1. The problem statement, all variables and given/known data Calculate the pH at the equivalence point for the titration of 0.20 M NH3 with 0.20 M HCl? Kb of ammonia is 1.8e-5 This is just a old test I am going over, I managed to get a pH of 4.98. but that is not right the right answer is 5.12 and I cant figure out why. I would assume you could use the henderson equation but I only get 4.98 which is wrong. Any help?
acid base titration equivalence point calculation Note: you should not use Henderson-Hasselbalch, however, you should not forget about dilution.
I did and didn not use the HH eq, not do i understand what you mean by dilution. I also read link, and this is onlything really useful that I understood but still does not explain what I am doing wrong: Spoiler In the case of titration of weak base with strong acid, situation is very similar - pH at the equivalence point is determined by the weak base salt hydrolysis. Thus we need pKa of conjugated acid to calculate H+ and pH. Check lecture and cheat sheet mentioned above for details. It would be great if you told me what I am doing wrong...
Try here: dilution effects. Generally speaking, you have mixed two solutions, concentrations have changed as the final volume differs from the initial for each reagent.