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A chemist combines 23.85 mL of a 1.197 M solution of acid "HA (Ka = 1.41 x 10-9) with a 0.5005 M solution of NaOH. 1) Calculate the pH when 24.19 mL of NaOH is added 2) Calculate the pH at the half equivalence point of the titration 3) Calculate the pH when 83.79 mL of NaOH is added 4) Determine the equivalence volume of the titration 5) Determine the pH of the titration at the equivalence point

A chemist combines 23.85 mL of a 1.197 M solution of acid "HA (Ka = 1.41 x 10-9) with a 0.5005 M solution of NaOH. 1) Calculate the pH when 24.19 mL of NaOH is added 2) Calculate the pH at the half equivalence point of the titration 3) Calculate the pH when 83.79 mL of NaOH is added 4) Determine the equivalence volume of the titration 5) Determine the pH of the titration at the equivalence point

Chemistry
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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A chemist combines 23.85 mL of a 1.197 M solution of acid "HA (Ka = 1.41 x 10-9) with a 0.5005 M solution of NaOH. 1) Calculate the pH when 24.19 mL of NaOH is added 2) Calculate the pH at the half equivalence point of the titration 3) Calculate the pH when 83.79 mL of NaOH is added 4) Determine the equivalence volume of the titration 5) Determine the pH of the titration at the equivalence point
Transcribed Image Text:A chemist combines 23.85 mL of a 1.197 M solution of acid "HA (Ka = 1.41 x 10-9) with a 0.5005 M solution of NaOH. 1) Calculate the pH when 24.19 mL of NaOH is added 2) Calculate the pH at the half equivalence point of the titration 3) Calculate the pH when 83.79 mL of NaOH is added 4) Determine the equivalence volume of the titration 5) Determine the pH of the titration at the equivalence point
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