CBSE · Class 12 · Chemistry · SolutionsState Henry's law and explain its various applications. Also, discuss the limitations of Henry's law.

Statement of Henry's Law\nHenry's law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the liquid or solution. Mathematically, it is expressed as:

$$p = K_H \cdot x$$\nWhere $p$ is the partial pressure of the gas, $x$ is the mole fraction of the gas in the solution, and $K_H$ is Henry's law constant.

Applications of Henry's Law

1. Production of Carbonated Beverages: To increase the solubility of $CO_2$ in soft drinks and soda water, the bottles are sealed under high pressure.
2. Deep Sea Diving (Scuba Diving): Scuba divers breathe air compressed at high pressure underwater. Due to high pressure, the solubility of atmospheric gases like nitrogen and oxygen increases in blood. When divers surface slowly, pressure decreases, releasing dissolved gases and forming painful nitrogen bubbles known as 'bends'. To avoid this, tanks are diluted with helium.
3. Climb Climbers / High Altitudes: At high altitudes, the partial pressure of oxygen is low, leading to low concentrations of oxygen in the blood and tissues of climbers, causing a condition known as anoxia.

Limitations of Henry's Law

• The pressure of the gas should not be too high.
• The temperature should not be too low.
• The gas should not undergo any chemical dissociation or association in the solvent.