A 100.0 ml. solution containing 0.794 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.228 M KOH. Calculate the pH of the solution after the addition of 60.0 mL of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H, M, HM", and M2-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. (M) (HM"] = M

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.