QUESTION 1 Calculate the pH after addition of 24.38 mL of 0.1148 M HCIO4 to 25.00 mL of 0.1989 M CH3CH2NH2. Kы(CH3CH2NH2) = 6.400e- 4. Key Concept: Titration of a weak base by a strong acid. Up to just before the equivalence point, the Henderson-Hasselbach equation can be used to determine pH. Although this is not the normal form it works quite nicely: pH = pKa - log(nb/na) Strategy Calculate initial mol of base, calculate mole of acid added →nb = initial mol of base minus mol acid added; na = mol of acid added.;

QUESTION 1 Calculate the pH after addition of 24.38 mL of 0.1148 M HCIO4 to 25.00 mL of 0.1989 M CH3CH2NH2. Kы(CH3CH2NH2) = 6.400e- 4. Key Concept: Titration of a weak base by a strong acid. Up to just before the equivalence point, the Henderson-Hasselbach equation can be used to determine pH. Although this is not the normal form it works quite nicely: pH = pKa - log(nb/na) Strategy Calculate initial mol of base, calculate mole of acid added →nb = initial mol of base minus mol acid added; na = mol of acid added.;

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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