How do you determine pH for a titration of a weak base with astrong acid? Specif

Question

How do you determine pH for a titration of a weak base with astrong acid? Specifically, could you work this problem so I canhave an example:

A 25.0-mL sample of 0.100 M NH3 (Kb = 1.8 x10-5) is titrated with 0.100 M HCl solution. Calculatethe pH after the addition of 0.0 mL, 4.0 mL, 12.5 mL, 20.0 mL,24.0mL, 24.5 mL, 25.0 mL, 25.1 mL, 26.0 mL, 28.0mL, and 30.0mL.

I particularly get stuck on how to calculate pH from the finalmolarities of the solution. We have [NH3] and[NH4+] and [H+] seems to be zero,so other than using Henderson-Hasselbalch (buffer) equation, isthere another way to find pH?

Explanation / Answer

Nevermind, i figured it out.

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