The reaction between acetic acid CHCOOH and sodium acetate CHCOONa can be represented as follows:CHCOOH + HO CHCOO + HOThis is a weak acid acetic acid and its conjugate base acetate ion system, which acts as a buffer solution. The equilibrium constant for this reaction is given by the acid dissociation constant Ka of acetic acid:Ka = [CHCOO][HO] / [CHCOOH]Now, let's consider the effect of increasing the pH on this equilibrium. Increasing the pH means decreasing the concentration of HO ions in the solution. According to Le Chatelier's principle, when a change is applied to a system in equilibrium, the system will adjust itself to counteract the change.In this case, when the concentration of HO ions decreases, the equilibrium will shift to the right to produce more HO ions. This means that more acetic acid will dissociate into acetate ions and HO ions, and the concentration of acetate ions will increase.Mathematically, we can use the Henderson-Hasselbalch equation to describe the relationship between pH, pKa, and the concentrations of the weak acid and its conjugate base:pH = pKa + log [CHCOO] / [CHCOOH] As the pH increases, the ratio of [CHCOO] to [CHCOOH] must also increase to maintain the equilibrium. This means that the concentration of acetate ions will increase, and the concentration of acetic acid will decrease.In conclusion, increasing the pH of the reaction between acetic acid and sodium acetate will shift the equilibrium position to the right, resulting in an increase in the concentration of acetate ions and a decrease in the concentration of acetic acid.