Chapter 16, Problem 76PS

Interpretation Introduction

Interpretation:

Stronger Bronsted acid has to be identified from the given compounds.

${{\text{[V(H}}_{\text{2}}{\text{O)}}_{\text{6}}\text{]}}^{\text{2+}}{\text{ or [V(H}}_{\text{2}}{\text{O)}}_{\text{6}}{\text{]}}^{\text{3+}}$

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.

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid $\text{(HA)}$ donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).