## Question

###### A 100.0 mL solution containing 0.852 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.852 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.277 M KOH. Calculate the pH of the solution after the addition of 53.0 mL of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH = -.57 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?-1 = 3.72 [HM") = 3.75 [H,M] = 7.32

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