Solubility laws and polarity: Identify the incorrect statement regarding Raoult’s law, molecular polarity, and typical properties of nonpolar compounds.

Introduction / Context:
Understanding when Raoult’s law or Henry’s law applies is crucial for predicting solubilities and vapour–liquid equilibria. Polarity also governs miscibility and electrical properties of substances in solutions and mixtures.

Given Data / Assumptions:

• Raoult’s law applies best to ideal solutions where solvent–solute interactions resemble solvent–solvent interactions.
• Gas solubility in liquids at low concentrations generally follows Henry’s law.
• Symmetry often correlates with nonpolarity (e.g., CH4, CCl4).

Concept / Approach:
Polar gases in nonpolar solvents rarely behave ideally; their solubility follows Henry’s law, not Raoult’s. Nonpolar molecules tend to be nonconductive and do not ionise. Many hydrocarbons are indeed nonpolar.

Step-by-Step Solution:

Verification / Alternative check:
Experimental solubility data for polar gases (e.g., NH3, SO2) in nonpolar solvents deviate strongly from Raoult’s ideal-solution prediction and are handled via Henry’s constants.

Why Other Options Are Wrong:

• (b), (c), and (d) reflect accepted chemical principles regarding symmetry, hydrocarbon polarity, and electrical properties of nonpolar compounds.

Common Pitfalls:
Misapplying Raoult’s law to dilute gas solubility problems; remember Raoult’s is for solvent partial pressures in liquid mixtures, not for dilute gases dissolving in liquids.

Final Answer:
Raoult's law holds good for the solubility of polar gases in non-polar liquids.