What happens to [H+], pH and the %dissociation of an weak acid like HA is diluted 10 times


HA acid:
Ks = 1* 10^(-6)
1M solution


I would really appreciate the help

I'm not really sure if this is spelled correctly


I know how to calculate these but I just dont know what happens to them when the acid is diluted 10 times

This post was edited by twiiztedacer on Nov 23 2014 08:34am

% dissociation stays the same - Ka (dissociation constant) stays the same with concentration

1 M diluted to 0.1 M --> [H+] decrease by 10 times

-log[H+] = pH

log is base 10 so a change in [H+] of 10 means a change in pH of 1

pH will increase by 1

This post was edited by ArnoldChlamydia on Nov 23 2014 10:00am

about the % dissociation im not sure what u meant to ask - if the value of Ka changes or if % dissociation changes, either way they both stay the same. HCl is a strong acid -> fully dissociates

This post was edited by ArnoldChlamydia on Nov 23 2014 10:49am