Titration of a weak base with a strong acid (continued) | Khan Academy

Calculating the pH for titration of weak base, ammonia, with strong acid, HCl, at the equivalence point and past the equivalence point. Created by Jay.
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[@td6063]

this whole titration series has been extremely helpful, this is what the equillibrium series should have been

[@jcash409]

7:35 the whole time you have been using no. of moles in the I section and now you put in the concentration of NH4? Shouldnt it be 0.004

[@AndyU96]

At the last section, NH3 is all used up to neutralize H3O+, so the reaction is:
(NH3) + (H3O+) ----> (NH4+) + (H2O)
No NH3 left, we have excess H3O+, and plenty of NH4+, so the question is:
Will that NH4+ not react with water?

[@mohammadhatamleh6713]

well what you're saying is true but if you do the calculation you'll realize that the 0.004 mols of NH4 will barely affect it all. This is because the 0.002 mols of H30 will cause 0.004 mols of NH4 to be neglected since it is a weak acid compared to H30

[@quintenspeelt5063]

for future people who see this, the H3O+ that NH4+ will create (the amout of concentration) is so small (4.73 x 10-6) that it will not affect the ph at all so you can just leave that behind

[@kfc1970]

great work. so helpful.👌🙏

[@yumenoritsu]

Thanks~! :)

[@shadajaradat4397]

Thanksss sir

[@hongyimarkye5708]

Than you.

[@brayan9645]

why isn't he using the Henderson hasselbalch equation by inputting cl- as the base and HCI into the log a d then adding pka?

[@nurlybektoktarov469]

Lifehack: put it at the speed 1.5 and Khan Academy will speak like normal human 😄