At 25 °C and 775 Torr, carbon dioxide has a solubility of 0.0347 M in water. What is its solubility at 25 °C and 1350 Torr?

Answer 1

Henry's Law:

C = kP

C = concentration = 0.0347 M

k = Henry's constant = ?

P = pressure = 775 torr

Solving for Henry's constant, we have ...

k = C/P = 0.0347 M / 775 torr

k = 4.48x10^-5 M / torr

Applying this constant to the new pressure, we can find the solubility:

C = kP

C = (4.48x10^-5 M / torr)(1350 torr)

C = 0.0605 M