Consider the dissociation of the tricrotic acid, H3Y.
H3Y + H20 <--> H3O^+ + H2Y^- K(a1)= 2.0 x 10^-4
H2Y^- + H2O <--> H3O^+ + HY^2- K(a2)= 8.0 x 10^-8
HY^2- + H2O <--> H30^+ + Y^3_ K(a3)= 4.0 x 10^-13
Use the values of K(a1), K(a2), K(a3), and K(w) to evaluate the equilibrium constants associated with each of the reactions shown below:
H3Y + OH^- <--> H2O + H2Y^-
H2Y^- OH^- <--> H2O + HY^2-
HY^2- + OH^- <--> H2O + Y^3-