Water chemistry

I give you a little about water chemistry

Bicarbonate equilibrium:

• One of the most important acid / base systems in water ..

Control the pH of most water ..
Water is exposed to carbon dioxide (CO2) from the atmosphere and dissolved to give H2CO3

As follows:

CO2 (g) + H20 ⇔ CO2 (aq) Gas dissolution

CO2 (aq) + H20 ⇔ H2CO3 Carbonic acid
formation

Carbonic acid breaks down in water in two steps:

As follows:

-Carbonic acid donates one proton (H +) to create bicarbonate HCO3

H2CO3 ⇔ H + + HCO3- 1

Bicarbonate donates a proton (H +) to form carbonate CO3-2

2-HCO3- ⇔ H + + CO3

• The constant stability of these reactions at 25 degrees Celsius as follows:

CO2 (aq) + H20 ⇔ H2CO3 pKH = 1.46
H2CO3 + H + + HCO3- pK1 = 6.35
HCO3-⇔ H + + CO3-2 pK2 = 10.33

• Annex Picture showing the distribution of the common pH of natural water ...

Reference

Water Chemistry 3 Book
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