Finding the Concentration of H3CO2 in a CO2+H2O reaction.

[miniradman]

1. Find the equlibrium constant if there is 0.030moles/L of Carbon Dioxide going in the forward direction and water is in excess to form Carbonic Acid (H2CO3)

Homework Equations

[products]/[reactants] = K

The Attempt at a Solution

I'm trying to figure out how Carbon Dioxide in the atmosphere will affect the chemistry of the oceans. From my research I've found that CO2_(g) = CO2_(aq) in water is 1.45 g/L where I deduced a equilbrium of 0.030 moles/L. My next step is where I have to figure out how much Carbonic Acid is made (CO2 + H₂0 = H₂CO₃) when I know that the equlibrium for the forward direction is 0.039 L/mol. So:

[H₂CO₃]/[CO₂][H₂O]

which based on what I know translates to
[H₂CO₃]/(0.03)[[H₂O] = 0.039L/mol

However, L/mol is not the same as mol/L and I need to find the concentration of [H₂CO₃] because after that I need to figure out the K values for H₂CO₃ = H⁺+HCO₃
and
HCO₃ = H⁺+CO₃
equilibriums

*sorry, I do apologize but I'm not sure how to get the "reversible reaction" symbol on the physics forums, so I just used an "=" sign *

ps. I was read on wikipedia that the solubility of Carbon Dioxide is 1.45g/L at 25 degrees C at 100kpa. The pressure, is that including the rest of the atmosphere? or just the carbon dioxide alone? because I've calculate the partial pressure of the CO₂to be 11.6139 pa at sea level.

 

[miniradman]

Should I give anymore detail?
More explanation?
More of my working Out?
was the layout incorrect?
... or do people just don't like me...

 

[Borek]

There are thick books written on the subject. Just carbonic acid is not enough to analyze anything, although you can be sure increasing partial pressure of CO₂ lowers water pH. Google for seawater chemistry.

 

[chemisttree]

Yes, it's a http://aslo.org/lo/toc/vol_18/issue_6/0897.pdf