25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50 M NaOH. Calculate the pH of the mixture, a) at the half equivalence point. b) List the major species in equilibrium in part (a) c) at the equivalence point. d) after adding 20.0 mL of 0.50 M NaOH.

25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50 M NaOH. Calculate the pH of the mixture, a) at the half equivalence point. b) List the major species in equilibrium in part (a) c) at the equivalence point. d) after adding 20.0 mL of 0.50 M NaOH.

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 110CP: A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where...

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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

25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50
M NaOH. Calculate the pH of the mixture,
a) at the half equivalence point.
b) List the major species in equilibrium in part (a)
c) at the equivalence point.
d) after adding 20.0 mL of 0.50 M NaOH.

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