Determine the pH during the titration of 20.1 mL of 0.429 M hydrocyanic acid (K₂ = 4.0x10-10) by 0.359 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 5.40 mL of KOH (c) At the half-equivalence point (the titration midpoint)

Determine the pH during the titration of 20.1 mL of 0.429 M hydrocyanic acid (K₂ = 4.0x10-10) by 0.359 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 5.40 mL of KOH (c) At the half-equivalence point (the titration midpoint)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 56P

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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

Determine the pH during the titration of 20.1 mL of 0.429 M hydrocyanic acid (Ka
by 0.359 M KOH at the following points.
(a) Before the addition of any KOH
(b) After the addition of 5.40 mL of KOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 36.0 mL of KOH
=
4.0×10-10)

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