d
\((d)\) The general rule that explains solubility on the basis of the polarity of  molecules is that "like dissolves like." In other words, polar compounds dissolve in  polar solvents and nonpolar compounds dissolve in nonpolar solvents. This is  generally true because a polar solvent such as water has partial charges that can  interact with the partial charges on a polar compound. The negative poles of the  solvent molecules surround the positive pole of the polar solute, and the positive  poles of the solvent molecules surround the negative pole of the polar solute. Clustering of the solvent molecules around the solute molecules separates solute  molecules from each other, which is what makes them soluble. The interaction  between a solvent and a molecule or an ion that is dissolved in that solvent is called  solvation.
Because nonpolar compounds have no net charge, polar solvents are not attracted  to them. In order for a nonpolar molecule to dissolve in a polar solvent such as   water, the nonpolar molecule would have to push the water molecules apart,  disrupting their hydrogen bonding. Hydrogen bonding is so strong that it excludes  the nonpolar compound. In contrast, nonpolar solutes dissolve in non-polar solvents  because of the van der Waals interactions between solvent and solute molecules. 

\(w.r.t.\) the question asked, \(1\) -pentanol has maximum number of carbons, so it is least soluble in water. \(\{\) extent of \(H-\) bonding decreases \(\}\)