Step 1: Statement of Henry’s Law.
Henry’s Law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the surface of the liquid.
Mathematically, it is expressed as:
p = kH x
where p = partial pressure of the gas,
kH = Henry’s law constant,
x = mole fraction of the gas in the solution.
This means that when the pressure of a gas increases, its solubility in the liquid also increases, provided the temperature remains constant.
Step 2: Daily-Life Application 1 – Carbonated Beverages.
Soft drinks and soda water are prepared by dissolving carbon dioxide gas in water under high pressure. When the bottle is opened, the pressure decreases and the dissolved CO2 escapes in the form of bubbles. This happens according to Henry’s Law.
Step 3: Daily-Life Application 2 – Scuba Diving.
While scuba diving, divers breathe air at high pressure under water. Due to high pressure, more nitrogen dissolves in their blood. If a diver comes to the surface too quickly, the pressure suddenly decreases and nitrogen bubbles form in the blood, causing a dangerous condition called “the bends”. To prevent this, divers ascend slowly and use special gas mixtures.
Conclusion.
Thus, Henry’s Law explains how the solubility of gases changes with pressure and has important applications in everyday life such as in soft drinks and scuba diving.