ENTHALPY CHANGE OF SOLUTION Meaning and
Definition
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Enthalpy change of solution refers to the amount of heat energy released or absorbed when a solute is dissolved in a solvent to form a homogeneous solution. It can be described as the difference in enthalpy (or heat content) between the initial state, where the solute and solvent are separate, and the final state, where they are completely mixed.
When a solute dissolves in a solvent, there are usually intermolecular forces that need to be overcome or formed between the solute and solvent particles. These intermolecular forces can be in the form of hydrogen bonding, dipole-dipole interactions, or London dispersion forces. The enthalpy change of solution takes into account the energy required to break these forces between the solute and solvent particles, as well as the energy released when new forces are formed between the solute and solvent particles.
The enthalpy change of solution is dependent on various factors, such as the nature of the solute and solvent, temperature, pressure, and concentration. It can be calculated experimentally by measuring the temperature change during the dissolution process and applying the appropriate thermochemical equations.
Overall, the enthalpy change of solution is an important concept in thermodynamics and is used to understand and analyze the energy changes that occur during the process of solvation.
