Chapter 4.4, Problem 1PPB

Interpretation Introduction

Interpretation:

The molecular, ionic, and net ionic equations for the neutralization reaction between ${\text{NH}}_{\text{3}}$ and ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ are to be written.

Concept introduction:

The ionic and net ionic equations can be written using the following steps:

Write a balanced molecular equation along with the state of each substance. Rewrite the equation as a complete ionic equation showing which compounds are dissociated into ions, using the knowledge of solubility rules.

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.

Cancel out the spectator ions on both sides of the equation to get the net ionic equation.