When carbon dioxide dissolves in water, essentially all of itreacts to form carbonic acid, H2CO3.
CO2(g) + H2O(l) <---> H2CO3(aq)
The carbonic acid can then dissociate into H+ and bicarbonateions,
H2CO3(aq) <----> H+(aq) + HCO-3(aq).
Consider a body of otherwise pure water that is in equilibrium withthe atmosphere near sea level, where the partial pressure of carbondioxide is 3.4x10^-4 bar (or 340 ppm). Calculate the molality ofcarbonic acid and of bicarbonate ions in the water, and determinethe pH of the solution. Note that even "natural" precipitation issomewhat acidic.
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Here is some data from the back of the book that I think isimportant, anything else that is needed let me know.
G(CO2)(g) = -394.36kJ
G(H2O)(l) = -237.13kJ
G(H2CO3)(aq) = -623.08kJ
G(H+)(aq) = 0kJ
G(HCO3-)(aq) = -586.77kJ
If anybody has any idea how to do this problem, any input isappreciated.
When carbon dioxide dissolves in water, essentially all of itreacts to form carbonic acid, H2CO3.
CO2(g) + H2O(l) <---> H2CO3(aq)
The carbonic acid can then dissociate into H+ and bicarbonateions,
H2CO3(aq) <----> H+(aq) + HCO-3(aq).
Consider a body of otherwise pure water that is in equilibrium withthe atmosphere near sea level, where the partial pressure of carbondioxide is 3.4x10^-4 bar (or 340 ppm). Calculate the molality ofcarbonic acid and of bicarbonate ions in the water, and determinethe pH of the solution. Note that even "natural" precipitation issomewhat acidic.
-------------------------------------------
Here is some data from the back of the book that I think isimportant, anything else that is needed let me know.
G(CO2)(g) = -394.36kJ
G(H2O)(l) = -237.13kJ
G(H2CO3)(aq) = -623.08kJ
G(H+)(aq) = 0kJ
G(HCO3-)(aq) = -586.77kJ
If anybody has any idea how to do this problem, any input isappreciated.