A student dissolves 0.0100 mol of an unknown weak base in 100.0 mL water and titrates the solution with 0.100 M HNO3. After 60.0 mL of 0.100 M HNO3 was added, the pH of the resulting solution was 7.96. Calculate the K value for the weak base. %3D

A student dissolves 0.0100 mol of an unknown weak base in 100.0 mL water and titrates the solution with 0.100 M HNO3. After 60.0 mL of 0.100 M HNO3 was added, the pH of the resulting solution was 7.96. Calculate the K value for the weak base. %3D

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A student dissolves 0.0100 mol of an unknown weak base in 100.0 mL water and titrates the solution with 0.100 M
HNO3. After 60.0 mL of 0.100 M
HNO3 was added, the pH of the resulting solution was 7.96. Calculate the
K value for the weak base.

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