21 4.5 Ionic Equations

Practice questions

1. 1. 1. What is the chemical equation that represents [latex]\ce{NaBr}[/latex] dissociating in water?
         1. [latex]\ce{NaBr {(s)} {\rightarrow} Na^{+} {(aq)} + Br^{-}{(aq)}}[/latex]
         2. [latex]\ce{NaBr {(s)} {\rightarrow} Na_{2}^{+} {(aq)} + Br_{2}^{-}{(aq)}}[/latex]
         3. [latex]\ce{NaBr {(s)} {\rightarrow} NaOH {(aq)} + BrH {(aq)}}[/latex]
         4. [latex]\ce{NaBr {(s)} {\rightarrow} NaBr {(aq)}}[/latex]
      2.  What is the chemical equation that represents [latex]\ce{SrCl_{2} {(s)}}[/latex] dissociation in water?
         1. [latex]\ce{SrCl_{2} {(s)} {\rightarrow} Sr_{2}^{2+} {(aq)} + 2Cl_{2}^{-}}[/latex]
         2. [latex]\ce{SrCl_{2} {(s)} {\rightarrow} Sr^{2+} {(aq)} + 2Cl^{-}}[/latex]
         3. [latex]\ce{SrCl_{2} {(s)} {\rightarrow} SrCl_{2} {(aq)}}[/latex]
         4. [latex]\ce{SrCl_{2} {(s)} {\rightarrow} Sr^{2+} {(aq)} + Cl^{-}}[/latex]
      3.  Which of the following represents the chemical equation of [latex]\ce{{(NH_{4})}_{3}PO_{4}{(s)}}[/latex] dissociating in water?
         1. [latex]\ce{{(NH_{4})}_{3}PO_{4} {(s)} {\rightarrow} {(NH_{4})}_{3}PO_{4} {(aq)} + H_{2}O}[/latex]
         2. [latex]\ce{{(NH_{4})}_{3}PO_{4} {(s)} {\rightarrow} 3NH_{4}^{+} {(aq)} + PO_{4}^{3-} {(aq)}}[/latex]
         3. [latex]\ce{{(NH_{4})}_{3}PO_{4} {(s)} {\rightarrow} NH_{4}^{+} {(aq)} + PO_{4}^{3-} {(aq)}}[/latex]
         4. [latex]\ce{{(NH_{4})}_{3}PO_{4} {(s)} {\rightarrow} {(NH_{4})}_{3}PO_{4} {(aq)}}[/latex]
      4. Write the chemical equation that represents [latex]\ce{Fe{(C_{2}H_{3}O_{2})}_{3} {(s)}}[/latex] dissociating in water.
      5. Write the complete ionic equation for the reaction of [latex]\ce{FeCl_{2} {(aq)}}[/latex] and [latex]\ce{AgNO_{3} {(aq)}}[/latex].
      6.  Is the following statement true? This is the complete ionic equation for the reaction of [latex]\ce{BaCl_{2} {(aq)}}[/latex] and [latex]\ce{Na_{2}SO_{4} {(aq)}}[/latex]: [latex]\ce{Ba^{2+}{(aq)} + 2Cl^{-}{(aq)} + 2Na^{+}{(aq)} + SO_{4}^{2-}{(aq)} {\rightarrow} 2Cl^{-}{(aq)} + 2Na^{+}{(aq)} + BaSO^{4}{(s)}}[/latex]
      7. Is the following statement true? This is the complete ionic equation for the reaction of [latex]\ce{KCl {(aq)}}[/latex] and [latex]\ce{NaC_{2}H_{3}O_{2} {(aq)}}[/latex]:[latex]\ce{K^{+}{(aq)} + Cl^{-}{(aq)} + Na^{+}{(aq)} + C_{2}H_{3}O_{2}^{-}{(aq)} {\rightarrow} Na^{+} {(aq)} + Cl^{-}{(aq)} + K^{+}{(aq)} + C_{2}H_{3}O_{2}^{-}}[/latex]
      8. Write the net ionic equation for the reaction of [latex]\ce{FeCl_{2} {(aq)}}[/latex] and [latex]\ce{AgNO_{3} {(aq)}}[/latex].
