00:01
So we have these compounds which act as perfect solutions because they have a weak acid and a conjugate base.
00:09
Now we're going to see how they react with a strong acid and a strong base.
00:16
So strong acid like hcl, when dissolves in water, it's going to dissociate into h plus ncl minus ions.
00:26
The h plus ions are going to accumulate.
00:30
But when we have a buffered solution like ch3c ooh, what's going to happen is that the ch3coo minus the conjugate base is going to react with the h plus ions and it's going to form ch3cooh plus cl minus.
00:57
This means the h plus ions is not going to accumulate but instead it's going to react.
01:04
So this is going to be our equation for when this buffer solution reacts with a strong acid.
01:14
Now for a strong base, the ch3c -o -o -h, when it reacts with n -a -o -h, the o -h minus ions in the n -o -h have a very strong affinity for the h -plus ions.
01:32
So this is going to give us n -a -c -h -3 -c -o plus h -2o...