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A 100.0 mL solution containing 0.756 g of maleic acid (MW = 116.072 g/mol) is titrated...

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Chemistry

A 100.0 mL solution containing 0.756 g of maleic acid (MW =116.072 g/mol) is titrated with 0.217 M KOH. Calculate the pH ofthe solution after the addition of 60.0 mL of the KOH solution.Maleic acid has pKa values of 1.92 and 6.27.

At this pH (pH = 9.48), calculate the concentration of each formof maleic acid in the solution at equilibrium. The three forms ofmaleic acid are abbreviated H2M, HM–, and M2–, which represent thefully protonated, intermediate, and fully deprotonated forms,respectively.

Answer & Explanation Solved by verified expert
3.7 Ratings (371 Votes)
Mass of maleic acid 0756 g Moles of maleic acid 0756 116072 651 x 103 moles Conc of KOH solution 0217 M Volume of KOH solution 60 mL 0060 L Moles of KOH added 0217 x 0060 001302 moles The    See Answer
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