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Solvation refers to the process by which solute particles (such as ions or molecules) are surrounded and dispersed by solvent molecules, typically in a liquid medium. This interaction is fundamental in chemistry, biology, and materials science, influencing solubility, reaction rates, and biological activity.

In solvation, solvent molecules (e.g., water in aqueous solutions) interact with solute particles through forces like hydrogen bonding, ionic interactions, or van der Waals forces. For ionic solutes, solvation often involves the formation of a hydration shell, where water molecules orient themselves around charged ions to stabilize them. Nonpolar solutes, however, tend to dissolve in nonpolar solvents due to favorable dispersion interactions.

The extent of solvation depends on factors such as solvent polarity, solute structure, temperature, and pressure. Highly polar solvents like water effectively solvate ionic and polar compounds, while nonpolar solvents (e.g., hexane) dissolve nonpolar substances. Solvation enthalpy—the energy change accompanying the process—can be endothermic or exothermic, affecting equilibrium and reaction dynamics.

Solvation plays a critical role in biological systems, where enzymes and proteins rely on proper solvation for function. It also impacts industrial processes, such as drug formulation, where solubility determines bioavailability. Understanding solvation helps in designing solvents for specific applications, optimizing chemical reactions, and studying molecular interactions.

In contrast to solvation, dissolution refers to the broader process of a solute dispersing in a solvent, while solvation specifically describes the molecular-level interactions between solute and solvent. Both concepts are essential in physical chemistry and are widely studied using techniques like spectroscopy, calorimetry, and computational modeling.