3. A student titrated 20.00 mL of a weak base solution, 0.150 M CH3NH2 (Kb = 4.40 × 10-4) with 0.100 M HCl solution. Calculate the pH at the equivalence point.
3. A student titrated 20.00 mL of a weak base solution, 0.150 M CH3NH2 (Kb = 4.40 × 10-4) with 0.100 M HCl solution. Calculate the pH at the equivalence point.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 52QAP: A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of...
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![3. A student titrated 20.00 mL of a weak base solution, 0.150 M CH3NH2 (Kb = 4.40 × 10-4)
with 0.100 M HCl solution. Calculate the pH at the equivalence point.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2849072-e5a2-41cb-8552-ffda5aa1016f%2F3b80e0fe-eda3-4d71-a6d6-f01ed21ed9d0%2Fh52kpic_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. A student titrated 20.00 mL of a weak base solution, 0.150 M CH3NH2 (Kb = 4.40 × 10-4)
with 0.100 M HCl solution. Calculate the pH at the equivalence point.
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