Chapter 18, Problem 71A

Interpretation Introduction

Interpretation:

The ionization equation and acid ionization constant of given compound is to be written.

Concept introduction:

Ionization equations show the species which are formed on dissolving the compound in aqueous solution.

Acid ionization constant tells about equilibrium that whether reactants are favored or products.

For a reaction,

$HA+H_{2}O\rightleftharpoons A^{-}+H_3{O}^{+}$

Acid ionization constant is given by:

$\begin{array}{l}{k}_a=\frac{\left[A^{-}\right]\times \left[H_3{O}^{+}\right]}{\left[HA\right]}\\ where,\\ \left[A^{-}\right]isconcentrationof{A}^{-}\\ \left[H_3{O}^{+}\right]isconcentrationof{H}_3{O}^{+}\\ \left[HA\right]isconcentrationofHA\end{array}$

Answer to Problem 71A

Ionization equation:

$HClO+H_{2}O\rightleftharpoons Cl{O}^{-}+H_3{O}^{+}$

The acid ionization constant is:

$k_a=\frac{\left[Cl{O}^{-}\right]\times \left[H_3{O}^{+}\right]}{\left[HClO\right]}$

Explanation of Solution

When $HClO(hypochlorousacid)$ is dissolved in aqueous medium, ionic equation is given by:

$HClO+H_{2}O\rightleftharpoons Cl{O}^{-}+H_3{O}^{+}$

Thus, acid ionization constant is:

$k_a=\frac{\left[Cl{O}^{-}\right]\times \left[H_3{O}^{+}\right]}{\left[HClO\right]}$

Conclusion

Thus,

Ionization equation:

$HClO+H_{2}O\rightleftharpoons Cl{O}^{-}+H_3{O}^{+}$

The acid ionization constant is:

$k_a=\frac{\left[Cl{O}^{-}\right]\times \left[H_3{O}^{+}\right]}{\left[HClO\right]}$