Editing Enthalpy change of solution (section)

==Dependence on the nature of the solution==
The [[enthalpy of mixing]] of an [[ideal solution]] is zero by definition, but the enthalpy of dissolution of nonelectrolytes has the value of the [[enthalpy of fusion]] or vaporisation. For non-ideal solutions of [[electrolyte]]s it is connected to the [[activity coefficient]] of the solute(s) and the temperature derivative of the [[relative permittivity]] through the following formula:<ref>[[Gustav Kortüm]], Elektrolytlösungen, [[Akademische Verlagsgesellschaft m. b. H.]], Leipzig 1941, p.&nbsp;124.</ref>
<math display="block">
 H_\text{dil} = \sum_i \nu_i RT \ln \gamma_i \left(1 + \frac{T}{\epsilon} \frac{\partial\epsilon}{\partial T}\right).
</math>

{|class="wikitable"
|+ Enthalpy change of solution in [[water]] at 25&nbsp;°C for some selected compounds<ref>[[CRC Handbook of Chemistry and Physics]], 90th ed. {{Webarchive|url=https://web.archive.org/web/20120902091218/http://www.crcpress.com/product/isbn/9781420090840|date=2012-09-02}}.</ref>
! Compound !! Δ''H''<sup><s>o</s></sup> in [[Joule|kJ]]/[[mole (unit)|mol]]
|-
| [[hydrochloric acid]] || −74.84
|-
| [[ammonium nitrate]] || +25.69
|-
| [[ammonia]] || −30.50
|-
| [[potassium hydroxide]] || −57.61
|-
| [[caesium hydroxide]] || −71.55
|-
| [[sodium chloride]] || +3.87 
|-
| [[potassium chlorate]] || +41.38
|-
| [[acetic acid]] || −1.51
|-
| [[sodium hydroxide]] || −44.50
|}