As the solubility of gas in liquid decrease with increase in temperature, is there any possibilities to increase the CO2 solubility in the water around 50-80 C?
One way to look at this is through Henry's Law. According to Henry's Law
Kp/Kh = C, Where "p" is partial pressure, Kh is Henry constant and C is concentration. To increase the solubility, either partial pressure has of CO2 has to be increased or Kh has to be decreased. Kh at a given temperature can be roughly estimated as follows
Kh = Kho exp [-C * (( 1/T) - (1/To))]
Kho - is henry constant at reference temperature (298K)
To - Reference temperature (298K)
C - Temperature dependent constant
Since Kh is a temperature dependent constant, to increase the concentration, increase partial pressure of CO2 would be a solution. This can be done by increasing the total pressure or increasing the mass fraction of CO2
Reference-
https://chemengineering.wikispaces.com/Henry%27s+Law
You may possibly want to check the following paper: http://www.sciencedirect.com/science/article/pii/S0009254104004929
Dear Kiran Subramani
Please find the paper suggested by Mr. Carlos Araújo Queiroz as an attachment.
Article Energizing the CO2 utilization by Chemo-enzymatic approaches...
Dear Kiran Subramani
Take a look at the curves for fractional amount in CO2-Water equilibrium curves. At acidic pH's, CO2 is freely existent in the water as aqueous CO2 gas in the solution. By increasing the temperature, CO2 solubility decreases and you can see CO2 gas bubbles on the surfaces of the water in your test container. Since, you are looking to conduct your experiment at high temperatrures with higher CO2 solubility (Which ends in higher bicarbonate ions or higher carbonate ions in the solution), you need to increase pH value and i think this is the only way.
But if you want to have higher temperatures and higher CO2 solubility in acidic conditions, i think it is impossible based on Henry's law for gas solubilities and also equilibrium curves for CO2-(HCO3-)-(CO3 2-) systems.
Best regards,
Askar
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