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Carbonate System Alkalinity

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Carbonate System Alkalinity

Lecture 21

- TOTH is the total amount of component H+, rather than the total of the species H+.
- Every species containing H+ contributes positively to TOTH while every species formed by subtracting H+ contributes negatively to TOTH.

- For pure water:TOTH = [H+] - [OHâ€“]
- Of course in pure water [H+] = [OHâ€“] so TOTH = 0.

- Now we dissolve CaCO3 to our solution and chose Ca2+ and CO32- as components.
- In near neutral pH, almost all the CO32- will react to form HCO3â€“:
CO3+ + H2O = HCO3- + OHâ€“

- some Ca2+ (though generally not much) will form Ca(OH)+, so our mole balance equation will be
TOTH = [H+] - [OHâ€“] + [HCO3â€“] - [Ca(OH)+]

- In near neutral pH, almost all the CO32- will react to form HCO3â€“:
- Since we have not added [H+], TOTH remains 0.

- Now we dissolve CO2 in our solution:
H2O + CO2â‡‹ H2CO3

- In near neutral pH, almost all the H2CO3 will react to form HCO3â€“:
H2CO3 = HCO3- + H+

- If we chose CO2 as our component,
HCO3â€“ = CO2 + H2O - H+

TOTH = [H+] - [OHâ€“] - [HCO3â€“]

- In near neutral pH, almost all the H2CO3 will react to form HCO3â€“:
- This time HCO3- contributes negatively.
- Every species containing H+ contributes positively to TOTH while every species formed by subtracting H+ contributes negatively to TOTH.
- How we write the TOTH equation depends on how we defined components.

?

- Remember our problem set problem on the dissolution of galena:
PbS + 2H+ â‡‹ Pb2+ + H2S

- We used mass balance to solve this.
- A number of other reactions are possible:
H2S â‡‹ H+ + HSâ€“

HSâ€“ â‡‹ H+ + S2-

Pb2+ + S2â€“ â‡‹ PbSaq

- However, we may still write a conservation equation
- Î£S = PbSaq + H2S + HSâ€“ + S2â€“
- And if galena is the only source of Pb and S, then
Î£Pb = Î£S

- Mass balance, or conservation, equations can be useful constraints on our system. However, they often come with caveats, like the above (galena the only source of Pb and S).

- Aqueous solutions are always electrically neutral (period, no caveats).
- Thus the following constraint always holds:
- Often, however, charge and mass conservation equations end up being the same (since we can only add electrically neutral substances to our solution).

- We now turn our attention to carbonate.
- Water at the surface of the Earth inevitably contains dissolved CO2, either as a result of equilibration with the atmosphere or because of respiration by organisms. CO2 reacts with water to form carbonic acid:
CO2+ H2O â‡„ H2CO3

- Some of the carbonic acid dissociates to form bicarbonate and hydrogen ions:
H2CO3â‡„ H+ + HCO3â€“

- Some of the bicarbonate will dissociate to an additional hydrogen ion and a carbonate ion:
HCO3â€“â‡„ H+ + CO32â€“

- We can write three equilibrium constant expressions for these reactions:

- Another important reaction in the carbonate system is precipitation of carbonate minerals (mainly calcite) in veins in rocks, in soils (caliche), as shells, on your faucet, etc., and dissolution of carbonate, as in limestone caverns and sinkholes:
CaCO3 â‡„ Ca2+ + CO32-

- Suppose now that we have a known fixed total carbonate activity, e.g.,
- Î£CO2 = H2CO3 + HCO3â€“+ CO32-

- Combining this with our equilibrium constant expressions, we can solve for the species activities as a function of pH, e.g.:

- If we have a solution with fixed Î£CO2 that is closed and contains no other dissolved species, the pH is also fixed.
- We can calculate pH by simultaneously solving charge and mass balance equations together with equilibrium constant expressions:
- (note typo in book -missing exponent 2)

- We can guess our solution will be acidic, in which case we can ignore CO32â€“ and OHâ€“, we means we can drop terms containing K2 and Kw. Therefore:
- This illustrates a key part of solving such equations â€“ knowing when and how to simplify them by neglecting terms.

- Particularly simple relationships occur when the activities of two species are equal.
- These are determined by equilibrium constant expressions:
- CO2 E.P.:
[H+] = [HCO3â€“]

- Bicarbonate E.P.
- [CO32â€“] = [H2CO3]
- Carbonate E.P.
- [OHâ€“] = [HCO3â€“]
- Two others [H2CO3] = [HCO3â€“], [HCO3â€“] = [CO32-]

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- Conservative ions are those whose concentrations are not affected by changes in pH, temperature, and pressure, assuming no precipitation or dissolution.
- In natural waters, the principal conservative ions are Na+, K+, Ca2+, Mg2+, Clâ€“, and .
- These ions are conservative because they are fully dissociated from their conjugate acids and bases over the normal range of pH of natural waters.

