Cue Column | Note Column

Formula? | $p = K_H \times x$ where p = partial pressure of gas above solution, K_H = Henry's law constant, x = mole fraction of gas in solution

What is K_H? | Henry's law constant (units: atm or bar). It is CHARACTERISTIC of gas-solvent pair. Higher K_H = lower solubility at same pressure.

Temperature effect? | K_H INCREASES with temperature → x decreases for same p → gas becomes LESS soluble in hot liquids

Application 1: | Carbonated beverages: Bottled under high $CO_{2}$ pressure. On opening, pressure drops → $CO_{2}$ solubility decreases → fizzing (bubbles form)

Application 2: | Deep sea divers ("the bends"): At depth, high pressure dissolves $N_{2}$ in blood. Rapid ascent → pressure drops → $N_{2}$ bubbles form in tissues and blood vessels → decompression sickness. Prevention: slow ascent, use He-$O_{2}$ mixture.

Limitations: | Henry's law applies only to dilute solutions of gases that do NOT react with or dissociate in the solvent (e.g., $CO_{2}$ technically reacts, but law approximately holds at moderate pressures).

Summary

Henry's law: p = K_H × x. Gas solubility decreases with temperature. High pressure increases gas solubility. Both carbonation and the bends are direct applications of Henry's law.