Question

A buffer solution contains 0.1 M CH3COOH and 0.15M CH3COONa.

1.0cm3 of 0.1M NaOH was added to 1.0dm3 of the buffer solution.

Answer 1

What is the change in the pH of the solution? (Ka of CH3COOH = 1.75 x10-5 mol dm-3)

Answer 2

I should find the conc. of H+ right?

Answer 3

The previous question is linked to this question actually

Answer 4

i cant remeber that formula :(

Answer 5

Could it be
\[CH_3COOH \rightleftharpoons CH_3COO^-+H^+\]

Answer 6

\[n(NaOH)=\frac{MV}{1000}=\frac{0.1}{1000}=1 \times 10^{-4}mol\]

Answer 7

i am sorry really i dont want to tell you the wrong one :) i really not getting it

Answer 8

Its alright I'll figure out on my own then, thanks

Answer 9

ur welcome

Answer 10

for ur last question
this what happens when u add acid and base
Consider a solution containing both acetic acid, CH3COOH, and acetate ions, CH3COO-.

Any strong base that is added to the solution is neutralized by acetic acid:
CH3COOH (aq) + OH-(aq) CH3COO-(aq) + H2O (aq)

Any strong acid that is added to the solution is neutralized by acetate:
CH3COO-(aq) + H+(aq) CH3COOH (aq)

The amount of strong acid or base that a buffer can neutralize is called the buffer capacity. After the strong base or acid is neutralized, equilibrium will be reestablished.

Answer 11

Got it

Answer 12

Its done here :)
http://answers.yahoo.com/question/index?qid=20130926060011AAkUcJH