Net Ionic Equations - AP Chemistry

1. Identify the spectator ions in the reaction: $NaCl + AgNO_3 \rightarrow NaNO_3 + AgCl$?

   $Na^+$ and $NO_3^-$ are spectator ions. These ions appear unchanged on both sides of the equation.

2. Identify the precipitate in the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$.

   $PbI_2$ is the precipitate. Lead iodide is insoluble and forms as a solid.

3. Which ions are typically not included in net ionic equations?

   Spectator ions. They remain unchanged and don't participate in the reaction.

4. Identify the spectator ions in the reaction: $Na_2S + 2HCl \rightarrow 2NaCl + H_2S$.

   $Na^+$ and $Cl^-$ are spectator ions. These ions remain in solution and don't react.

5. What is the net ionic equation for $H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O$?

   $2H^+ + 2OH^- \rightarrow 2H_2O$. Diprotic acid neutralized by two hydroxide ions.

6. What is the net ionic equation for $2HCl + Mg \rightarrow MgCl_2 + H_2$?

   $Mg + 2H^+ \rightarrow Mg^{2+} + H_2$. Active metal displaces hydrogen from acid.

7. Identify the spectator ions in the reaction: $Ca(NO_3)_2 + Na_2SO_4 \rightarrow CaSO_4 + 2NaNO_3$.

   $Na^+$ and $NO_3^-$ are spectator ions. These ions don't participate in the precipitation.

8. What is the net ionic equation for $AgNO_3 + NaCl \rightarrow AgCl + NaNO_3$?

   $Ag^+ + Cl^- \rightarrow AgCl$. Shows formation of insoluble silver chloride precipitate.

9. What is the net ionic equation for $K_2SO_4 + Ba(NO_3)_2 \rightarrow BaSO_4 + 2KNO_3$?

   $Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Formation of insoluble barium sulfate from ionic reactants.

10. Write the net ionic equation for $CaCO_3 \rightarrow CaO + CO_2$.

    No net ionic equation; no ions in the reaction. No ionic compounds are involved in this decomposition.

11. Write the net ionic equation for $NH_4Cl + NaOH \rightarrow NH_3 + NaCl + H_2O$.

    $NH_4^+ + OH^- \rightarrow NH_3 + H_2O$. Base removes proton from ammonium to form ammonia.

12. What is the net ionic equation for $2NaOH + FeCl_2 \rightarrow Fe(OH)_2 + 2NaCl$?

    $Fe^{2+} + 2OH^- \rightarrow Fe(OH)_2$. Iron hydroxide precipitates from solution.

13. What is the net ionic equation for $Zn + 2HCl \rightarrow ZnCl_2 + H_2$?

    $Zn + 2H^+ \rightarrow Zn^{2+} + H_2$. Metal displacement reaction producing hydrogen gas.

14. What is the net ionic equation for $FeCl_3 + 3NaOH \rightarrow Fe(OH)_3 + 3NaCl$?

    $Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3$. Iron hydroxide forms as an insoluble precipitate.

15. Identify the precipitate in the reaction: $Ca(OH)_2 + 2HCl \rightarrow CaCl_2 + 2H_2O$.

    No precipitate; only water forms. This is an acid-base reaction, not precipitation.

16. What is the net ionic equation for $2NaOH + CuSO_4 \rightarrow Cu(OH)_2 + Na_2SO_4$?

    $Cu^{2+} + 2OH^- \rightarrow Cu(OH)_2$. Hydroxide ions precipitate copper as insoluble hydroxide.

17. What is the net ionic equation for $2HCl + CaCO_3 \rightarrow CaCl_2 + CO_2 + H_2O$?

    $2H^+ + CO_3^{2-} \rightarrow CO_2 + H_2O$. Carbonate reacts with acid to form gas and water.

18. Write the net ionic equation for $Na_2S + 2HCl \rightarrow 2NaCl + H_2S$.

    $S^{2-} + 2H^+ \rightarrow H_2S$. Sulfide ion is protonated by acid to form gas.

19. Identify the precipitate in the reaction: $Mg(NO_3)_2 + 2NaOH \rightarrow Mg(OH)_2 + 2NaNO_3$.

    $Mg(OH)_2$ is the precipitate. Magnesium hydroxide is insoluble in water.

20. State the definition of an acid-base reaction.

    A reaction where an acid and a base react to form water and a salt. Proton transfer from acid to base forms neutral products.

21. Explain the role of spectator ions in a reaction.

    They do not participate in the chemical change. They appear on both sides unchanged during reaction.

22. Identify the precipitate in the reaction: $AgNO_3 + NaBr \rightarrow AgBr + NaNO_3$.

    $AgBr$ is the precipitate. Silver bromide is insoluble and precipitates.

23. Identify the spectator ions in the reaction: $KCl + AgNO_3 \rightarrow AgCl + KNO_3$.

    $K^+$ and $NO_3^-$ are spectator ions. These ions are present but don't participate in reaction.

24. State the definition of a precipitation reaction.

    A reaction where an insoluble solid forms and separates from solution. Soluble salts combine to form an insoluble product.

25. What is the net ionic equation for $K_2CO_3 + 2HNO_3 \rightarrow 2KNO_3 + CO_2 + H_2O$?

    $CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate ion reacts with acid to produce gas.

26. Write the net ionic equation for $HCl + NaOH \rightarrow NaCl + H_2O$.

    $H^+ + OH^- \rightarrow H_2O$. Shows only the acid-base neutralization, omitting spectators.

27. Write the net ionic equation for $2HCl + Mg(OH)_2 \rightarrow MgCl_2 + 2H_2O$.

    $2H^+ + 2OH^- \rightarrow 2H_2O$. Acid-base reaction producing water from ions.

28. Write the net ionic equation for $Na_2CO_3 + 2HCl \rightarrow 2NaCl + CO_2 + H_2O$.

    $CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate reacts with acid to produce gas and water.

29. What is a net ionic equation?

    An equation showing only the species that change during the reaction. Shows only species that actually react or are produced.

30. Write the net ionic equation for $2NaCl + Pb(NO_3)_2 \rightarrow PbCl_2 + 2NaNO_3$.

    $Pb^{2+} + 2Cl^- \rightarrow PbCl_2$. Lead chloride forms as an insoluble precipitate.

31. What does a complete ionic equation include?

    All ions present in the reaction, including spectator ions. Shows both reacting and non-reacting ions in solution.

32. What is the net ionic equation for $BaCl_2 + Na_2SO_4 \rightarrow BaSO_4 + 2NaCl$?

    $Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Shows formation of insoluble barium sulfate precipitate.

33. Identify the precipitate in the reaction: $CaCl_2 + Na_2CO_3 \rightarrow CaCO_3 + 2NaCl$.

    $CaCO_3$ is the precipitate. Calcium carbonate is insoluble in water.

34. Write the net ionic equation for $Al_2(SO_4)_3 + 3BaCl_2 \rightarrow 3BaSO_4 + 2AlCl_3$.

    $3Ba^{2+} + 3SO_4^{2-} \rightarrow 3BaSO_4$. Three equivalents of precipitation reaction occur.

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