Chapter 14, Problem 14.42CP

(a)

Interpretation Introduction

Interpretation:

Balanced equation for the reaction of ${\text{H}}_{\text{3}}{\text{BO}}_{\text{3}}$ with water has to be written.  In this reaction ${\text{H}}_{\text{3}}{\text{BO}}_{\text{3}}$ act as Bronsted-Lowry acid.

Concept Introduction:

Bronsted-Lowry acid and bases:

The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.

(b)

Interpretation Introduction

Interpretation:

Balanced equation for the reaction of ${\text{H}}_{\text{3}}{\text{BO}}_{\text{3}}$ with water has to be written.  In this reaction ${\text{H}}_{\text{3}}{\text{BO}}_{\text{3}}$ act as Lewis acid.

Concept Introduction:

Lewis acid and base:

In Lewis acid-base reactions, the base donates pair of electron to an acid to forms covalent bond.

$\begin{array}{l}{\text{A}}^{\text{+}}\text{+ }{\text{B}}^{\text{-}}\stackrel{}{\to }\text{A-B}\\ \text{Lewis}\text{Lewis}\text{Covalent bond}\\ \text{acid}\text{base}\end{array}$