Chapter 4.2, Problem 1PPB

Interpretation Introduction

Interpretation:

The given compounds are to be classified as either soluble or insoluble in water.

Concept introduction:

The solubility of the compounds can be predicted on the basis of the following solubility rules:

The compounds containing an alkali metal cation or ammonium ion are water soluble.

The compounds containing nitrate ion, chlorate ion, perchlorate ion, or acetate ion are water soluble.

The compounds containing chloride ion, bromide ion, or iodide ion are water soluble with the exception of compounds containing ${\text{Ag}}^{\text{+}}$, ${\text{Hg}}_2^{2+}$ or ${\text{Pb}}^{\text{2+}}$ ions.

The compounds containing sulfate ion are water soluble with the exception of compounds containing ${\text{Ag}}^{\text{+}}$, ${\text{Hg}}_2^{2+}$, ${\text{Pb}}^{\text{2+}}$, ${\text{Ca}}^{\text{2+}}$, ${\text{Sr}}^{\text{2+}}$, or ${\text{Ba}}^{2+}$ ions.

The compounds containing carbonate ions, phosphate ions, sulfide ions, and most metal hydroxides are insoluble in water except for the compounds containing alkali metal cations or ammonium ion.