Chapter 13.5, Problem 1RC

Interpretation Introduction

Interpretation:

The gases that has greatest Henry’s Law constant in water at given temperature should be identified.

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 $\text{(mol/L}\text{.atom)}$

Like dissolves like principle: ‘Like dissolves like’ principle says that polar compounds including ionic compound should be more soluble in polar solvent.  Likewise, non–polar compound should be more soluble in non–polar solvent. Other hand, compounds with similar intermolecular force (hydrogen bonding is the principal intermolecular force) capability to soluble in one another because solute-solvent interactions are similar signification to the solute-solute interaction.

Note: Polar solvent should be having O atoms and N atoms with lone pairs.

Example, Methanol and water both are polar molecules. Methanol dissolves in water but Hexane does not dissolved in water because Hexane is non polar.

Polar molecule: Polar molecules have large dipole moments.

Non-Polar molecules: Non-polar molecules have bonded atoms with similar electronegativity results to have zero dipole moments.

Solubility is the quantity of solute (solid, liquid or gas) that will dissolve in a given amount of solvent (solid, liquid or gas) at definite temperature and pressure.  Solubility depends on the physical and chemical property of solvent, solute and concentration of the solution.