Question

Calculate the pH in the titration

Answer 1

25.0 ml of 0.1M acetic acid by sodium hydroxide after the addition to the acid solution of 10ml of 0.1M NaOH

Answer 2

How should we start?

Answer 3

you're titrating a weak acid, so find \([H_3O^+]\) after neutralization. Take into account the conjugate base of acetic acid and how that influences the pH.

Answer 4

\[CH_3COOH+NaOH \rightleftharpoons CH_3COONa+H_2O\]
Acetic acid is acid, Water is conjugate acid
NaOH is base, Sodium acetate is conjugate base

Answer 5

Should we use an ICE table for this?

Answer 6

\[CH_3COOH+NaOH \rightleftharpoons CH_3COONa+H_2O \]
I 2.5x10-3 1x10-3 0
C -1x10-3 -1x10-3 +1x10-3
E 1.5x10-3 0 1x10-3

[CH3COOH]=0.1M
[CH3COONa]=0.02857M

Hmm

Answer 7

The problem with applying Henderson - Hasselbalch equation is they did not give the Ka for this titration... :\

Answer 8

i'm sure they're expecting you to look up the Ka in your book, or elsewhere. I don't think it's possible otherwise

Answer 9

Yep, that's exactly what you are supposed to do.

Answer 10

I got pH=4.58

Answer 11

Correct!

Answer 12

Awesome thanks :)