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A 100.0 mL solution containing 0.753 g of maleic acid (MW = 116.072 g/mol) is titrated...

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Chemistry

A 100.0 mL solution containing 0.753 g of maleic acid (MW =116.072 g/mol) is titrated with 0.259 M KOH. Calculate the pH ofthe solution after the addition of 50.0 mL of the KOH solution.Maleic acid has pKa values of 1.92 and 6.27.

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.

Answer & Explanation Solved by verified expert
4.0 Ratings (823 Votes)
Maleic acid molecular weight MW 116072 Mass of maleic acid used 0753 g Number of moles of maleic acid massMW 0753 116072 00064873 moles Molarity of maleic acid molesV 0006487301 0064873 M Molarity of KOH M 0259 M Volume of KOH used V 50 mL mmoles of KOH used MV 0259 x 50 1295mmoles 001295 moles of KOH used At equilibrium H2M OH HM H2OpKa1 192 HM OH M2 H2O pKa2 627 For    See Answer
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