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
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