What is the relationship between intermolecular hydrogen bonding and solubility?

The relationship between intermolecular hydrogen bonding and solubility is fundamentally rooted in the principle of “like dissolves like." Substances that can form hydrogen bonds with each other typically have increased solubility in one another, particularly when comparing polar solvents and solutes.

When a solute can engage in hydrogen bonding with a solvent, it often results in greater solubility because this type of bonding facilitates strong interactions between the molecules of the solute and the solvent, enabling the solute to be dispersed within the solvent. For example, substances like alcohols or carboxylic acids, which possess -OH or -COOH groups capable of forming hydrogen bonds, tend to dissolve well in polar solvents such as water due to these interactions.

While there can be scenarios where excessive hydrogen bonding might create rigid structures that are less favorable for solubility, in the general sense, strong hydrogen bonding among molecules typically aids solubility in polar environments. This means that if a solute can form strong hydrogen bonds with the solvent, its solubility will increase, making the correct understanding of this concept pivotal in chemistry.

The notion that more hydrogen bonding might lead to decreased solubility doesn't hold true within the context of most solubility scenarios