Thanks, Brian.
Yes, the measured acidity is total phenolpthalein acidity (titrated o pH 8.3) in which mineral acid (HCl) dominated (I added concentrated HCl to the solution).
Apparently, the measured acidity might not be correct (acidity = 1186 mg/L as CaCO3 which is equivalent to ~23.72mmol NaOH). However, I run the React module to titrate this solution (pH 2) with NaOH. It requires about 100 mmol to bring pH to 8.3. In this run, I assume CO2aq is in equilibrium with atmospheric CO2 (during titration) so I used HCO3-/CO2 = 1.2E-05 mol/l, which is calculated from Henry's law.
So it comes to this question:
(a) The solution is in equilibrium with N2 filled in head space during the experiment. Is it correct (acceptable) to assume the CO2(aq) is in equilibrium with very low PCO2, then calculate CO2aq = KCO2xPCO2 according to Henry's law? this method should give HCO3-/CO2 = <1.2E-05 mol/l.
OR
( should I calculate CO2aq from CO2 (aq) + H2O --> H+(aq) + HCO3-(aq), assuming HCO3-= H+ = 0.01 mol/l? this method gives HCO3-/CO2 = 0.01^2/4.45e-7 = 224.7 mol/L (which is too high, is it odd?)
Thanks,
Tyler