List the balanced net ionic equations for all reactions that you observed in this experiment. Use your observations to provide evidence for all successful reactions completed and products formed. Where applicable, list ions in their coordination complex form; for example, when Cu2+ exists as the hexaaquo complex, use [Cu(H2O)6]2+ (aq) in your equation. Note: The zinc cation also forms a hexaaquo complex in aqueous solution

1)Cu(NO3)2 added to NaOH and distilled water

2)Then putting the solution under heat to create a solid CuO

3)Then decanting the solution and keeping the solid CuO

4)Then adding HCl to the solids

5)Then adding NH3 to the solution

6)Then adding H2SO4 to the solution

7)Add .15g of zinc to the solution and stir until evolution of gas stops giving you Cu+ (s)

8)Wash the copper metal from step 7 with about 5mL of 95% ethanol.

This, with so many parts, will almost take a book (well, a chapter anyway). How much of this do you understand.?

To determine the balanced net ionic equations for the given reactions, we need to analyze the chemical reactions that occur and the observations made. Let's break down each step and find the corresponding balanced equations:

1) Cu(NO3)2 added to NaOH and distilled water:
When copper (II) nitrate (Cu(NO3)2) is added to sodium hydroxide (NaOH) in water:
Cu(NO3)2 (aq) + 2NaOH (aq) → Cu(OH)2 (s) + 2NaNO3 (aq)

The observation in this step is the formation of a blue precipitate of copper (II) hydroxide (Cu(OH)2).

2) Solution heated to create solid CuO:
The copper (II) hydroxide from step 1 is heated:
2Cu(OH)2 (s) → CuO (s) + H2O (g)

The observation here is the formation of a black solid of copper (II) oxide (CuO) and the liberation of water vapor.

3) Solution decanted to keep the solid CuO:
This step does not involve any chemical reaction. We simply separate the CuO solid from the solution.

4) HCl added to the solids:
Hydrochloric acid (HCl) is added to the solid CuO:
CuO (s) + 2HCl (aq) → CuCl2 (aq) + H2O (l)

The observation in this step is the dissolution of the black CuO solid, resulting in the formation of a blue solution of copper (II) chloride (CuCl2) and water.

5) NH3 added to the solution:
Ammonia (NH3) is added to the copper (II) chloride solution:
CuCl2 (aq) + 2NH3 (aq) → [Cu(NH3)4]2+ (aq) + 2Cl- (aq)

The observation in this step is the formation of a deep blue solution due to the complexation of copper (II) ion with ammonia, resulting in the formation of the tetraamminecopper(II) complex, [Cu(NH3)4]2+.

6) H2SO4 added to the solution:
Sulfuric acid (H2SO4) is added to the solution containing the [Cu(NH3)4]2+ complex:
[Cu(NH3)4]2+ (aq) + H2SO4 (aq) → CuSO4 (aq) + 4NH4+ (aq)

The observation here is the formation of a blue solution of copper (II) sulfate (CuSO4) and the liberation of ammonium ions (NH4+).

7) .15g of zinc added to the solution:
Zinc (Zn) is added to the solution, resulting in the following reaction:
Cu2+ (aq) + Zn (s) → Cu (s) + Zn2+ (aq)

The observation in this step is the evolution of gas (hydrogen gas) as the zinc reacts with the copper (II) ions, resulting in the reduction of copper (II) ions to copper metal.

8) Copper metal washed with 95% ethanol:
No chemical reaction occurs in this step. We are merely washing the copper metal with ethanol to remove any impurities.

Overall, these are the balanced net ionic equations for the observed reactions in the given experiment. The produced evidence mentioned for each step confirms the formation of specific products and changes occurring during the reactions.