Sandy Posted March 31, 2015 Report Share Posted March 31, 2015 Why does the dissociation constant change with temperature? Reply Link to post Share on other sites More sharing options...
Ossih Posted April 2, 2015 Report Share Posted April 2, 2015 Hey! By dissociation constant I'm assuming you mean Ka right? Okay so Ka = [H+][A-] / [HA] and the relative proportions depend on this dissociation equilibrium HA <--> H+ + A- Ka is just an equilibrium constant for this equilibrium, and equilibrium constants are dependent on temperature. If you think about it, dissociation is endothermic, so if I increase the temperature, I should end up with a higher relative proportion of [H+]. I hope that makes sense ! Remember that temperature is the only thing that affects equilibrium constants. Reply Link to post Share on other sites More sharing options...
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