00:01
The first step of the reaction is the dissociation of carbonic acid that is h2co3.
00:07
This will dissociate into h plus and hco3 that is bicarbonate ion.
00:13
Now we will apply the simple ice rule here.
00:16
The initial concentration of h2co3 we know that it is equal to 0 .100 and that of both the constituent ions is equal to zero.
00:24
The change in concentration let us assume it to be x.
00:27
So x amount of h2co3 is reduced and similarly x amount of both the constituent ions is formed.
00:35
Now at equilibrium we can see that equivalent concentration of h2co3 will be 0 .100 minus x and that of both the constituent ions will be x.
00:46
Talking about step 2, this is the further dissociation of bicarbonate ions.
00:52
This will dissociate into h plus and carbonate ions that is co3 2 negative.
00:56
Now apply the ice rule here as well.
00:58
The initial concentration is x.
01:00
The change will be minus x, x and x.
01:06
So at equilibrium the equivalent concentration will be 0, x and x.
01:12
So the concentration of h plus in the final equilibrium is given by the concentration of h plus from both the steps...