Chapter 3.6, Problem 3.5CYU

(a)

Interpretation Introduction

Interpretation:

The balanced equation for formation of dihydrogen phosphate from Phosphoric acid in water should be explained.

Concept Introduction:

The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction, therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products.

Bronsted Acid: An acid donates (loses)${\text{H}}^{+}$ ion.

Bronsted Base: A base accepts (gains)${\text{H}}^{+}$ ion.

(b)

Interpretation Introduction

Interpretation:

The net ionic equation for the ionization of dihydrogen phosphate in water and the nature of the dihydrogen phosphate should be explained.

Concept Introduction:

The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction, therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products.

Bronsted acid: An acid donates (loses) ${\text{H}}^{+}$ ion.

Bronsted Base: A base accepts (gains) ${\text{H}}^{+}$ ion.

Amphiprotic substance: An amphiprotic substance is a substance that can donate or accept a proton.