- Non-conservative ions are those that will undergo association and dissociation reactions in this pH range. These include the proton, hydroxyl, and carbonate species as well as B(OH)4â€“, H3SiO4â€“, HSâ€“, NH4OH, phosphate species, and many organic anions.
- Virtually all the non-conservative species are anions, the two principle exceptions being H+ and NH4OH.

- Alkalinity is an important and fairly readily measured property of natural waters.
- Alkalinity is a measure of acid-neutralizing capacity of a solution and is defined as the sum of the concentration (in equivalents) of bases that are titratable with strong acid.
- Mathematically, we define alkalinity as the negative of TOTH when the components are the principal species of the solution at the CO2equivalence point (which carbonate species there?) The acidity can be defined as the negative of alkalinity, and hence equal to TOTH.

- Consider a solution containing a fixed total dissolved concentration of CaCO3. At the CO2 equivalence point, H2CO3 is the principal carbonate species, so we choose our components as H+, H2O, CO2, and Ca2+.
H2CO3= H2O + CO2

HCO3-=H2O + CO2-H+

CO32-= H2O + CO2-2H+

- The proton mole balance equation is then:
TOTH = [H+] - [HCO3-] -2[CO32-] -[OHâ€“]

- The alkalinity is then:
Alk= -TOTH = -[H+] + [HCO3-] + 2[CO32-] + [OHâ€“]

- The above is also the carbonate alkalinity: the alkalinity due to the presence of carbonate ions.
- In many solutions, carbonate alkalinity is very nearly equal total alkalinity. To be clear, we sometimes call the alkalinity as defined previously Total Alkalinity.

- Charge balance requires:
- Î£cations - Î£ anions = 0
- Î£cons. cations-Î£cons. anions+Î£non-cons. cations-Î£non-cons. anions = 0
- Î£cons. cations-Î£cons. anions= -Î£non-cons. cations+Î£non-cons. anions
- The right hand side is equal to the alkalinity:
- Alk = Î£cons. cations-Î£cons. anions
- = -Î£non-cons. cations+Î£non-cons. anions
- This equation emphasizes an important point. The difference of the sum of conservative anions and cations is a conservative property(they cannot be changed except by the addition or removal of components).
- Since alkalinity is equal to this difference, alkalinity is also a conservative quantity (i.e., independent of pH, pressure and temperature). Thus total alkalinity is conservative, even though concentrations of individual species are not.

- In determining alkalinity, we need to correctly write the TOTH equation.
- To do so, we need to decide on a proper system of components (as usual, we want the minimum number of components) and then decide which species are formed by adding H+ and which are formed by subtracting H+.
- The Morel & Hering method is to produce a matrix-like table (a tableau) with species across the top and components listed vertically.
- Entries in the Tableau are the stoichiometric coefficient of each component needed to form each species.
- Consider a solution containing H3SiO4â€“, H4SiO4, B(OH)3, B(OH)4â€“, H2S, HSâ€“, HPO42-, H2CO3, HCO3â€“, CO32â€“, and, H+, and OHâ€“. We also recall that we always chose H2O as a component.

Alk = -TOTH = -{[H+] - [OH-] - [HCO3â€“] - 2[CO32-] - [HPO42-] - [H3SiO4-] - [HS-]}

- We have learned how to calculate alkalinity, but it can also be measured by titration.
- Titration is the process of progressively adding a strong acid or base to a solution until a specified pH, known as an end-point, is reached.
- In the case of the determination of alkalinity, this end-point is the CO2 equivalence point, as the definition suggests.
- The analytical definition of alkalinity is its acid neutralizing capacity when the end-point of the titration is the CO2 equivalence point.

- Consider a solution containing sodium carbonate (Na2CO3). Because the carbonate ion can act as a proton acceptor, Na2CO3is a base.
- We assume ideal behavior, complete dissociation, and a volume of solution large enough that the titration results in trivial dilution.

- The charge balance equation during the titration is:
[Na+] + [H+] = [Clâ€“] + [ HCO3â€“] + 2[CO32-] + [OHâ€“]

- Since the Clâ€“ concentration is conservative, it will be equal to the total amount of HCl added.

- Using equilibrium constant expressions to eliminate some species, e.g.,
- and noting mass balance requires 2[Na]=Î£CO2, we derive the following:

- This plot shows the how carbonate species in a 5 mM Na2CO3 solution change with pH as HCl is added during titration.
- Notice how the HCl curve flattens at the equivalence points - pH changes rapidly with small additions of HCl.
- This means we donâ€™t have to hit the pH of the E.P. with great precision to obtain the alkalinity.
- In practice, a solution indicator or pH meter would be used.

- The end-point is reached here at 10 mM HCl.

- In this example, titration yielded an alkalinity of 10 mM.
- Can we obtain the same result from calculation?
TOTH = [H+] - [OH-] - [HCO3â€“] - 2[CO32-]

- Charge balance is (before addition of HCl):
[Na+] + [H+] = [HCO3â€“] + 2[CO32-] + [OHâ€“]

- Solving the two equations, we find:
Alk = -TOTH = [Na+] = 10 mM