Carbon Water

What is the equilibrium concentration of carbon dioxide in water that is in contact with air at 25 °C and 0.98?

What is the equilibrium concentration of carbon dioxide in water that is in contact with air at 25 °C and 0.982 atm. The mole fraction of CO2 in air is 3.01 × 10-4. The Henry’s law constant for carbon dioxide is 4.48 × 10-5 M/mm Hg.

I have no idea HOW to do answer this problem, a little help please?

For starters, K is not given in particularly useful units. You could look up the K for CO2 with more useful units or simply convert as I have done below:

K = 4.48 * 10-5 M/mm Hg. One atm = 760 mm, and I prefer to use mol/L for big M, so

K = 4.48 * 10-5 mol/L mm x 760 mm/1 atm, so

K = 0.0341 mol/L atm.

To use Henry's Law, we also need the partial pressure of CO2. This is given by the mole fraction times the total pressure.

p(CO2) = x(CO2) * P(total), or

p(CO2) = (3.01 x 10-4) * 0.982 atm

p(CO2) = 2.96 x 10-4 atm.

Now we have everything we need to solve for the CO2 conc with Henry's Law.

[CO2aq] = p(CO2) * K

[CO2aq] = 2.96 x 10-4 atm * 0.0341 mol/L atm

[CO2aq] = 1.01 x 10-5 mol/L

Note that by doing that conversion of K, we end up with the correct units. For more info, see the article in wikipedia. Maybe this helps?

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