Chapter 3, Problem 2LGP

Interpretation Introduction

Interpretation:

The p K_a values of acidic hydrogen of the given species are to be determined using table 3.1.

Concept introduction:

The strength of an acid is generally described in terms of acidity constant $\left(K_{\text{a}}\right)$ and $\text{p}{K}_{\text{a}}$ values.

A large value of $K_{\text{a}}$ indicates that the acid is strong and a small value of $K_{\text{a}}$ indicates a weak acid.

The value of pK_a of a reagent can be mathematical defined as

$\text{p}{K}_{\text{a}}\text{= }-\text{log(}{K}_{\text{a}}\text{) }$

The higher is the dissolution constant, that is, the reagent can produce more ions when dissolved in water, the stronger is the acid. Thus, by the above relation, strong acids have low pK_a.

The stronger the acid, the weaker is its conjugate base.

Larger the value of pK_a of the conjugate base, the stronger is the acid.

The ${\text{ pK}}_{\text{a}}$ value gives the measure of strength of an acid. The smaller the pK_a value, the stronger is the acid. The larger the pK_a value, the weaker is the acid.

Alcohol is too weak an acid to ionize in the presence of strong sulfuric acid.

The ester is nonelectrolyte and will not ionize in water.