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

The value of Ka
`= 1.1*10^(-2)`

It is a weak acid

Step-by-step 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 = (concentration \ of \ product )/(concentration \ of \ reactant )`

`= ([H^+][ClO_2^-])/([HClO_2])`

Substituting values since all value of concentration are at equilibrium

`Ka = (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