Question

Determine net ionic equations, if any, occuring when aqueous solutions of the following reactants are mixed. Select "True" or "False" to indicate whether or not the stated reaction (or "no reaction") correctly corresponds to the expected observation in each case. Lead(II) nitrate and sodium chloride; No reaction occurs. Sodium bromide and hydrochloric acid; No reaction occurs. Nickel(II) chloride and lead(II) nitrate; Pb2+(aq) + 2Cl-(aq) --> PbCl2(s) Magnesium chloride and sodium hydroxide; No reaction occurs. Ammonium sulfate and barium nitrate; Ba2+(aq) + SO42-(aq) --> BaSO4(s)

Answer 1

The correct net ionic equations include the formation of lead(II) chloride from lead(II) nitrate and sodium chloride, the formation of magnesium hydroxide from magnesium chloride and sodium hydroxide, and the formation of barium sulfate from ammonium sulfate and barium nitrate.

Step-by-step explanation:

When determining net ionic equations for reactions between aqueous solutions, it is necessary to consider the solubility rules to decide whether a solid precipitate forms. Let's consider each pair of reactants:

• Lead(II) nitrate and sodium chloride: True, a reaction occurs. Lead(II) nitrate reacts with sodium chloride to form a precipitate of lead(II) chloride. The net ionic equation is Pb^{2+}(aq) + 2Cl^-(aq) → PbCl_2(s).
• Sodium bromide and hydrochloric acid: False, no reaction occurs because all species remain in their ionic form in solution.
• Nickel(II) chloride and lead(II) nitrate: False, no reaction occurs since both potential products, nickel nitrate and lead chloride, are soluble.
• Magnesium chloride and sodium hydroxide: False, a reaction occurs. Magnesium hydroxide, an insoluble precipitate, is formed. The net ionic equation is Mg^{2+}(aq) + 2OH^-(aq) → Mg(OH)_2(s).
• Ammonium sulfate and barium nitrate: True, a reaction occurs. A precipitate of barium sulfate forms. The net ionic equation is Ba^{2+}(aq) + SO_4^{2-}(aq) → BaSO_4(s).

Answer 2

For 1: The correct answer is False.

For 2: The correct answer is True.

For 3: The correct answer is True.

For 4: The correct answer is False.

For 5: The correct answer is True.

Step-by-step explanation:

Net ionic equation of any reaction does not include any spectator ions. If no net ionic equation is formed, it is said that no reaction has occurred.

Spectator ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form. Solids, liquids and gases do not exist as ions.

• For 1: Lead(II) nitrate and sodium chloride

The chemical equation for the reaction of lead (II) nitrate and sodium chloride is given as:

`Pb(NO_3)_2(aq.)+2NaCl(aq.)\rightarrow PbCl_2(s)+2NaNO_3(aq.)`

Ionic form of the above equation follows:

`Pb^(2+)(aq.)+2NO_3^-(aq.)+2Na^+(aq.)+2Cl^-(aq.)\rightarrow PbCl_2(s)+2Na^+(aq.)+2NO_3^-(aq.)`

As, sodium and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

`Pb^(2+)(aq.)+Cl^-(aq.)\rightarrow PbCl_2(s)`

Hence, the correct answer is False.

• For 2: Sodium bromide and hydrochloric acid

The chemical equation for the reaction of sodium bromide and hydrochloric acid is given as:

`NaBr(aq.)+HCl(aq.)\rightarrow NaCl(aq.)+HBr(aq.)`

Ionic form of the above equation follows:

`Na^(+)(aq.)+Br^-(aq.)+H^+(aq.)+Cl^-(aq.)\rightarrow Na^+(aq.)+Cl^-(aq.)+H^+(aq.)+Br^-(aq.)`

There are no spectator ions in the equation. So, the above reaction is the net ionic equation.

Hence, the correct answer is True.

• For 3: Nickel (II) chloride and lead(II) nitrate

The chemical equation for the reaction of lead (II) nitrate and nickel (II) chloride is given as:

`Pb(NO_3)_2(aq.)+NiCl_2(aq.)\rightarrow PbCl_2(s)+Ni(NO_3)_2(aq.)`

Ionic form of the above equation follows:

`Pb^(2+)(aq.)+2NO_3^-(aq.)+Ni^(2+)(aq.)+2Cl^-(aq.)\rightarrow PbCl_2(s)+Ni^(2+)(aq.)+2NO_3^-(aq.)`

As, nickel and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

`Pb^(2+)(aq.)+Cl^-(aq.)\rightarrow PbCl_2(s)`

Hence, the correct answer is True.

• For 4: Magnesium chloride and sodium hydroxide

The chemical equation for the reaction of magnesium chloride and sodium hydroxide is given as:

`MgCl_2(aq.)+2NaOH(aq.)\rightarrow Mg(OH)_2(s)+2NaCl(aq.)`

Ionic form of the above equation follows:

`Mg^(2+)(aq.)+2Cl^-(aq.)+2Na^+(aq.)+2OH^-(aq.)\rightarrow Mg(OH)_2(s)+2Na^+(aq.)+2Cl^-(aq.)`

As, sodium and chloride ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

`Mg^(2+)(aq.)+OH^-(aq.)\rightarrow Mg(OH)_2(s)`

Hence, the correct answer is False.

• For 5: Ammonium sulfate and barium nitrate

The chemical equation for the reaction of ammonium sulfate and barium nitrate is given as:

`(NH_4)_2SO_4(aq.)+Ba(NO_3)_2(aq.)\rightarrow BaSO_4(s)+2NH_4NO_3(aq.)`

Ionic form of the above equation follows:

`2NH_4^(+)(aq.)+SO_4^(2-)(aq.)+Ba^(2+)(aq.)+2NO_3^-(aq.)\rightarrow BaSO_4(s)+2NH_4^+(aq.)+2NO_3^-(aq.)`

As, ammonium and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

`Ba^(2+)(aq.)+SO_4^(2-)(aq.)\rightarrow BaSO_4(s)`

Hence, the correct answer is True.