The solubility of nitrogen in water exposed to the atmosphere,where the partial pressure of nitrogen is 593 mm,is 5.3 × 10^-4 M.At the same temperature,what would be the solubility of pure nitrogen,at a pressure of 760 mm? A)4.1 × 10^-4 M B)6.8 × 10^-4 M C)1500 M D)2400 M E)none of the above

Question

Quizplus · Accepted Answer

The solubility of a gas is directly proportional to the partial pressure of the gas above the liquid. Therefore, we can use the following equation:

Solubility1/Solubility2 = Partial pressure1/Partial pressure2

where Solubility1 is the solubility of nitrogen in water at a partial pressure of 593 mm, and Solubility2 is the solubility of pure nitrogen at a pressure of 760 mm.

Substituting the known values:

5.3 × 10^-4 / Solubility2 = 593 / 760

Solving for Solubility2:

Solubility2 = 6.8 × 10^-4 M

Therefore, the answer is B.

The Solubility of Nitrogen in Water Exposed to the Atmosphere,where