Increasing the pH of the solution means that the concentration of H3O+ ions hydronium ions is decreasing, as pH is inversely related to the concentration of H3O+ ions. In the given acid-base reaction:CH3COOH aq + H2O l CH3COO- aq + H3O+ aq When the pH increases, the concentration of H3O+ ions decreases. According to Le Chatelier's principle, the equilibrium will shift to counteract this change. In this case, the equilibrium will shift to the right to produce more H3O+ ions. This means that more CH3COOH will react with H2O to form CH3COO- and H3O+ ions.The equilibrium constant Ka for this reaction is given by:Ka = [CH3COO-][H3O+] / [CH3COOH]Since the equilibrium is shifting to the right, the concentration of CH3COO- and H3O+ will increase, while the concentration of CH3COOH will decrease. However, the value of the equilibrium constant Ka remains constant at a given temperature. This means that the ratio of the concentrations of the products to the reactants will still be equal to the original Ka value at the new equilibrium position.To find the new equilibrium concentrations at a given pH, you would need to know the initial concentrations of the species involved and the value of Ka for the reaction. Then, you can use an ICE Initial, Change, Equilibrium table to calculate the new equilibrium concentrations based on the change in pH.