Indicate the principal type of solute-solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute- solvent interaction: (a) \(\mathrm{KCl}\) in water, (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right),(\mathrm{c})\) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water.

In the given solutions, we have the following solutes and solvents: a) KCl in water b) CH2Cl2 in benzene (C6H6) c) Methanol (CH3OH) in water

For each solution, let's assess the interaction between the solute and the solvent: a) KCl is an ionic compound, and water is a polar solvent. Ionic compounds dissolved in polar solvents generally undergo ion-dipole interactions. b) CH2Cl2 is a polar molecule due to electronegativity difference between carbon and chlorine atoms, while benzene is a non-polar solvent. The type of interaction for this case is a dispersion interaction (weakest of the three types of van der Waals forces), between the polar CH2Cl2 molecules and the non-polar benzene molecules. c) Methanol is a polar molecule due to the presence of the hydroxyl group (OH-) and water is also a polar solvent. The interaction between a polar solute and a polar solvent is a hydrogen bonding interaction, specifically between the hydroxyl groups in both methanol and water.

Based on the type of solute-solvent interactions, we can order the solutions from weakest to strongest interaction as follows: - Dispersion interaction: CH2Cl2 in benzene (weakest) - Hydrogen bonding interaction: Methanol in water (medium strength) - Ion-dipole interaction: KCl in water (strongest) So, the final ranking of the solutions from weakest to strongest solute-solvent interaction is: (b) CH2Cl2 in benzene, (c) methanol in water, and (a) KCl in water.