Calculate the pH at each of the following points for the titration of 200 mL of 0. 45 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide. H3His ↔ H+ + H2His- Ka1 = 3.98x10-3 H2His- ↔ H+ + HHis2- Ka2 = 9.12x10-7 HHis2- ↔ H+ + His3- Ka3 = 4.67x10-10 Vol. of NaOH Calculated pH 0 mL 37.5 mL 50 mL 75 mL 100 mL 150 mL 200 mL 225 mL 250 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 )
Calculate the pH at each of the following points for the titration of 200 mL of 0. 45 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide. H3His ↔ H+ + H2His- Ka1 = 3.98x10-3 H2His- ↔ H+ + HHis2- Ka2 = 9.12x10-7 HHis2- ↔ H+ + His3- Ka3 = 4.67x10-10 Vol. of NaOH Calculated pH 0 mL 37.5 mL 50 mL 75 mL 100 mL 150 mL 200 mL 225 mL 250 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 )
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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 200 mL of 0. 45 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide.
H3His ↔ H+ + H2His- Ka1 = 3.98x10-3
H2His- ↔ H+ + HHis2- Ka2 = 9.12x10-7
HHis2- ↔ H+ + His3- Ka3 = 4.67x10-10
|
Vol. of NaOH |
Calculated pH |
|
0 mL
|
|
|
37.5 mL
|
|
|
50 mL
|
|
|
75 mL
|
|
|
100 mL
|
|
|
150 mL
|
|
|
200 mL
|
|
|
225 mL
|
|
|
250 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 )
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