The pH of acetic acid. (1 Viewer)

[de rigueur]

Hihi.

CH3COOH + NaOH > CH3COONa + H2O

CH3COOH has a concentration of 0.001M
Calculate the pH.

[CH3COOH] = -log [H+]
= -log [0.001]
= 3

Is this right?

 

[fullonoob]

Hihi.

CH3COOH + NaOH > CH3COONa + H2O

CH3COOH has a concentration of 0.001M
Calculate the pH.

[CH3COOH] = -log [H+]
= -log [0.001]
= 2

Is this right?

lol thats weird O_O
your calc must be effed or something cos it = 3 when you type it in
calculate ph of [CH3COOH] or what ??
your answer is wrong in my opinion
cos theres 3 H+ and 1 OH
i dno how to calculate H+ and OH- in the same equation so can't help sorry
You have to find pOH and pH and i've no idea how to do that

 

[de rigueur]

haha.. yeah i get that its 3 not 2.
fixed that now!

thanks for helping...me shit at chem calcs

 

[fullonoob]

hey i never said 3 was right xD
could someone please answer the question, i can't do it

 

[adomad]

just use -log{H+} = pH... and acetic acid ch3cooh isn't made up from 3 H^+ and an OH^-. when it ionises, it becomes CH3COOH<--->CH3COO^- +H^+. but acetic acid doens't completely ionise. if the question tells you that is is like only a 2% ionisation, then you must find the 2% and then use -log{H+} = pH.

 

[Status]

CH3COOH + NaOH > CH3COONa + H2O

CH3COOH has a concentration of 0.001M
Calculate the pH.

Since Acetic acid only ionises 1.3%

[CH3COOH] = -log [H+]
= -log [0.001 x (1.3/100) ]
pH = 4.9

 

[Julz666]

CH3COOH + NaOH > CH3COONa + H2O

CH3COOH has a concentration of 0.001M
Calculate the pH.

Since Acetic acid only ionises 1.3%

[CH3COOH] = -log [H+]
= -log [0.001 x (1.3/100) ]
pH = 4.9

Unless the 1.3% is specified, we assume it ionizes 100%
so it becomes
-log(0.001)
which equals 3

 

[Julz666]

calculate ph of [CH3COOH] or what ??
cos theres 3 H+ and 1 OH

the structure of CH3COOH means that the OH cannot isonise, as it is bound to the carbon, meaning that only the H will ionise, leaving CH3COO-