Increasing the temperature generally increases the ionization constant Ka of weak acids, such as acetic acid CH3COOH . This is because the ionization of weak acids is an endothermic process, meaning it absorbs heat. When the temperature increases, the equilibrium shifts towards the ionized form CH3COO- and H+ to absorb the excess heat, according to Le Chatelier's principle.As the Ka value increases, the ionization of acetic acid increases, leading to a higher concentration of H+ ions in the solution. This, in turn, affects the pH of the solution. The pH of a solution is calculated using the formula:pH = -log10[H+]Since the concentration of H+ ions increases with the increase in Ka, the pH of the solution will decrease, making the solution more acidic.However, without specific temperature values, it is not possible to provide an exact numerical change in the Ka value or the pH of the 0.1 M acetic acid solution.