In 100cm3 buffer solution of 0.1M CH3COOH and 0.05M HCl are added 3cm3 HCl 0.01M. Ph =?

Question

I'll wait for answer!

Answer 1

If I might respectfully suggest you review the question once again as the the way you present the facts of the question it does not make sense.

It appears you are attempting to find the pH of a solution of a strong acid (HCL) in a buffer solution.

A buffer is a weak acid such as given here (Ch3COOH) with its molarity and its volume which you give, however you need the conjugate base and its molarity and volume for the above weak acid which is not given. The conjugate base would be a salt of the weak acid which would be, as an example (CH3COONa) and that buffer system would buffer the strong acid (HCL) not allowing the pH to drop dramatically. The way you are wording the question you are stating a weak acid CH3COOH ( only one part of the buffer) and as stated above you need the other part of the buffer, not given, but instead is added to a strong acid (HCl, with no volume given), as if it is part of the buffer system, which it is not, and that is added to a strong acid (HCL) with molarity and volume given to be buffered.

Kindly reconsider restating the question.

Thanks.

Answer 2

pH=-log[H+]. Or pH=- log[H3O+]

For the Molarity of HCl [0.01]

You would plug that in and have:

pH= - log[0.01]. = 2. For that particular concentration. This is very acidic.