Calculate the pH at each of the following points for the titration of 100 mL of 0. 6 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide. H3His ↔ H+ + H2His- Ka1 = 3.98x10-3H2His- ↔ H+ + HHis2- Ka2 = 9.12x10-7HHis2- ↔ H+ + His3- Ka3 = 4.67x10-10 Vol. of NaOHCalculated pH0 mL 30 mL 50 mL 75 mL 100 mL 125 mL 135 mL 150 mL 175 mL Please provide a sketch of the titration curve and label both the x & y axis and applicable equations used at each data point (e.g., pH = - log[H+] or pH = pKa or pH = pKa + log )

A triprotic acid is one that can dissociate to furnish three protons by three equilibrium equations.…

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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

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

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Calculate the pH at each of the following points for the titration of 100 mL of 0. 6 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide.

H₃His ↔ H⁺ + H₂His^- Ka1 = 3.98x10^-3

H₂His^- ↔ H⁺ + HHis^2- Ka2 = 9.12x10^-7

HHis^2- ↔ H⁺ + His^3- Ka3 = 4.67x10^-10

Vol. of NaOH	Calculated pH
0 mL
30 mL
50 mL
75 mL
100 mL
125 mL
135 mL
150 mL
175 mL

Please provide a sketch of the titration curve and label both the x & y axis and applicable equations used at each data point (e.g., pH = - log[H⁺] or pH = pK_a or pH = pK_a + log )

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