Calculating the pH of 0.1M Acetic Acid Neutralized by NaOH (Ka = 1.7 x 10^-5)

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SUMMARY

The discussion focuses on calculating the pH of a 0.1M acetic acid solution when it is half neutralized by sodium hydroxide (NaOH). The equilibrium constant for acetic acid (Ka = 1.7 x 10^-5) is critical for this calculation. The resulting pH after half neutralization is determined to be 4.7695. Participants emphasize the importance of understanding the neutralization process and the role of weak acids in pH calculations.

PREREQUISITES
  • Understanding of weak acid dissociation and equilibrium constants (Ka)
  • Knowledge of pH calculation methods
  • Familiarity with neutralization reactions
  • Basic chemistry concepts related to acetic acid and sodium hydroxide
NEXT STEPS
  • Study the Henderson-Hasselbalch equation for pH calculations
  • Learn about the properties of weak acids and their dissociation
  • Explore titration curves for weak acid-strong base reactions
  • Investigate the impact of concentration on pH in buffer solutions
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Chemistry students, educators, and anyone involved in acid-base chemistry who seeks to understand pH calculations and neutralization processes.

shaiqbashir
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Hi Guys!


cakculate the pH of a 0.1M acetic acid when it is half neutralized by NaOH solution (Ka= 1.7 x 10^-5)

Ans: 4.7695


My dear friends! I am unable to understand the language of this question , Please tell me this question in some easier words so that i can just solve it on. A little hint will work i guess

Thanks in advance
 
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You start with solution of acetic acid and add NaOH till half of the acid reacted.
 

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