[H2A]aq is the species concentration used to relate the total acid concentrations in both phases of the liquid-liquid equilibrium mixture which is what I am interested in. Only undissociated acid is transferred between the two phases in this case.
I will try as you suggest and see how well...
I have an initial aqueous phase concentration of diprotic acid H2A of 0.2 M.
pKa1 4.418
pKa2 5.412
pKa 9.830
Ka1 3.82E-05
Ka2 3.87E-06
Ka 1.48E-10
[ACID]aq = [H2A]aq + [HA-]aq + [A2-]
I have calculated the equilibrium concentrations of all species in the aqueous phase as...
Could you please then explain which relationship I can use to solve the problem?
I am a final year Chemical Engineering student with only my basic A-Level Chemistry to rely on here and I'm not finding that it's helping much in this case.
All the relationships described involve at least 2...
I have previously found and read that webpage but cannot figure out how that helps in this case.
As far as I can work out I need to work out the stoichiometric relationship between the A2- and H+ ions.
Is is accurate simply to say that [A2-] is equal to [H+]/2 from the dissociation...
I would like to relate the pH of an aqueous phase diprotic acid solution to a value of the undissociated acid species concentration in the aqueous phase, and vice versa.
I have Ka1 and Ka2 values for the acid.
The overall dissociation equilibrium can be written:
Ka1*Ka2 =...