## Carbonate Species vs. pH (Open System)

Given is H2O in contact with the atmosphere (open system). What is the carbonate species distribution in the pH range between 1 and 10?

Titration Calculations

For a fixed CO2 partial pressure (0.00039 atm) and a given temperature (25), the equilibrium state of the open system is uniquely determined by a set of thermodynamic equations that yields pH = 5.61. In order to decrease or increase pH you should add acids (HCl) or bases (NaOH).

Addition of HCl. Start with pure water (button H2O) and select ‘Open CO2 System’ with the default parameter pCO2 = 3.408. Then enter the desired pH value, say pH = 3, and set an arbitrary start value for chloride (to mimic HCl addition), say 1 mM Cl.

Click on Start and perform charge-balance adjustment with Cl. The program promptly outputs the correct amount of Cl (which is equivalent to the molar amount of HCl). The output tables (including table Ions) display the complete speciation. Some of these data are listed in the table below.

Repeat the calculation for any other pH < 5.61. The table below gives you some idea. Completion of this table is going faster than expected.

Addition of NaOH. For pH > 5.61 repeat the above procedure, but use Na instead of Cl (in order to simulate NaOH addition). Examples are given in the bottom half of the table below.

Results

Table. The table summarizes the titration calculations at 25. It contains the amount of HCl or NaOH to achieve the pH, the carbonate speciation, the ionic strength (I in mM), and the alkalinity (Alk in meq/L). Here, CO2 stands for the composite carbonic acid; this value remains constant throughout the whole titration.1 The pure CO2 system is marked by light-red color.

Diagram. The diagram displays the calculated data: DIC and carbonate species in logarithmic scale as a function of pH. The H+ curve is a straight line that results from H+ = 10-pH.2 Mass Conservation (Mole Balance). In contrast to the closed CO2 system, the total dissolved inorganic carbon is no longer a constant:

 (1) DIC  =  CO2 + HCO3- + CO3-2 + NaHCO3 + NaCO3-  ≠  const

At pH ≈ 5.5 the DIC begins to increase exponentially.3

Footnotes & Remarks

1. At pH ≤ 1 the CO2 value slightly deviates from 0.0133 mM. This is an artifact of the enhanced ionic strength (I = 0.122 M) that enter the activation corrections.

2. These results are used in the PowerPoint presentation.

3. Due to the small amount of Na and DIC the two aqueous complexes, NaHCO3 and NaCO3-, do not play any role at all.