Final answer:
Henry's Law states that gas solubility in a liquid is directly proportional to the gas's partial pressure above the liquid. The law has limitations, including that it's not accurate with association/dissociation of gases, at high pressures, or near solvent saturation.
Step-by-step explanation:
Henry's Law Explanation: Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This relationship can be represented by the equation C = kH*P, where C is the concentration of dissolved gas at equilibrium, P is the partial pressure of the gas, and kH is the Henry's law constant, which varies for each combination of gas, solvent, and temperature.
Limitations of Henry's Law-
However, Henry's Law has its limitations. It is most accurate when:
- The solute is a gas.
- The concentration of the gas is relatively low.
- No chemical reaction occurs between the gas and the solvent.
- The system is at constant temperature.
Henry's Law does not hold well when the gas undergoes association or dissociation in the solvent, or at high pressures where the gas may not behave ideally. It also does not apply when the solvent is near saturation or precipitates out of solution.