I would like to use a liquid solvent for some experimentation with a carbon dioxide solubility as low as possible under usual pressure and temperature conditions (say, $\pu{1 atm}$ and $\pu{293 K}$).
Until then, I was unable to find much information on the topic:
A study of $\ce{CO2}$ solubility in water and seawater by Weiss [1], indicating that $\ce{CO2}$ is less soluble in saline water than in pure water.
Publications concerning several organic solvent (acetone, cyclohexane, ethanol, methanol, etc.), a sum-up in IUPAC SDS Vol 50 [2]. To the naked eye, it seems that all of them can dissolve much more $\ce{CO2}$ than water, being poor candidates to answer my needs.
Publications concerning olive, linseed or other origin oils (see Simon and Gutknecht [3] for instance). However such fats seems to also have a higher solubility coefficient than water.
I do not know if such liquid does exist, but it would be great. Up to now, my best candidate is salty water.
References
- Weiss, R. F. Carbon Dioxide in Water and Seawater: The Solubility of a Non-Ideal Gas. Marine Chemistry 1974, 2 (3), 203–215. https://doi.org/10/cb6n2j.
- Carbon Dioxide in Non-Aqueous Solvents at Pressures Less than 200 kPa; Fogg, P. G., Clever, H. L., Eds.; Solubility data series; Pergamon Press: Oxford, 1992. ISBN 978-0-08-040495-0. PDF
- Simon, S. A.; Gutknecht, J. Solubility of Carbon Dioxide in Lipid Bilayer Membranes and Organic Solvents. Biochimica et Biophysica Acta (BBA) - Biomembranes 1980, 596 (3), 352–358. https://doi.org/10/bj647m.
Update
I understand the "like dissolves the like"[1] rule of thumb so that a highly polar solvent would be the worst for a non-polar molecule such as $\ce{CO2}$. Water as a solvent would then be the best choice (possibly salted to further reduce its $\ce{CO2}$ solubility) for my needs.
But as Rolf pointed out, the dissociation of $\ce{CO2}$ into carbonate ions also happens and might increase its solubility. For such reasons an aprotic solvent could be useful.
However, when comparing between water (molar fraction 0.00061) which is a strongly polar (dielectric constant: 80 and dipole moment 1.85$~$D) but protic solvent and dimethyl sulfoxide (molar fraction 0.0091[2]) which is also polar (dielectric constant: 47 and dipole moment 3.96$~$D) but aprotic solvent, dimethyl sulfoxide as a higher solubility for carbon dioxide than water.
What can be the reasons for such unexpected outcome? Are my reasonings and assumptions correct or am I flawed in my thinkings?
References
- Polar Protic? Polar Aprotic? Nonpolar? All About Solvents. - Master Organic Chemistry. https://www.masterorganicchemistry.com/2012/04/27/polar-protic-polar-aprotic-nonpolar-all-about-solvents/
- Li Hua & Chen Wanren, 2005, Solubility of dilute SO2 and CO2 in dimethyl sulfoxide, Physics and Chemistry of Liquids, 43:3, 289-298, DOI: 10.1080/00319100500083583