A scientist looking to remove oxygen from above a liquid sample pumps nitrogen into a sealed compartment to displace the oxygen, then places his liquid sample into the compartment. If the nitrogen pressure (partial pressure) was 1.8 atm, what would be the concentration of dissolved nitrogen gas if the Henry’s Law constant for nitrogen gas was 6.8 × 10-4 M atm-1 at this temperature?

1.2 × 10^-3 M

Explanation:

Henry's law law states that; once the temperature is constant, the amount of a given mass of gas that is dissolved in a particular type and volume of solvent is directly proportional to the partial pressure of that gas in equilibrium with the solvent.

From Henry's law;

Cg= K × Pg

Where;

Cg = concentration of gas

K= constant of Henry's law

Pg= partial pressure of the gas

Cg= 6.8 × 10^-4 M atm^-1 × 1.8 atm

Cg = 1.2 × 10^-3 M

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