Chemistry? Calculate the concentration of all species in a 0.180 M solution of H2CO3.?

Calculate the concentration of all species in a 0.180 M solution of H2CO3.

Answer 1

Tricky. That’s because there are NO molecules of H2CO3 in a solution of carbonic acid. Molecules of H2CO3 do not exist in liquid water. Carbonic acid is actually a solution of CO2 in equilibrium with small amounts of H+ ions and HCO3^- ions. The equilibrium lies far to the left, which means that most of the CO2 stays CO2.
CO2(aq) + H2O(l) <==> H+ + HCO3^-

HCO3^- is a weak acid, so there will be even less CO3^2- in solution.
HCO3^- <==> H+ + CO3^2-
____________

CO2(aq) + H2O(l) <==> H+ + HCO3^- ……….. Ka = 4.3×10^-7 (*)
Ka = [H+][HCO3^-] / [CO2]
4.3×10^-7 = x² / 0.180
x = 2.8×10^-4 …. x = [H+] = [HCO3^-]
[H+] = 2.8×10^-4 …… pH = 3.57
[OH-] = 1.0×10^-14 / 2.8×10^-4 = 3.6×10^-11

HCO3^- <==> H+ + CO3^2- …… Ka = 4.8×10^-11
Ka = [H+][CO3^2-] / [HCO3^-]
4.8×10^-11 = [CO3^2-]

* Ka values from http://clas.sa.ucsb.edu/staff/Resource%2…

Answer 2

no

Leave a Comment