Carbon Dioxide Equation in Water:

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The Carbon Dioxide - Bicarbonate Equilibrium CO2 dissolves rapidly in water, and reacts with water to form carbonic acid, which rapidly ionizes to form bicarbonate and carbonate.

Dissolved CO2 causes water to become slightly acidic; the current atmospheric levels of CO2 are sufficient, in the absence of other factors, to bring the pH of pure water from a neutral pH of 7.0 to a pH of 5.7, which is roughly the same pH as normal rain.

However, the oceans contain many pH buffers, including borate, phosphate, and silicate, which tend to counteract this effect, while acid rain increases it. The pH of sea water today is typically between 7.36 and 8.4, which is slightly basic. Buffering by bicarbonate and other ions is important in maintaining the correct pH; depletion of CO2 in lakes by eutrophication can raise the pH as high as 9.0.

Living cells contain the enzyme carbonic anhydrase, which greatly accelerates the reaction in both directions, helping cells to get rid of excess CO2. Bicarbonate is also sequestered by plants and animals to form calcium carbonate. The vast majority of the earth's carbon is locked in the form of limestone and other carbonate rocks.

 

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