Consider the titration of 100.0 mL of 0.016 M HClO₂ (Ka = 3.5 x 108) with 0.0400 M NaOH. Calculate the pH (a) before addition of any NaOH. b) after addition of 10.0 mL of 0.0400 M NaOH. c) halfway to the equivalnce point.

Consider the titration of 100.0 mL of 0.016 M HClO₂ (Ka = 3.5 x 108) with 0.0400 M NaOH. Calculate the pH (a) before addition of any NaOH. b) after addition of 10.0 mL of 0.0400 M NaOH. c) halfway to the equivalnce point.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 88AE: Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012)...

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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.

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Consider the titration of 100.0 mL of 0.016 M HCIO₂ (Ka = 3.5 x 108) with 0.0400 M NaOH.
Calculate the pH
(a) before addition of any NaOH.
b) after addition of 10.0 mL of 0.0400 M NaOH.
c) halfway to the equivalnce point.

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Step 1: Reaction between weak acid and NaOH

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Step 2: pH before addition of any NaOH

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Step 3: pH after addition of 10 ml of 0.04 M NaOH

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Step 4: pH halfway to the equivalence point

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