etermine the pH during the titration of 72.8 mL of 0.367 M formic acid (Ka = 1.8x104) by 0.367 M KOH at the following oints. (Assume the titration is done at 25 °C.) a) Before the addition of any KOH D) After the addition of 16.0 mL of KOH :) At the half-equivalence point (the titration midpoint) d) At the equivalence point e) After the addition of 109 mL of KOH

etermine the pH during the titration of 72.8 mL of 0.367 M formic acid (Ka = 1.8x104) by 0.367 M KOH at the following oints. (Assume the titration is done at 25 °C.) a) Before the addition of any KOH D) After the addition of 16.0 mL of KOH :) At the half-equivalence point (the titration midpoint) d) At the equivalence point e) After the addition of 109 mL of KOH

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.7QAP

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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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Determine the pH during the titration of 72.8 mL of 0.367 M formic acid (Kā = 1.8×10-4) by 0.367 M KOH at the following
points. (Assume the titration is done at 25 °C.)
(a) Before the addition of any KOH
(b) After the addition of 16.0 mL of KOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 109 mL of KOH

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Step 2: Calculate pH before addition of KOH

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Step 3: When added of 16.0 ml of KOH

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Step 4: pH at the half equvilence point

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Step 5: pH at equvilence point

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Step 6: pH when added 109 ml of KOH

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