What Is the pH After Titrating Butanoic Acid with NaOH?

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SUMMARY

The discussion focuses on calculating the pH after titrating 0.02 L of 0.1 M butanoic acid with 0.01 L of 0.1 M NaOH. The pH after titration is determined to be 4.81. The key to solving this problem involves recognizing the transition from a weak acid solution to a buffer system, which can be analyzed using the Henderson-Hasselbalch equation, and finally considering the hydrolysis of the conjugate base formed during the titration.

PREREQUISITES
  • Understanding of weak acid and strong base titration principles
  • Familiarity with the Henderson-Hasselbalch equation
  • Knowledge of acid dissociation constant (Ka) and its application
  • Basic concepts of hydrolysis in acid-base chemistry
NEXT STEPS
  • Study the Henderson-Hasselbalch equation in detail
  • Learn about buffer solutions and their pH calculations
  • Explore the concept of hydrolysis of conjugate bases
  • Practice additional titration problems involving weak acids and strong bases
USEFUL FOR

Chemistry students, educators, and anyone involved in laboratory work related to acid-base titrations and buffer solutions.

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Hi.
I am having trouble with acid-base titration excercises. 0.02 L butanoic acid @ 0.1 M is titrated with 0.01 L NaOH solution @ 0.1 M. The Ka of butanoic acid is 1.54X10^-5. Find the pH. The answer is 4.81. I know how to find the pH when no NaOH is added, but I really don't see how the Ka fits in when adding a base. An explanation would really be appreciated. Thanks.
 
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