      9. What is the balanced net ionic equation for the reaction between [latex]\ce{HCl}[/latex] and [latex]\ce{Ca{(OH)}_{2}} {(aq)}[/latex]?
         1. 1. [latex]\ce{H^{+}{(aq)} + OH^{-}{(aq)} {\rightarrow} H_{2}O{(l)}}[/latex]
            2. [latex]\ce{2H^{+}{(aq)} + 2Cl^{-}{(aq)} + Ca^{2+}{(aq)} + 2OH^{-}{(aq)} {\rightarrow} 2H_{2}O{(l)} + 2CaCl_{2}{(aq)}}[/latex]
            3. [latex]\ce{2H^{+}{(aq)} + 2OH^{-}{(aq)} {\rightarrow} H_{2}O{(l)}}[/latex]
            4. [latex]\ce{2H^{+}{(aq)} + 2Cl^{-}{(aq)} + Ca^{2+}{(aq)} + 2OH^{-}{(aq)} {\rightarrow} 2H_{2}O{(l)} + 2Ca^{2+}{(aq)} + 2Cl^{-}{(aq)}}[/latex]
      10. What is the balanced net ionic equation for the following reaction: [latex]\ce{6HCl {(aq)} + 2Al {(s)} {\rightarrow} 2AlCl_{3}{(aq)} + 3H_{2}{(g)}}[/latex].
          1. [latex]\ce{6H^{+}{(aq)} + 6Cl^{-}{(aq)} + 2Al{(s)} {\rightarrow} 2Al^{3+}{(aq)} + 6Cl^{-}{(aq)} + 3H_{2}{(g)}}[/latex]
          2. [latex]\ce{H^{+}{(aq)} + Al{(s)} {\rightarrow} Al^{3+}{(aq)} + H_{2}{(g)}}[/latex]
          3. [latex]\ce{6H^{+}{(aq)} + 2Al{(s)} {\rightarrow} 2Al^{3+}{(aq)} + 3H_{2}{(g)}}[/latex]
          4. [latex]\ce{H^{+}{(aq)} {\rightarrow}  3H_{2}{(g)}}[/latex]
      11. Identify the spectator ions in the reaction between [latex]\ce{FeCl_{2}{(aq)}[/latex] and [latex]\ce{AgNO_{3}{(aq)}}[/latex]:
          1. [latex]\ce{Cl^{-}}[/latex] and [latex]\ce{NO_{3}^{-}}[/latex]
          2. [latex]\ce{Fe^{2+}}[/latex] and [latex]\ce{NO_{3}^{-}}[/latex]
          3. [latex]\ce{Ag^{+}}[/latex] and [latex]\ce{NO_{3}^{-}}[/latex]
          4. [latex]\ce{Ag^{+}}[/latex] and [latex]\ce{Cl^{-}}[/latex]
      12. Identify the spectator ions in the following reaction: [latex]\ce{BaCl_{2}{(aq)}}[/latex] and [latex]\ce{Na_{2}SO_{4}{(aq)}}[/latex].
          1. [latex]\ce{Na^{+}}[/latex] and [latex]\ce{Cl^{-}}[/latex]
          2. [latex]\ce{Ba^{2+}}[/latex] and [latex]\ce{Cl^{-}}[/latex]
          3. [latex]\ce{Ba^{2+}}[/latex] and [latex]\ce{SO_{4}^{2-}}[/latex]
          4. [latex]\ce{Na^{+}}[/latex] and [latex]\ce{SO_{4}^{2-}}[/latex]

Answers

1. a
2. b
3. b
4. [latex]\ce{Fe{(C_{2}H_{3}O_{2})}_{3} {(s)} {\rightarrow} Fe^{3+} {(aq)} + 3C_{2}H_{3}O_{2}^{-}{(aq)}}[/latex]
5. [latex]\ce{Fe^{2+}{(aq)} + 2Cl^{-}{(aq)} + 2Ag^{+}{(aq)} + 2NO_{3}^{-}{(aq)} {\rightarrow} Fe^{2+}{(aq)} + 2NO_{3}^{-}{(aq)} + 2AgCl{(s )}}[/latex]
6. True
7. True
8. [latex]\ce{2Cl^{-}{(aq)} + 2Ag^{+}{(aq)} {\rightarrow} 2AgCl {(s)}}[/latex]
9. a
10. c
11. b
12. a