Recent content by jonnyupton

[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 =...