Chapter 4.4, Problem 1PPC

Interpretation Introduction

Interpretation:

The diagram representing the ions remaining in the solution, after stoichiometric amounts of aqueous barium hydroxide and hydrobromic acid are combined, is to be determined.

Concept introduction:

When aqueous solutions of two ionic compounds are combined, the formation of soluble or insoluble compounds can be predicted by using the solubility rules.

A balanced ionic equation indicates the dissociated ions in the solution. The net ionic equation shows the ions participating in the reaction.

The compounds containing 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 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 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.