Question

-Calculate [H3O+] for the 0.10 M CH3COOH solution which has a pH = 2.88.

-What percent of the weak acid is dissociated?
*Can someone just help me figure out how i would approach the problem?? Thanks!(:

Answer 1

well you know \([H_3O^+]\) from pH, so just find what percent \([H_3O^+]\) is from\([CH_3COOH]\) (which is 0.1 M).

Answer 2

Thanks for replying!!
ok so I got 1.32x10^-3 for the [H3O+] .. How would I find what percent of that is from CH3COOH?

Answer 3

\(\dfrac{[H_3O^+]}{[CH_3COOH]}*100\%\)

Answer 4

hm no wait. that seems wrong

Answer 5

so for the bottom part, are you referring to the molecular mass in moles?

Answer 6

i was thinking.. i don't actually remember seeing that formula in class, but you're the expert! haha(:

Answer 7

hm it's not really a formula, it's like if you have 10 cats and you let 2 lose, what percent of cats did you let lose?

\(\dfrac{2}{10}*100\%\)=20%

same kind of thing

Answer 8

i think it works: 0.0013182567385564/0.1*100%=1.3182567385564%

Answer 9

ohh ok! so that's for the second part though right?
and the first part i put in what i got for h30 right?

Answer 10

Wait nvm, I got it!
hahaha.. ok so let me just put in the second part and see if that's right!

Answer 11

Totallly worked, thank you sooooooooooo soooooo much! Hahaha..
Seriously, most amazing person on here! Thanks!!(:

Answer 12

okay awesome ! no problem at all ! i wasn't sure if that was right for a min lol

Answer 13

Oh come on now, you're always right! Hahaha, well once again, thanks a lot!!(: