Enthalpy change of solution
Enthalpy Change of Solution
The enthalpy change of solution (ΔH_sol) is the enthalpy change associated with the dissolution of a solute in a solvent to form a solution. It is a specific type of enthalpy change and is a crucial concept in thermodynamics and physical chemistry.
Definition[edit | edit source]
The enthalpy change of solution is defined as the amount of heat absorbed or released when one mole of a solute dissolves in a specified amount of solvent. This process can either be endothermic (absorbing heat) or exothermic (releasing heat), depending on the nature of the solute and solvent involved.
Calculation[edit | edit source]
The enthalpy change of solution can be calculated using the following steps:
1. Lattice Enthalpy (ΔH_lattice): The energy required to break the ionic bonds in the solute. 2. Hydration Enthalpy (ΔH_hydration): The energy released when the ions are surrounded by water molecules.
The overall enthalpy change of solution is given by:
ΔH_sol = ΔH_lattice + ΔH_hydration
Factors Affecting Enthalpy Change of Solution[edit | edit source]
Several factors can influence the enthalpy change of solution, including:
- Nature of the Solute and Solvent: Different substances have different lattice and hydration enthalpies.
- Temperature: The solubility and enthalpy change can vary with temperature.
- Pressure: For gases, pressure can significantly affect solubility and enthalpy change.
Applications[edit | edit source]
Understanding the enthalpy change of solution is essential in various fields such as:
- Pharmaceuticals: For drug formulation and solubility studies.
- Chemical Engineering: In designing processes involving dissolution.
- Environmental Science: For understanding the dissolution of pollutants.
Related Concepts[edit | edit source]
See Also[edit | edit source]
References[edit | edit source]
External Links[edit | edit source]
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Contributors: Prab R. Tumpati, MD
