Chapter 16, Problem 16.50QP

Interpretation Introduction

Interpretation:

• All the species that are present in a phosphoric acid solution has to be written.
• Which species can act as a Brønsted acid, which as a Brønsted base, and which as both a Brønsted acid and a Brønsted base has to be indicated

Concept Information:

Bronsted's definitions of acid and base:

Bronsted's definition is based on the chemical reactions that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

    $\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.

To write: all the species that is present in a phosphoric acid solution

Which species can act as a Brønsted acid, which as a Brønsted base, and which as both a Brønsted acid and a Brønsted base.