Alkalinity or ATis a measure of the ability of a solution to neutralize acids to the equivalence point of carbonate or bicarbonate.Alkalinity is closely related to the acid neutralizing capacity (ANC) of a solution and ANC is often incorrectly used to refer to alkalinity. The alkalinity is equal to the stoichiometricsum of the basesin solution. In the natural environment carbonate alkalinity tends to make up most of the total alkalinity due to the common occurrence and dissolution of carbonate rocks and presence of carbon dioxide in the atmosphere.Other common natural components that can contribute to alkalinity include borate, hydroxide, phosphate, silicate, nitrate, dissolved ammonia, the conjugate bases of some organic acidsand sulfide. Solutions produced in a laboratory may contain a virtually limitless number of bases that contribute to alkalinity. Alkalinity is usually given in the unit mEq/L (milliequivalent per liter). Commercially, as in the pool industry, alkalinity might also be given in the unit ppm or parts per million.
Total alkalinity is the measure of the amount of alkaline buffers (primarily carbonates and bicarbonates) in your water.These alkaline substances buffer the water against sudden changes in pH. Total alkalinity is considered the key to water balance. It is the first parameter you should balance when making routine adjustments to your water.
If you neglect to check the total alkalinity in your pool or spa, you may have trouble balancing the pH. You may also notice that pH fluctuates suddenly despite your best efforts to keep it in the ideal range. If the alkalinity is too low, anything introduced to the water will have an immediate impact on pH.Abrupt shifts in pH can cause scaling or corrosion of metal equipment and fixtures as well as other problems. When the total alkalinity is high, the pH has a tendency to drift upward, causing scale to form.
Raw Water:
| M-alkalinity as CaCo3 | mg/l | 160 |
When the total alkalinity is too low, add sodium bicarbonate. If the total alkalinity is too high, you can lower it by using muriatic acid or sodium bisulfate.
Maintaining an ideal level of alkalinity will protect your pool or spa and its equipment from the harmful effects of sudden pH fluctuations. Think of the alkalinity as training wheels: it keeps the pH in balance without allowing it to tip too far to either side. Of course the pH can still drift upward or downward, but that change will happen gradually as long as the alkalinity falls within the ideal range. The ideal range of total alkalinity for pools and spas is between 80 and 120 ppm (mg/L).
When the total alkalinity is too low, add sodium bicarbonate. If the total alkalinity is too high, you can lower it by using muriatic acid or sodium bisulfate.
For more detailed advice on the specific chemical treatment for your pool or spa, contact your dealer.
Alkalinity is sometimes incorrectly used interchangeably with basicity. For example, the pH of a solution can be lowered by the addition of CO2.This will reduce the basicity; however, the alkalinity will remain unchanged
Theoretical treatment of alkalinity
In typical groundwater or seawater the measured alkalinity is set equal to:
AT = [HCO3−]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T + 2[PO4−3]T + [HPO4−2]T+ [SiO(OH)3−]T− [H+]sws− [HSO4−]
AT = [HCO3−]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T + 2[PO4−3]T + [HPO4−2]T+ [SiO(OH)3−]T− [H+]sws− [HSO4−]
(Subscript T indicates the total concentration of the species in the solution as measured. This is opposed to the free concentration, which takes into account the significant amount of ion pair interactions that occur in seawater.)
Alkalinity can be measured by titrating a sample with a strong acid until all the buffering capacity of the aforementioned ions above the pH of bicarbonate or carbonate is consumed. This point is functionally set to pH 4.5. At this point, all the bases of interest have been protonated to the zero level species, hence they no longer cause alkalinity. For example, the following reactions take place during the addition of acid to a typical seawater solution:
HCO3−+ H+→ CO2 + H2O
CO3−2+ 2H+→ CO2 + H2O
B(OH)4−+ H+→ B(OH)3 + H2O
OH−+ H+→ H2O
PO4−3+ 2H+→ H2PO4−
HPO4−2+ H+→ H2PO4−
[SiO(OH)3−] + H+→ [Si(OH)40]
It can be seen from the above protonation reactions that most bases consume one proton (H+) to become a neutral species, thus increasing alkalinity by one per equivalent. CO3−2 however, will consume two protons before becoming a zero level species (CO2), thus it increases alkalinity by two per mole of CO3−2. [H+] and [HSO4−] decrease alkalintiy, as they act as sources of protons. They are often represented collectively as [H+]T.
Alkalinity is typically reported as mg/L as CaCO3. This can be converted into mill Equivalents per Liter (mEq/L) by dividing by 50 (the approximate MW of CaCO3/2).
Alkalinity is typically reported as mg/L as CaCO3. This can be converted into mill Equivalents per Liter (mEq/L) by dividing by 50 (the approximate MW of CaCO3/2).
Example problems
Sum of contributing species
The following equations demonstrate the relative contributions of each component to the alkalinity of a typical seawater sample. Contributions are in μmol.kg−soln-1 and are obtained from A Handbook of Methods for the analysis of carbon dioxide parameters in seawater "[1],"(Salinity = 35, pH = 8.1, Temperature = 25°C).
AT = [HCO3−]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T + 3[PO4−3]T + [HPO4−2]T+ [SiO(OH)3−]T− [H+] − [HSO4−] − [HF]
Phosphates and silicate, being nutrients, are typically negligible. At pH = 8.1 [HSO4−] and [HF] are also negligible. So,
AT = [HCO3-]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T− [H+]
AT = 1830 + 2*270 + 100 + 10 − 0.01
AT = 2480 μmol.kg−soln-1
AT = [HCO3−]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T + 3[PO4−3]T + [HPO4−2]T+ [SiO(OH)3−]T− [H+] − [HSO4−] − [HF]
Phosphates and silicate, being nutrients, are typically negligible. At pH = 8.1 [HSO4−] and [HF] are also negligible. So,
AT = [HCO3-]T + 2[CO3−2]T+ [B(OH)4−]T + [OH−]T− [H+]
AT = 1830 + 2*270 + 100 + 10 − 0.01
AT = 2480 μmol.kg−soln-1
Addition of CO2
The addition (or removal) of CO2 to a solution does not change the alkalinity. This is because the net reaction produces the same number of equivalents of positively contributing species (H+) as negative contributing species (HCO3- and/or CO3--).
At neutral pH's:
CO2 + H2O → HCO3− + H+
At high pH's:
CO2 + H2O → CO3−2 + 2H+
At neutral pH's:
CO2 + H2O → HCO3− + H+
At high pH's:
CO2 + H2O → CO3−2 + 2H+
Dissolution of carbonate rock
Addition of CO2 to a solution in contact with a solid can affect the alkalinity, especially for carbonate minerals in contact with groundwater or seawater . The dissolution (or precipitation) of carbonate rock has a strong influence on the alkalinity. This is because carbonate rock is composed of CaCO3 and its dissociation will add Ca+2and CO3−2 into solution. Ca+2 will not influence alkalinity, but CO3−2 will increase alkalinity by 2 units.
P ALKALINITY
Alkalinity in trisodium Phoshate
P alkalinity
V1* 40*N*100/w *1000
W= material of aliquot
N= Normality of HCL