Calculate the pH of a 0.10M solution oh hypochlorous acid, HOCl.
Ka = 3.5 x 10^-8
I understand the chemical equation will be:
HOCl + H20 === H30^+ + OCl^-
But as for the ICE table I don't understand which side would have the +x and which would have the -x.
2007-02-02 08:51:57 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
OK see the basic thing. HOCl is the stronger acid than H2O. Hence in this case HOCl acts as ACID and H2O acts as BASE. According to the (let us take) Bronsted-Lowery theory stronger acid is the proton donor and base is proton acceptor.
HOCl is loosing the proton so it gets the negative charge and H2O is accepting the proton so it gets the negative charge.
Now see the problem:
[H]+= \|KaxC
[H]+=\|3.5X10^-8X0.1
AFTER THIS YOU CALCULATE THE PH
2007-02-02 09:45:07 · answer #1 · answered by manidhar 2 · 0⤊ 0⤋
The HOCl loses a few, so it's -x, and the H3O+ and OCl- gain a few, so they're +x.
The H+ concentration is root (Ka x molarity), and then the pH is the negative logarithm of that. The acid is so weak that you really don't have to work out the equilibrium concentration of HOCl - use the initial concentration.
2007-02-02 17:00:33 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
i was gonna say that!!!
2007-02-02 17:17:49 · answer #3 · answered by taharniegsi 4 · 0⤊ 0⤋