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Last updated date: 09th Dec 2023
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# What is the dissolution reaction of $C{H_3}CO{O^ - }$ anion and what type of dissociation constant do you get from this reaction?

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Hint: We have to remember that the Arrhenius concept said that an acid is a substance that can donate a proton whereas base is a substance that accepts a proton. Acid dissociates in a solution giving a proton. Acid and base react to give its respective conjugate acid and conjugate base.

$C{H_3}COOH + {H_2}O\overset {} \leftrightarrows C{H_3}CO{O^ - } + {H_3}{O^ + }$
${K_a} = \dfrac{{\left[ {C{H_3}CO{O^ - }} \right]\left[ {{H_3}{O^ + }} \right]}}{{\left[ {C{H_3}COOH} \right]}}$
${K_a}$ is the dissociation constant i.e. acid ionization constant that measures the strength of an acid. These types of dissociation are also known as acid-base dissociation. $C{H_3}CO{O^ - }$ Acetate ion is the conjugate base of acetic acid. This system usually occurs in equilibrium, which means the rate of forward reaction is equal to the rate of backward reaction that occurs at the same rate. Arrhenius concept said that an acid is a substance that can donate a proton whereas base is a substance that accepts a proton. Acid dissociates in a solution giving a proton.
Acid$+$ base $\overset {} \leftrightarrows$conjugate acid $+$ conjugate base
An acid is said to be strong or weak on the basis of its dissociation levels. When the concentration of un dissociated species is too low then an acid is said to be strong whereas if it is high an acid is weak. If the value of $p{K_a}$is less than zero than an acid is said to be strong.
We have to know that an acetic acid is a weak monoprotic acid. This acid can be dangerous to skin as it causes skin irritation. The above dissociation that we have discussed is the dissociation in acid-base reactions. ${K_a}$ is the dissociation constant i.e. acid ionization constant that measures the strength of an acid.