A 100.0 mL 100.0 mL solution containing 0.960 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.295 M KOH. Calculate the pH of the solution after the addition of 56.0 mL 56.0 mL of the KOH KOH solution. Maleic acid has p K a pKa values of 1.92 and 6.27. pH = 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 , H2M, , HM−, and M 2 − , which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. [M2−]= M [HM−]= M [H2M]=