Chapter 16, Problem 16.92QP

Interpretation Introduction

Interpretation:

${\text{Al}}^{\text{3+}}$ is not a Bronsted acid, but ${\text{Al(H}}_{\text{2}}{\text{O)}}_{\text{6}}{}^{\text{3+}}$ is a Bronsted acid has to be explained

Concept Information:

Bronsted's definition is based on the chemical reaction that occurs 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 Explain: ${\text{Al}}^{\text{3+}}$ is not a Bronsted acid, but ${\text{Al(H}}_{\text{2}}{\text{O)}}_{\text{6}}{}^{\text{3+}}$ is a Bronsted acid