[Optikspik]

If U have 0,3 Molar of carbonic acid and the [CO_32- is 2*10-13M in a system of the following equlibriums:
H2CO3 <=> H+ HCo3(-)
HCO3(-) <=> H+ CO3(2-) How will the pH vaulebe affected if u add LiHCO_3 to the reaction?
Given is that kb for HCO3(-) is bigger than ka so it works more like a base than an acid. But Im unsure how i use le chateliers principle to answer this question? How should i resonate?
Thanks in advance

[Borek]

Concentration of CO₃^2- doesn't matter. If you have a solution of carbonic acid its pH is dominated by the first dissociation step. What happens to the first dissociation equilibrium when you add HCO₃^-?