Chapter 18.8, Problem 18.9P

(a)

Interpretation Introduction

Interpretation:

Balanced net ionic equation for dissolution of solid ${\text{Li}}_{\text{2}}\text{O}$ in water has to be written.

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.
• 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.
• Amphoteric oxides act as both acids and bases and dissolves both strong acid and in strong base but insoluble in water.

(b)

Interpretation Introduction

Interpretation:

Balanced net ionic equation for dissolution of ${\text{SO}}_{\text{3}}$ in water has to be written.

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.
• 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.
• Amphoteric oxides act as both acids and bases and dissolves both strong acid and in strong base but insoluble in water.

(c)

Interpretation Introduction

Interpretation:

Balanced net ionic equation for dissolution of ${\text{Cr}}_{\text{2}}{\text{O}}_{\text{3}}$ in strong acid has to be written

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.
• 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.
• Amphoteric oxides act as both acids and bases and dissolves both strong acid and in strong base but insoluble in water.

(d)

Interpretation Introduction

Interpretation:

Balanced net ionic equation for dissolution of ${\text{Cr}}_{\text{2}}{\text{O}}_{\text{3}}$ in strong base to give $\text{Cr}{\left(\text{OH}\right)}_4^{-}$ has to be written

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.
• 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.
• Amphoteric oxides act as both acids and bases and dissolves both strong acid and in strong base but insoluble in water.