A 100.0 mL solution containing 0.976 g of maleic acid (MW =116.072 g/mol) is titrated with 0.296 M KOH. Calculate the pH ofthe solution after the addition of 56.00 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 maleicacid in the solution at equilibrium. The three forms of maleic acidare abbreviated H2M, HM–, and M2–, which represent the fullyprotonated, intermediate, and fully deprotonated forms,respectively.
[M2-] = ___ M
[HM-] = ___ M
[H2M] = ___ M
