAs the concentration of H3O+ ions decreases due to this reaction, the equilibrium of the weak acid dissociation will shift to the right, according to Le Chatelier's principle, to counteract the decrease in H3O+ ions. This means that more of the weak acid HA will dissociate into its conjugate base A- and H3O+ ions:HA + H2O H3O+ + A- shifts to the right As a result, the concentration of the conjugate base A- will increase, and the concentration of the weak acid HA will decrease. This shift in equilibrium will continue until a new equilibrium position is established, with a higher concentration of the conjugate base A- and a lower concentration of the weak acid HA .In summary, increasing the pH of a solution i.e., increasing the concentration of OH- ions will shift the equilibrium position of a weak acid and its conjugate base to favor the formation of the conjugate base A- and the consumption of the weak acid HA .