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# How does temperature affect the dissociation constant?

Last updated date: 20th Jun 2024
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Hint: You must know that the dissociation of the acid in water is a reversible reaction which means the equilibrium is reached even after the condition is changed. The effect of temperature on the dissociation constant is dependent on whether the reaction is absorbing heat or releasing heat.

The acid dissociation constant is the equilibrium constant of the dissociation reaction of the acid. The acid dissociation is represented by ${K_a}$. It is the quantitative measure of the strength of an acid iin solution. The acid dissociation constant is measured in mol/L.
$HA + {H_2}O \rightleftharpoons {A^ - } + {H_3}{O^ + }$
Here HA is an acid which dissociates in the conjugate base of the weak acid ${A^ - }$ and the hydrogen ion combines with the water to form hydronium ion.
When the concentration of the HA, ${A^ - }$and ${H_3}{O^ + }$ does not change with time, then the reaction has attained equilibrium, so the dissociation constant is given as shown below.
${K_a} = \dfrac{{[{A^ - }][{H_3}{O^ + }]}}{{[HA][{H_2}O]}}$