Nov 21, 2014 · Glacial acetic acid is pure acetic acid, not mixed with water. The smell of glacial acetic acid is much stronger than that of dilute acetic acid. Other than the greater intensity, the smell is ... Acetic acid with a molar concentration of 0.1 M has a pH of 2.87, and 0.0001 M of acetic acid has a pH of 4.3. As the molar concentration of acetic acid in a solution decreases, the pH increases, which indicates that it is a weaker acetic acid than those that have higher molar concentrations. Now acetic acid is a weak acid and weak acids don't donate protons very well. So acetic acid is gonna stay mostly protonated. When you think about this reaction coming to an equilibrium, you're gonna have a relatively high concentration of your reactants here. Introduction Vinegar is a common household item containing acetic acid as well as some other chemicals. This experiment is designed to determine the molar concentration of acetic acid in a sample of vinegar by titrating it with a standard solution of NaOH. CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l) By adding the sodium hydroxide, which… Calculate the K a of a weak acid given the pH and molarity. Return to the Acid Base menu. Return to a listing of many types of acid base problems and their solutions. Calculate K a from pH and Other Concentration Data (not molarity) Calculate K b from pH and Molarity An acid dissociation constant, K a, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction ↽ − − ⇀ − + + known as dissociation in the context of acid–base reactions.