Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10 –5 . a. What is the pH after 15.00 mL of HCl have been added? b. What is the pH at the equivalence point? c. What is the pH 2.00 mL past the equivalence point volume?
Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10 –5 . a. What is the pH after 15.00 mL of HCl have been added? b. What is the pH at the equivalence point? c. What is the pH 2.00 mL past the equivalence point volume?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 105CWP: Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25C. (Ka for HCN = 6.2 1010.)...
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Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10 –5 .
a. What is the pH after 15.00 mL of HCl have been added?
b. What is the pH at the equivalence point?
c. What is the pH 2.00 mL past the equivalence point volume?
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