Chapter 18, Problem 18.37P

Interpretation Introduction

Interpretation:

The difference and similar between Arrhenius and Brønsted - Lowry acid-base definitions has to explained, and example has to be given for Brønsted - Lowry bases that are not Arrhenius bases and Brønsted - Lowry acids that are not Arrhenius acids.

Concept introduction:

Arrhenius Acids and Bases:

Acid release hydrogen ion in water, base release hydroxide ions in water.

  $\begin{array}{l}\text{HCl(aq) }\to {\text{H}}^{\text{+}}{\text{(aq) + Cl}}^{\text{-}}\text{(aq)}\mathrm{.................}\text{Acid}\\ \text{NaOH(aq) }\to {\text{Na}}^{\text{+}}{\text{(aq)+ OH}}^{\text{-}}\text{(aq)}\mathrm{...........}\text{Base}\end{array}$

An acid is a substance that produces hydronium ions, ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ when dissolved in water.

Brønsted –Lowry definitions:

A Brønsted –Lowry acid is a proton donor, it donates a hydrogen ion (${\text{H}}^{\text{+}}$), a Brønsted -Lowry base is a proton acceptor, it accepts a hydrogen ion (${\text{H}}^{\text{+}}$).