Chapter 15, Problem 40RQ

Interpretation Introduction

Interpretation:

The reason that alkali metal ions have little effect on the acidic character of the solution is to be discussed.

Concept Introduction:

Bronsted-Lowry acids are the species which donate ${\text{H}}^{+}$ and the ones that accept the ${\text{H}}^{+}$ ions are considered as Bronsted-Lowry bases. The species formed after the donation of ${\text{H}}^{+}$ by a Bronsted-Lowry acid is called its conjugate base while the species that are formed after accepting ${\text{H}}^{+}$ by a base is called its conjugate acid.

According to the Lewis concept, a species that is able to accept a pair of electrons to form a coordinate bond is known as acid. A Lewis base is the species that can donate an electron pair to form a coordinate bond. The formation of coordinate bond between a donor and acceptor is considered an example of neutralization reaction, according to the Lewis concept.

Metal ions that are small in size, as well as their hydrates, form acidic solutions in water as they polarize the water molecule and weaken their O-H bonds to release protons. The acidic character varies directly with the charge on the metal ion and inversely with its size.