Simple pH Problem (If I could remember)

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SUMMARY

The discussion centers on calculating the pH of a solution after mixing 100 mL of 0.1M sodium acetate with 100 mL of 0.1M acetic acid, resulting in an initial pH of 4.7. Upon adding 60 mL of 0.1M NaOH, the pH must be recalculated using the Henderson-Hasselbalch equation. The key point is that acetic acid is monoprotic, thus it has a single pKa value, which simplifies the calculation process. Participants express confusion regarding the application of pKa in multi-acid systems, but in this case, only the pKa of acetic acid is relevant.

PREREQUISITES
  • Understanding of the Henderson-Hasselbalch equation
  • Knowledge of pKa values, specifically for acetic acid
  • Familiarity with acid-base titration concepts
  • Basic skills in solution concentration calculations
NEXT STEPS
  • Review the Henderson-Hasselbalch equation and its applications in buffer solutions
  • Study the pKa of acetic acid and its implications in acid-base chemistry
  • Learn about titration curves and how to interpret them
  • Explore the effects of strong bases on weak acid solutions
USEFUL FOR

Chemistry students, particularly those studying acid-base equilibria, educators teaching General Chemistry, and anyone needing to understand buffer systems and pH calculations.

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Homework Statement


If one mixed 100mL of .1M Sodium acetate with 100 mL of .1M acetic acid, the pH of the solution would be 4.7 If 60 mL of .1M NaOH were added to this solution, what would be it's pH?


Homework Equations


Henderson Hasselback
pH=pKa+ log(base/acid)


The Attempt at a Solution


I haven't really made one because I'm not sure how to proceed. The thing that really confuses me is the pKa part of henderson-hasselbach. When we are dealing with solutions having more more than one pkA, which pkA do we use? I know I did a ton of these problems in Gen Chem but can't remember how!
 
Physics news on Phys.org
There's only one thing (ignoring water) that has a pKa: the acetic acid. Since acetic acid is monoprotic, it has only one pKa.
 

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