**Titration of Maleic Acid with KOH**A 100.0 mL solution containing 0.877 g of maleic acid (Molecular Weight = 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 $ pK_a $ values of 1.92 and 6.27.**pH Calculation:**pH = [Input box for pH]**Equilibrium Concentrations of Maleic Acid Forms**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 $ \text{H}_2\text{M}, \text{HM}^-, $ and $\text{M}^{2-}$, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.\[[\text{M}^{2-}] = \text{[Input box]} \, \text{M}\]\[[\text{HM}^-] = \text{[Input box]} \, \text{M}\]\[[\text{H}_2\text{M}] = \text{[Input box]} \, \text{M}\]**Instructions**1. Complete the calculations for pH after the titration.2. Calculate the equilibrium concentrations of each form of maleic acid using the provided $ pK_a $ values and the calculated pH.This exercise enables students to understand the relationship between acid-base titrations, pH, and the equilibrium concentrations of the different forms of a diprotic acid.

The explanation is given below-

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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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