Chapter 16, Problem 81IAE

Interpretation Introduction

(a)

Interpretation:

To explain whether ${\text{CH}}_{\text{3}}{\text{COO}}^{-}$ acts as an acid, base or amphiprotic in pure acetic acid.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.

Interpretation Introduction

(b)

Interpretation:

To explain whether ${\text{H}}_{\text{2}}\text{O}$ act as an acid, base or amphiprotic in pure acetic acid.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.

Interpretation Introduction

(c)

Interpretation:

To explain whether ${\text{CH}}_{\text{3}}\text{COOH}$ act as an acid, base or amphiprotic in pure acetic acid.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.

Interpretation Introduction

(d)

Interpretation:

To explain whether ${\text{HClO}}_{\text{4}}$ act as an acid, base or amphiprotic in pure acetic acid.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.