Problem 53 - Chemistry An Atoms First Approach

Question

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide

Step-by-Step Solution

Answer

a. \(SO_4^{2-}(aq) + Ba^{2+}(aq) \rightarrow BaSO_4(s)\) b. \(Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\) c. No reaction occurs. d. No reaction occurs. e. \(Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s)\)

Step 1: Write the balanced molecular equation

For the reaction between ammonium sulfate \((NH_4)_2SO_4\), and barium nitrate \((Ba(NO_3)_2)\): \[(NH_4)_2SO_4 (aq) + Ba(NO_3)_2(aq) \rightarrow 2NH_4NO_3(aq) + BaSO_4(s)\]

Step 2: Write the balanced total ionic equation

Split all strong electrolytes into ions: \[2NH_4^+(aq) + SO_4^{2-}(aq) + Ba^{2+}(aq) + 2NO_3^-(aq) \rightarrow 2NH_4^+(aq) + 2NO_3^-(aq) + BaSO_4(s)\]

Step 3: Write the net ionic equation

Remove the spectator ions (2NH4+ and 2NO3-): \[SO_4^{2-}(aq) + Ba^{2+}(aq) \rightarrow BaSO_4(s)\] b. Lead(II) nitrate and sodium chloride

Step 1: Write the balanced molecular equation

For the reaction between lead(II) nitrate \((Pb(NO_3)_2)\) and sodium chloride \((NaCl)\): \[Pb(NO_3)_2(aq) + 2NaCl(aq) \rightarrow 2NaNO_3(aq) + PbCl_2(s)\]

Step 2: Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Pb^{2+}(aq) + 2NO_3^-(aq) + 2Na^+(aq) + 2Cl^-(aq) \rightarrow 2Na^+(aq) + 2NO_3^-(aq) + PbCl_2(s)\]

Step 3: Write the net ionic equation

Remove the spectator ions (2Na+ and 2NO3-): \[Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\] c. Sodium phosphate and potassium nitrate

Step 1: Write the balanced molecular equation

For the reaction between sodium phosphate \((Na_3PO_4)\) and potassium nitrate \((KNO_3)\): \[Na_3PO_4(aq) + 3KNO_3(aq) \rightarrow 3NaNO_3(aq) + K_3PO_4(aq)\]

Step 2: Write the balanced total ionic equation

Split all strong electrolytes into ions: \[3Na^+(aq) + PO_4^{3-}(aq) + 3K^+(aq) + 3NO_3^-(aq) \rightarrow 3Na^+(aq) + 3NO_3^-(aq) + 3K^+(aq) + PO_4^{3-}(aq)\]

Step 3: Write the net ionic equation

All ions are spectator ions, so no reaction occurs. d. Sodium bromide and rubidium chloride

Step 1: Write the balanced molecular equation

For the reaction between sodium bromide \((NaBr)\) and rubidium chloride \((RbCl)\): \[NaBr(aq) + RbCl(aq) \rightarrow NaCl(aq) + RbBr(aq)\]

Step 2: Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Na^+(aq) + Br^-(aq) + Rb^+(aq) + Cl^-(aq) \rightarrow Na^+(aq) + Cl^-(aq) + Rb^+(aq) + Br^-(aq)\]

Step 3: Write the net ionic equation

All ions are spectator ions, so no reaction occurs. e. Copper(II) chloride and sodium hydroxide

Step 1: Write the balanced molecular equation

For the reaction between copper(II) chloride \((CuCl_2)\) and sodium hydroxide \((NaOH)\): \[CuCl_2(aq) + 2NaOH(aq) \rightarrow 2NaCl(aq) + Cu(OH)_2(s)\]

Step 2: Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Cu^{2+}(aq) + 2Cl^-(aq) + 2Na^+(aq) + 2OH^-(aq) \rightarrow 2Na^+(aq) + 2Cl^-(aq) + Cu(OH)_2(s)\]

Step 3: Write the net ionic equation

Remove the spectator ions (2Na+ and 2Cl-): \[Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s)\]