13. Consider a 50 mL solution of 0.150 MNH3 (Kb = 1.8 x 10-5). You are titrating it with a solution that is 0.120 MHCIO4. a) Find the pH of the solution after the addition of 15 mL of HCIO4. b) Find the pH of the solution at the one-half equivalence point. c) Find the pH of the solution at the equivalence point.
13. Consider a 50 mL solution of 0.150 MNH3 (Kb = 1.8 x 10-5). You are titrating it with a solution that is 0.120 MHCIO4. a) Find the pH of the solution after the addition of 15 mL of HCIO4. b) Find the pH of the solution at the one-half equivalence point. c) Find the pH of the solution at the equivalence point.
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 112CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...
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![13. Consider a 50 mL solution of 0.150 MNH3 (Kb = 1.8 × 10-5). You are titrating it with a
solution that is 0.120 MHCIO4.
a) Find the pH of the solution after the addition of 15 mL of HC1O4.
b) Find the pH of the solution at the one-half equivalence point.
c) Find the pH of the solution at the equivalence point.
d) Find the pH of the solution after the addition of 70 mL of HCIO4.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F961160e4-6bad-43bb-a101-67a2e89b2eec%2F502a914a-b3df-4edc-a47a-65fbd62a5346%2Furlirnb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:13. Consider a 50 mL solution of 0.150 MNH3 (Kb = 1.8 × 10-5). You are titrating it with a
solution that is 0.120 MHCIO4.
a) Find the pH of the solution after the addition of 15 mL of HC1O4.
b) Find the pH of the solution at the one-half equivalence point.
c) Find the pH of the solution at the equivalence point.
d) Find the pH of the solution after the addition of 70 mL of HCIO4.
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