Answer:
The value of Ka [tex]= 1.1*10^{-2}[/tex]
It is a weak acid
Explanation:
From the question we are told that
The concentration of [tex][HClO_2]=0.24M[/tex]
The concentration of [tex][H^+]=0.051M[/tex]
The concentration of [tex][ClO_2^-]=0.051M[/tex]
Generally the equation for the ionic dissociation of [tex]HClO_2[/tex] is
[tex]HClO_2_(aq) -------> H^{+}_{(aq)} + ClO_2^{-}_{(aq)}[/tex]
The equilibrium constant is mathematically represented as
[tex]Ka = \frac{concentration \ of \ product }{concentration \ of \ reactant }[/tex]
[tex]= \frac{[H^+][ClO_2^-]}{[HClO_2]}[/tex]
Substituting values since all value of concentration are at equilibrium
[tex]Ka = \frac{0.051 * 0.051}{0.24}[/tex]
[tex]= 1.1*10^{-2}[/tex]
Since the value of is less than 1 it show that in water it dose not completely
disassociated so it an acid that is weak
