Enthalpy change of solution

<p>In <a href="/facts/Thermochemistry/fQS7IsoT">thermochemistry</a>, the enthalpy of solution (heat of solution or enthalpy of solvation) is the <a href="/facts/Enthalpy/bBou8lCE">enthalpy</a> change associated with the <a href="/facts/Solvation/JVM6j8R1">dissolution</a> of a substance in a <a href="/facts/Solvent/LoMPMz8S">solvent</a> at <a href="/facts/Isobaric_process/SRx2Pd15">constant pressure</a> resulting in infinite dilution.
</p><p>The enthalpy of solution is most often expressed in <a href="/facts/Joule/9ndq9jD2">kJ</a>/<a href="/facts/Mole_(unit)/kCMFwCc0">mol</a> at constant temperature. The energy change can be regarded as being made up of three parts: the <a href="/facts/Endothermic/06xmHw6Q">endothermic</a> breaking of <a href="/facts/Chemical_bond/ArNUMnIB">bonds</a> within the <a href="/facts/Solute/MGchhMQV">solute</a> and within the solvent, and the formation of attractions between the solute and the solvent. An <a href="/facts/Ideal_solution/Ho6rPlcs">ideal solution</a> has a null <a href="/facts/Enthalpy_of_mixing/qgucNGGn">enthalpy of mixing</a>. For a non-ideal solution, it is an <a href="/facts/Excess_molar_quantity/hkvadLNB">excess molar quantity</a>.
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Enthalpy change of solution open-in-new

Enthalpy change of solution