Still am having trouble with titration

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SUMMARY

The discussion centers on creating a buffer solution with a target pH of 4.6 using 1M acetic acid (HAc) and 1M sodium hydroxide (NaOH). The user, David Westra, seeks clarification on the calculations required to determine the appropriate volumes of each solution needed to achieve the desired pH. The conversation highlights the importance of understanding buffer preparation in high school chemistry, particularly in relation to titration concepts.

PREREQUISITES
  • Understanding of buffer solutions and their pH calculations
  • Knowledge of titration principles and acid-base reactions
  • Familiarity with the Henderson-Hasselbalch equation
  • Basic skills in volumetric measurements and solution preparation
NEXT STEPS
  • Study the Henderson-Hasselbalch equation for buffer calculations
  • Practice titration techniques using acetic acid and sodium hydroxide
  • Explore the concept of buffer capacity and its implications
  • Review laboratory protocols for preparing standard solutions
USEFUL FOR

This discussion is beneficial for high school chemistry teachers, students learning about acid-base chemistry, and anyone interested in mastering buffer solution preparation and titration techniques.

westdavi
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Thank you for responding, but I am not sure how to solve this yet. I am sorry. Could you show me a more of the work needed? I teach high school chemistry, and it is beginning to look like the question is beyond the scope of the course, but now I am curious how to solve it.
Anyways, thanks for your help regardless
David Westra
You have two bottles, one filled with 1M HAc (HAc = acetic acid) and one filled with 1M NaOH. You want to make 100ml of a buffer with pH=4.6 by mixing together appropriate amounts of these solutions. How much of each solution do you use?
 
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I edited my reply to make it more detailed in your other post. Hope that helps.
 

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