Chapter 15, Problem 15.1QE

Interpretation Introduction

Interpretation:

The difference between Bronsted- Lowry acids and Arrhenius acids has to be determined.

Concept Introduction:

Matter dissolves in the water and produces a solution. Solution is generally a mixture of two or more compounds. Two types of solutions are:

1. Acids

2. Bases

Acid is a substance that produces ${\text{H}}^{\text{+}}$ ions when dissolved in water. Acids have sour taste. Acids are proton donors.

Bases are substances that produce ${\text{OH}}^{-}$ ions in water. Bases have bitter taste. Bases are proton acceptors.

Explanation of Solution

In Bronsted–Lowry theory, Acid is defined as a substance that donates a proton. In a solution, it breaks to give ${\text{H}}^{\text{+}}$ ions. A solution can be water or made of any other compounds. For example, $\text{HCl}$. All Bronsted–Lowry acids cannot be Arrhenius acids.

In Arrhenius theory, acid is generallydefined as a substance that produces ${\text{H}}^{\text{+}}$ ions when dissolved in water. In this theory, the solvent is water only. For example, acetic acid, nitric acid. All Arrhenius acids can be Bronsted–Lowry acids.