How Do You Calculate pH After Titration of HOBr with NaOH?

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SUMMARY

The discussion centers on calculating the pH after titrating 20.0 mL of 0.1 M sodium hydroxide (NaOH) into 50.0 mL of 0.14 M hypobromous acid (HOBr). The pH of the resulting solution is determined to be 8.24. Key calculations involve using the dissociation constant (Ka) of HOBr, which is 2.3e-9, and applying the Henderson-Hasselbalch equation after determining the concentrations of HOBr and its conjugate base, OBr-, from the neutralization reaction stoichiometry.

PREREQUISITES
  • Understanding of acid-base titration principles
  • Familiarity with the Henderson-Hasselbalch equation
  • Knowledge of dissociation constants (Ka and Kb)
  • Basic stoichiometry for neutralization reactions
NEXT STEPS
  • Study the Henderson-Hasselbalch equation in detail
  • Learn about calculating pH from weak acid and strong base titrations
  • Explore the concept of acid dissociation constants (Ka) and their applications
  • Review stoichiometric calculations in acid-base reactions
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Chemistry students, educators, and anyone involved in analytical chemistry or acid-base titration methodologies.

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Homework Statement


20.0 mL of a 0.1 M solution of sodium hydroxide is titrated into 50.0 ml of the 0.14 M HOBr solution. Calculate the pH of the resulting solution.

ph of HOBr is 4.74

Ka is 2.3e-9


Homework Equations



[H+] = ka(a/b)

-log[h+] = ph

ka*kb=kw


The Attempt at a Solution



honestly i have no clue how to do this problem. I already know the answer its 8.24, but I haven't a clue how to get it. can someone point me in the right direction?

thanks
 
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Calculate concentrations of HOBr and OBr- (just from the neutralization reaction stoichiometry), plug these numbers in the Henderson-Hasselbalch equation.
 

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