Estimate the Henry’s constant for the solubility of this compound in water at 25°C.

Question

A flask containing 706 mL of water at 25°C was exposed to 0.368 mmHg of a gaseous compound until a solubility equilibrium was established. The measured equilibrium concentration of the dissolved compound was 0.104 M.

Answer 1

Henry's Law:

P = KC

P = partial pressure of gas = 0.368 mm Hg

K = Henry's constant = ?

C = concentration = 0.104 M

K = P/C = 0.368 mm Hg / 0.104 M

K = 3.54mm Hg M^-1 or 3.54 mm Hg*L*mole^-1