Chapter 11.3, Problem 27SP

Interpretation Introduction

Interpretation: To determine the net ionic equation.

Concept Introduction: In a liquid or solid medium, an ionic reaction typically takes place when anions and cations interact to form a compound. When the ions of salts that are soluble in water interact with one another, water-insoluble salts are produced.

Answer to Problem 27SP

In the reaction, lead chloride will be precipitated. The net ionic equation will be:

  ${\text{Pb}}^{\text{2+}}\text{(aq)}{\text{+2Cl}}^{\text{\_}}\to {\text{PbCl}}_{\text{2}}\text{(ppt)}$

Explanation of Solution

The given chemical equation is:

  ${\text{NH}}_{\text{4}}\text{Cl(aq)}\text{+}{\text{Pb(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\to$

When ammonium chloride is treated with lead nitrate then it will form lead chloride and ammonium nitrate. It can be written as:

  ${\text{2NH}}_{\text{4}}\text{Cl(aq)}\text{+}{\text{Pb(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\to {\text{PbCl}}_2\text{(ppt)}\text{+}2{\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}\text{(aq)}$

Its ionic reaction can be written as:

  ${\text{NH}}_{\text{4}}{}^{+}\text{(aq)}+2{\text{Cl}}^{-}\text{(aq)}\text{+}{\text{Pb}}^{2+}{{\text{(NO}}_{\text{3}}\text{)}}^{\_}\text{(aq)}\to {\text{PbCl}}_2\text{(ppt)}\text{+}{\text{NH}}_{\text{4}}{}^{+}\text{(aq)}+{\text{NO}}_{\text{3}}{}^{\_}\text{(aq)}$

Ammonium ion and nitrate ion will be canceled out. So, the net ionic equation will be:

  ${\text{Pb}}^{\text{2+}}\text{(aq)}{\text{+2Cl}}^{\text{\_}}\to {\text{PbCl}}_{\text{2}}\text{(ppt)}$