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23 Nov 2019
When carbone dioxide "dissolves" in water, essentially all of itreacts to form carbonic acid, H2CO3:
CO2(g)+H2O(l)<----> H2CO3(aq)
The carbonic acid can then be dissociate into H+ and bicarbonateions,
H2CO3(aq) <----> H+(aq)+HCO3-(aq).
Consider a body of otherwise pure water (or perhaps a raindrop)that is in equilibrium with the atmosphere near sea level, wherethe partial pressure of carbon dioxide is 3.4*10^-4 bar (or 340parts per million). Calculate the molality of carbonic acid and ofbicarbonate ions in the water, and determin the pH of the solution.Note that even "natural" precipitation is somewhat acidic
When carbone dioxide "dissolves" in water, essentially all of itreacts to form carbonic acid, H2CO3:
CO2(g)+H2O(l)<----> H2CO3(aq)
The carbonic acid can then be dissociate into H+ and bicarbonateions,
H2CO3(aq) <----> H+(aq)+HCO3-(aq).
Consider a body of otherwise pure water (or perhaps a raindrop)that is in equilibrium with the atmosphere near sea level, wherethe partial pressure of carbon dioxide is 3.4*10^-4 bar (or 340parts per million). Calculate the molality of carbonic acid and ofbicarbonate ions in the water, and determin the pH of the solution.Note that even "natural" precipitation is somewhat acidic
