Chapter 13.5, Problem 1PE

Interpretation Introduction

Interpretation:

The molar concentration for oxygen in water at ${\text{25}}^{\text{o}}\text{C}$ for partial pressure $\text{0}\text{.22}\text{atm}$ should be calculated.

Concept introduction:

Henry’s law:

At constant temperature, amount of dissolved gas and volume of liquid proportional to the partial pressure of that gas in equilibrium with that liquid. This law applies most precisely for dilute solutions of a gas that does not react or dissociate with the solvent.

Henry’s law states that dissolved gases in liquid are directly proportional to the partial pressure of the gas over the solution.

$\text{c = kP}$

Where,

$\text{c}$ is molar concentration of dissolved gas $\text{(mol/L)}$

$\text{k}$ is proportionality constant

$\text{P}$ is partial pressure of the gas over the solution $\text{(mol/L}\text{.atom)}$