Chapter 4, Problem 17QP

Interpretation Introduction

Interpretation:

The diagram that best represents the mixture of aqueous solutions of AgNO₃ and NaCl is to be identified.

Concept introduction:

When two aqueous solutions of ionic compounds are mixed together, a precipitate is formed. The formation of a precipitate is determined by the solubility rules.

The compounds containing alkali metal cation or ammonium ion are watersoluble.

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

The compounds containing chloride ion, bromide ion, or iodide ion are watersoluble 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 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, which contain carbonate ion, phosphate ion, and sulfide ion, and most metal hydroxides are insoluble in water except the compounds containing alkali metal cation or ammonium ion.

Spectator ions are the ions that exist as a reactant and a product in a chemical reaction.