A 100.0 mL solution containing 0.877 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.256 M KOH. Calculate the pH of the solution after the addition of 59.0 mL of the KOH solution. Maleic acid has pKa 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. [M²-] = M %3D [HM-] = M [H,M] = 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.