Chapter 18, Problem 18.96P

Interpretation Introduction

Interpretation:

The reason has to be explained for most anions basic in water and the formula has to be given for the anions which are not basic in water.

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.

Bronsted –Lowry definitions:

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

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair, a Lewis base is a substance that can donate and share an electron pair.