Question

Calculate the Ka for the following acid. Determine if it is a strong or weak acid. HClO2(aq) dissolves in aqueous solution to form H+(aq) and ClO2−(aq). At equilibrium, the concentrations of each of the species are as follows: [HClO2]=0.24M [H+]=0.051M [ClO2−]=0.051M

Answer 1

Answer:

The value of Ka $= 1.1*10^{-2}$

It is a weak  acid

Explanation:

   From the question we are told that

             The concentration of $[HClO_2]=0.24M$

             The concentration of  $[H^+]=0.051M$

             The concentration of  $[ClO_2^-]=0.051M$

Generally the equation for the ionic dissociation of $HClO_2$ is

                $HClO_2_(aq) -------> H^{+}_{(aq)} + ClO_2^{-}_{(aq)}$

The equilibrium constant is mathematically represented as

                         $Ka = \frac{concentration \ of \ product }{concentration \ of \ reactant }$

                               $= \frac{[H^+][ClO_2^-]}{[HClO_2]}$

Substituting values since all value of concentration are at equilibrium

                    $Ka = \frac{0.051 * 0.051}{0.24}$

                          $= 1.1*10^{-2}$

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