To calculate the equilibrium constant K for the reaction of acetic acid in aqueous solution, we first need to find the concentration of hydrogen ions [H] and acetate ions [CHCOO] at equilibrium. The reaction of acetic acid CHCOOH in water can be represented as:CHCOOH + HO CHCOO + HOGiven the pH of the solution is 4.76, we can calculate the concentration of hydrogen ions [H] using the formula:pH = -log[H]4.76 = -log[H][H] = 10^-4.76 1.74 x 10^-5 MSince acetic acid is a weak acid, we can assume that the concentration of hydrogen ions [H] is equal to the concentration of acetate ions [CHCOO] at equilibrium. Therefore:[CHCOO] = [H] 1.74 x 10^-5 MNow, we can use the initial concentration of acetic acid 0.1 M to find the concentration of acetic acid at equilibrium:[CHCOOH] = Initial concentration - [CHCOO] = 0.1 - 1.74 x 10^-5 0.1 MFinally, we can calculate the equilibrium constant K using the formula:K = [CHCOO][H] / [CHCOOH]K = 1.74 x 10^-5 1.74 x 10^-5 / 0.1 3.0 x 10^-5 The equilibrium constant K for the reaction of acetic acid in aqueous solution is approximately 3.0 x 10^-5 .