Heat of neutralization

As the heat of neutralization or Neutralisationsenthalpie is called the heat of reaction or enthalpy , which in the highly exothermic reaction of a neutralization becomes free. Physically, heat differs from enthalpy in that the reaction conditions in the first case are isochoric (with constant volume) and in the second case isobaric (with constant pressure). The distinction is not important for neutralization reactions in aqueous solution, as these are both isochoric and isobaric. ${\ displaystyle \ Delta Q}$ ${\ displaystyle \ Delta H}$

The enthalpy of neutralization of hydroxide and oxonium ions is . For pairs of strong acids and bases that are completely dissociated in aqueous solution, this value is a good estimate, as the additional enthalpy of reaction of the corresponding weak acid-base pair can be neglected. ${\ displaystyle \ Delta H = -57 {,} 3 \, \ mathrm {\ tfrac {kJ} {mol}}}$

Individual evidence

↑ Hans Peter Latscha and Helmut Alfons Klein: Inorganic Chemistry . 9th edition. Springer, Berlin Heidelberg New York 2007, ISBN 978-3-540-69863-0 , pp. 222 .

[1] Hans Peter Latscha and Helmut Alfons Klein: Inorganic Chemistry . 9th edition. Springer, Berlin Heidelberg New York 2007, ISBN 978-3-540-69863-0 , pp. 222 .