Write the equation for the reaction associated with the Ka2 of sulfuric acid, H2SO4.
Write the equation for the reaction associated with the Kb2 of carbonate, CO32–.
To write the equations for the reactions associated with Ka2 and Kb2, we first need to understand what these terms mean.
Ka2 represents the acid dissociation constant for the second ionization of a polyprotic acid. This means it measures the extent to which the acid donates its second hydrogen ion (H+) in solution. In the case of sulfuric acid (H2SO4), it is a diprotic acid, meaning it can donate two hydrogen ions.
The equation for the first ionization of sulfuric acid is:
H2SO4 ⇌ H+ + HSO4–
To write the equation for the second ionization, we need to consider that the HSO4– ion can further dissociate to release another hydrogen ion. Therefore, the reaction associated with the Ka2 of sulfuric acid is:
HSO4– ⇌ H+ + SO42–
Now, let's move on to the Kb2 of carbonate. Kb2 represents the base dissociation constant for the second ionization of a polyprotic base. Carbonate (CO32–) is a polyprotic base that can accept two protons (H+).
The equation for the first ionization of carbonate is:
CO32– + H2O ⇌ HCO3– + OH–
To write the equation for the second ionization, we need to consider that the HCO3– ion can accept another hydrogen ion to form a new species. Therefore, the reaction associated with the Kb2 of carbonate is:
HCO3– + H2O ⇌ CO32– + H3O+