The solubility of $CO_{2}$ in water can be accounted for by

Analyze the question: CO₂ is a nonpolar molecule (linear, O=C=O, with the two C=O dipoles cancelling). Water is polar. We need to find the interaction that explains why CO₂ dissolves in water.

Concept: Solubility depends on the intermolecular attractions between solute and solvent.

• Polar solutes dissolve in water through dipole-dipole attraction or hydrogen bonding.
• Nonpolar solutes can dissolve only slightly, through weak attractions: the permanent dipole of water induces a temporary dipole in CO₂ (dipole-induced dipole). This is a type of Van der Waals force.

Working through the options:

• A. Van der Waal's forces: Water's polar molecules induce a temporary dipole in the CO₂ molecule, giving weak attractions. This is the physical dissolution of CO₂. ✔
• B. Ionic attraction: CO₂ is not ionic, so this is wrong.
• C. Dipole attraction: CO₂ has no net permanent dipole, so permanent dipole-dipole attraction cannot apply. This is the tempting distractor.
• D. Covalent bonding: A small fraction of CO₂ does react with water to form H₂CO₃ (carbonic acid), but that is a chemical reaction, not solubility as such. Dissolving itself does not involve forming covalent bonds between CO₂ and water.

Answer: The solubility of CO₂ in water is accounted for by Van der Waal's forces, which is option A.

Tip: Nonpolar gas in water means weak Van der Waals (induced dipole) forces. Permanent dipole-dipole attraction needs both molecules to be polar. Always check the molecule's shape first. CO₂ is symmetrical, so its dipoles cancel.