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

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To calculate the pH after titrating 20.0 mL of 0.1 M NaOH into 50.0 mL of 0.14 M HOBr, first determine the concentrations of HOBr and OBr- using stoichiometry from the neutralization reaction. The pH of the resulting solution can be found using the Henderson-Hasselbalch equation, which incorporates the concentrations of the acid and its conjugate base. The initial pH of HOBr is 4.74, and the dissociation constant (Ka) is 2.3e-9. The final pH after the titration is calculated to be 8.24.
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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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