In the titration of a solution of weak monoprotic acid with a 0.1375 M solution of NaOH, the pH half way to the equivalence point was 4.46 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1375 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
In the titration of a solution of weak monoprotic acid with a 0.1375 M solution of NaOH, the pH half way to the equivalence point was 4.46 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1375 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
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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In the titration of a solution of weak monoprotic acid with a 0.1375 M solution of NaOH, the pH half way to the equivalence point was 4.46 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1375 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
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