A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff: A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte. B. pH of the resulting solution at the equivalence point. C. pH of the resulting solution at 5.0 ml added titrant beyond the equivalence point.
A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff: A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte. B. pH of the resulting solution at the equivalence point. C. pH of the resulting solution at 5.0 ml added titrant beyond 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
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 weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff:
A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte.
B. pH of the resulting solution at the equivalence point.
C. pH of the resulting solution at 5.0 ml added titrant beyond the equivalence point.
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