What effect does hydrogen bonding have on water solubility?

Hydrogen bonding plays a critical role in increasing the water solubility of various substances. Water is a polar molecule, and its ability to form hydrogen bonds arises from the interaction between the slightly positive hydrogen atoms and the slightly negative oxygen atoms in adjacent water molecules. This characteristic allows water to interact favorably with other polar or ionic substances.

When a solute is introduced into water, the formation of hydrogen bonds between water molecules and solute molecules can lead to an energetic stabilization of the solute in solution. For example, when ionic compounds dissolve in water, the ions are surrounded by water molecules that form hydration shells, driven by hydrogen bonding with the water. Similarly, polar molecules can interact with water via hydrogen bonds, enhancing their solubility.

This solubilizing effect is particularly significant for substances that can either donate or accept hydrogen bonds, such as alcohols, sugars, and acids. These interactions promote the dissolution process, making the correct conclusion that hydrogen bonding increases water solubility.