The solubility of a gas in a liquid increases with increasing pressure. To understand the above statement, consider a familiar example: cola. In cola and other soft drinks, carbon dioxide gas remains dissolved in solution as long as the can or bottle remains pressurized. As soon as the lid is opened and pressure is released, the CO2 gas is much less soluble and escapes into the air. The relationship between pressure and the solubility of a gas is expressed by Henry's law: C=kP, where C is concentration in M,k is the Henry's law constant in units of mol/Latm, and P is the pressure in atm. Note: Since temperature also affects the solubility of a gas in an liquid, the Henry's law constant is specific to a partcular gas at a particular temperature. What pressure is required to achieve a CO2 concentration of 8.20102 at 20C