Chapter 14, Problem 7QAP

Interpretation Introduction

(a)

Interpretation:

The equilibrium constant K needs to be deduced for the reaction between an aqueous solution of sodium sulfite and H+ ions based on the net ionic equation.

Concept introduction:

1. A net ionic equation depicts only the chemical species that participate in a given reaction; it does not include the spectator ions.
2. There are various types of acid base reactions, each with a characteristic net ionic equation represented as shown below-

$\begin{array}{l}{\text{Strong acid-strong base: H}}^{\text{+}}{\text{(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}\text{O}\\ {\text{Weak acid-strong base: HB(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}{\text{O + B}}^{-}(\text{aq})\\ {\text{Strong acid-weak base: H}}^{\text{+}}\text{(aq) + B(aq)}\to {\text{BH}}^{+}(\text{aq})\end{array}$

3. The equilibrium constant (K) for a given acid-base reaction can be deduced based on the reciprocal rule which states that K for forward and reverse reactions are reciprocals of each other.

${\text{K}}_{\text{forward}}\text{ = }\frac{\text{1}}{{\text{K}}_{\text{reverse}}}\text{ -------(1)}$

Interpretation Introduction

(b)

Interpretation:

The equilibrium constant K needs to be deduced for the reaction between an aqueous solution of lithium hydroxide and H+ ions based on the net ionic equation

Concept introduction:

1. A net ionic equation depicts only the chemical species that participate in a given reaction; it does not include the spectator ions.
2. There are various types of acid base reactions, each with a characteristic net ionic equation represented as shown below-

$\begin{array}{l}{\text{Strong acid-strong base: H}}^{\text{+}}{\text{(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}\text{O}\\ {\text{Weak acid-strong base: HB(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}{\text{O + B}}^{-}(\text{aq})\\ {\text{Strong acid-weak base: H}}^{\text{+}}\text{(aq) + B(aq)}\to {\text{BH}}^{+}(\text{aq})\end{array}$

3. The equilibrium constant (K) for a given acid-base reaction can be deduced based on the reciprocal rule which states that K for forward and reverse reactions are reciprocals of each other.

${\text{K}}_{\text{forward}}\text{ = }\frac{\text{1}}{{\text{K}}_{\text{reverse}}}\text{ -------(1)}$

Interpretation Introduction

(c)

Interpretation:

The equilibrium constant K needs to be deduced for the reaction between an aqueous solution of potassium benzoate and H+ ions based on the net ionic equation

Concept introduction:

1. A net ionic equation depicts only the chemical species that participate in a given reaction; it does not include the spectator ions.
2. There are various types of acid base reactions, each with a characteristic net ionic equation represented as shown below-

$\begin{array}{l}{\text{Strong acid-strong base: H}}^{\text{+}}{\text{(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}\text{O}\\ {\text{Weak acid-strong base: HB(aq) + OH}}^{\text{-}}\text{(aq)}\to {\text{H}}_{\text{2}}{\text{O + B}}^{-}(\text{aq})\\ {\text{Strong acid-weak base: H}}^{\text{+}}\text{(aq) + B(aq)}\to {\text{BH}}^{+}(\text{aq})\end{array}$

3. The equilibrium constant (K) for a given acid-base reaction can be deduced based on the reciprocal rule which states that K for forward and reverse reactions are reciprocals of each other.

${\text{K}}_{\text{forward}}\text{ = }\frac{\text{1}}{{\text{K}}_{\text{reverse}}}\text{ -------(1)}$