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# How does the degree of dissociation affect $K_a$?

Last updated date: 18th Jun 2024
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Hint: The $K_a$ value is started by looking at the equilibrium constant for the dissociation of the acid. The upper the $K_a$, the more the acid dissociates. Thus, resilient acids must dissociate in water. In contrast, a weak acid is less expected to ionize and release a hydrogen ion, consequently resulting in a less acidic.

The greater the value of $K_a$, the greater the range of dissociation.
For several acid,$\;HA$ , we can inscribe the dissociation process as
$HA\left( {aq} \right){\text{ }} \leftrightarrow {H^ + }\left( {aq} \right){\text{ }} + {\text{ }}{A^ - }\left( {aq} \right)$
The equilibrium constant for this process is definite as the proportion of equilibrium products and reactants:
${K_a} = ([{H^ + }][{A^ - }])/([HA])$$K_a$ is huge, then the concentration of dissociated ions is greater than the concentration of liquefied acid, [$\;HA$]
Illustrations (take up the total concentration of acid is$1{\text{ }}M$):
If $K_a = 0.03\;$ then the degree of dissociation is $15.9\% ,$then if
$K_a = 0.05\;$ then the degree of dissociation is $20.0\% ,$and uncertainty
$K_a = 3.8\;$ at that time the degree of dissociation is $82.2\%$

Dissociation in Chemistry and biochemistry is a complete procedure in which particles (or ionic compounds for instance salts, or complexes) dispersed or split into slighter particles such as atoms, ions, or radicals, typically in a reversible manner. Such as, when an acid dissolves in water, a covalent bond among an electronegative atom and a hydrogen atom is damaged by heterolytic fission, which stretches a proton $({H^ + })$ and a negative ion.
Note: An acid dissociation continual ($K_a$) is a quantifiable measure of the strong point of a critical solution.
An acid $K_a$, (similarly predictable as acidity continual, or acid-ionization constant) is a quantifiable quantity of the strong point of an acid in solution. This one is the equilibrium constant for a chemical reaction.
$HA{\text{ }} \leftrightarrow {H^ + } + {A^ - }$