[IHeartOJ]

Hi,
I'm having a bit of trouble with this question.

Four beakers contain acids:

• 0.01M acetic acid - pH: 3.4
• 0.01M HCl acid - pH: 2.0
• 1x10^-5M acetic acid - pH 5.2
• 1x10^-5M HCl acid - pH 5.0

Explain with reference to Le Chatelier's Principle, why the pH values of the two 1x10^-5M acid solutions are much close than the pH values of the two 0.01M acid solutions

I know that HCl is a strong acid and therefore undergoes full ionisation and the pH = -log[H+] and that acetic acid is a weak acid and is only partially ionised which explains why its pH is slightly higher than its corresponding pair but I'm stuck on how to use Le Chatelier to explain why 1x10^-5M acid solutions are closer in pH values. Can anyone point me in the right direction?

[Borek]

What happens to the acid dissociation when you dilute the solution?