Chapter 4, Problem 4.62P

(a)

Interpretation Introduction

Interpretation:

The balanced net ionic equation that shows that the reaction between acetic acid and sodium hydroxide is different from the reaction between hydrochloric acid and sodium hydroxide is to be written.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Strong acids or bases and weak acids or bases can be differentiated by measuring the electrical conductivity. Strong acids or bases completely dissociates into ions in the water, therefore, it has more number of ions as compared to weak acids or bases.

(b)

Interpretation Introduction

Interpretation:

The major species in decreasing order of concentration when acetic acid is dissolved in water is to be listed.

Concept introduction:

Acid is a substance that dissociates in water to release ${\text{H}}^{+}$ ions. Depending upon the strength the acids can be classified into two types:

1. Strong acids

2. Weak acids

Strong acids are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release ${\text{H}}^{+}$ ions. They behave as strong electrolytes and conduct a large amount of electricity.

Weak acids are the substance that does not dissociates completely into its ions when dissolved in the solution. They dissociate partially in water to release ${\text{H}}^{+}$ ions. They behave as weak electrolytes and conduct less amount of electricity.