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

Short answer

Net ionic equations: a. Ammonium sulfate and barium nitrate: \[ Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) \] b. Lead(II) nitrate and sodium chloride: \[ Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s) \] c. Sodium phosphate and potassium nitrate: No reaction. d. Sodium bromide and rubidium chloride: No reaction. e. Copper(II) chloride and sodium hydroxide: \[ Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s) \]

Step-by-step solution

a. Ammonium sulfate and barium nitrate

1. Write the chemical formulas for the reactants: Ammonium sulfate: \( (NH_4)_2SO_4 \) Barium nitrate: \( Ba(NO_3)_2 \) 2. Exchange anions and write the chemical formulas for the possible products: Ammonium nitrate: \( NH_4NO_3 \) Barium sulfate: \( BaSO_4 \) 3. Check solubility rules: Ammonium nitrate is soluble because all ammonium salts are soluble. Barium sulfate is insoluble because sulfate salts are generally insoluble, with some exceptions (which barium is not a part of). 4. Write the net ionic equation: Since barium sulfate is insoluble, the net ionic equation is: \[ Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) \]

b. Lead(II) nitrate and sodium chloride

1. Write the chemical formulas for the reactants: Lead(II) nitrate: \( Pb(NO_3)_2 \) Sodium chloride: \( NaCl \) 2. Exchange anions and write the chemical formulas for the possible products: Lead(II) chloride: \( PbCl_2 \) Sodium nitrate: \( NaNO_3 \) 3. Check solubility rules: Lead(II) chloride is insoluble because chloride salts are generally soluble, but lead(II) is an exception. Sodium nitrate is soluble because all nitrates are soluble. 4. Write the net ionic equation: Since lead(II) chloride is insoluble, the net ionic equation is: \[ Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s) \]

c. Sodium phosphate and potassium nitrate

1. Write the chemical formulas for the reactants: Sodium phosphate: \( Na_3PO_4 \) Potassium nitrate: \( KNO_3 \) 2. Exchange anions and write the chemical formulas for the possible products: Sodium nitrate: \( NaNO_3 \) Potassium phosphate: \( K_3PO_4 \) 3. Check solubility rules: Both sodium nitrate and potassium phosphate are soluble (all nitrates and sodium and potassium salts are soluble). 4. Since both possible products are soluble, no reaction occurs.

d. Sodium bromide and rubidium chloride

1. Write the chemical formulas for the reactants: Sodium bromide: \( NaBr \) Rubidium chloride: \( RbCl \) 2. Exchange anions and write the chemical formulas for the possible products: Sodium chloride: \( NaCl \) Rubidium bromide: \( RbBr \) 3. Check solubility rules: Both sodium chloride and rubidium bromide are soluble (all sodium and rubidium salts are soluble). 4. Since both possible products are soluble, no reaction occurs.

e. Copper(II) chloride and sodium hydroxide

1. Write the chemical formulas for the reactants: Copper(II) chloride: \( CuCl_2 \) Sodium hydroxide: \( NaOH \) 2. Exchange anions and write the chemical formulas for the possible products: Copper(II) hydroxide: \( Cu(OH)_2 \) Sodium chloride: \( NaCl \) 3. Check solubility rules: Copper(II) hydroxide is insoluble because hydroxide salts are generally insoluble, except alkali metal and some alkaline earth metal hydroxides. Sodium chloride is soluble because all sodium salts are soluble. 4. Write the net ionic equation: Since copper(II) hydroxide is insoluble, the net ionic equation is: \[ Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s) \]