Chapter 18, Problem 18.105CHP

Interpretation Introduction

Interpretation:

• For given acid-base reaction, the chemical equation has to be written to show how aqueous solution of acidic oxides such as ${\text{SO}}_{\text{2}}$ and ${\text{SO}}_{\text{3}}$ can yield ${\text{H}}_3{\text{O}}^{\text{+}}$ ion.
• Among these two oxides, which produce a higher concentration of ${\text{H}}_3{\text{O}}^{\text{+}}$ ions has to be explained.

Concept Introduction:

Oxides can be classified into acidic, basic or amphoteric.

• Basic oxides are ionic formed by metal.  Water soluble basic oxide such as ${\text{Li}}_{\text{2}}\text{O}$ and ${\text{Na}}_{\text{2}}\text{O}$ reacts with water to gives ${\text{OH}}^{\text{-}}$ ions.  Basic oxides are placed on the left side of the periodic table.
• Acidic oxides are covalent and they formed by non-metals.  Water soluble acid oxides such as ${\text{P}}_{\text{4}}{\text{O}}_{\text{10}}$ and ${\text{SO}}_{\text{3}}$ dissolved by reacts with water to gives ${\text{H}}^{\text{+}}$ ions.  Acidic oxides are placed on the right side of the periodic table.
• Amphoteric oxides act as both acids and bases and dissolves both strong acid and in strong base but insoluble in water.  For example, amphoteric oxides act as acid when react with base and vice versa.