Chapter F, Problem I.19E

(a)

Interpretation Introduction

Interpretation:

Using the solubility rules, lead(II) and copper(II) ions has to be separated and also the net ionic equation has to be written.

Concept Introduction:

Soluble compounds:

• Compounds of the elements from Group 1 are soluble.
• Ammonium compounds, chlorides, bromides, iodides are soluble except for the cation being ${\text{Ag}}^{\text{+}}$, ${\text{Hg}}_{\text{2}}{}^{\text{2+}}$, and ${\text{Pb}}^{\text{2+}}$.
• Nitrates, acetates, chlorates, and also perchlorates are soluble except for the cation being ${\text{Ca}}^{\text{2+}}$, ${\text{Sr}}^{\text{2+}}$, ${\text{Ba}}^{\text{2+}}$, ${\text{Pb}}^{\text{2+}}$, ${\text{Hg}}_{\text{2}}{}^{\text{2+}}$, and ${\text{Ag}}^{\text{+}}$.

Insoluble compounds:

• Chromates, carbonates, oxalates, and phosphates are insoluble except for the elements of Group 1 and ammonium ion.
• Sulfides are insoluble except for the elements from Group 1 and 2 and also for ammonium ion.
• Hydroxides and oxides are insoluble except for the elements from Group 1 and 2.

(b)

Interpretation Introduction

Interpretation:

Using the solubility rules, ammonium and magnesium ions has to be separated and also the net ionic equation has to be written.

Concept Introduction:

Refer part (a).