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dissociation constant and temperature

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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.

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