Hi everyone, just did a lab today, and I wanted to double check my equations for each step, see if i could have done anything wrong, all feed back is appreciated!
Im going to write brief descripitions of the steps =D
Measure the mass of copper shavings and tip the copper into a beaker. slowly add concentrated HNO3 to the beaker containing the copper
My equation would look like: Cu (s) + 4HNO3 (aq) ==> Cu(NO3)2 (aq) + 2H2O (l) + 2NO2 (g)
Slowly add 4M NaOH.
Equation: 2 NaOH (aq) + Cu(NO3)2 (aq) ==> Cu(OH)2 (s) + 2 NaNO3 (aq)
Add boiling chips and water to the beaker, and heat it on a heating plate
Equation: Cu(OH)2 (s) ==> CuO(s) + H2O (l), the arrow separating the Cu(OH)2 and CuO has the heat element implemented, the triangle/delta symbol.
Place filtered CuO into a beaker and then add H2SO4.
Equation: CuO (s) + H2SO4 (aq) ==> CuSO4 (aq) + H2O (l)
Step 5: (here is the fun part)
Add zinc to the blue solution of Cu^2+. Put the solution into the fume hood while H2 gas is evolved. Stir until colorless
Equation: Here i thought it was Zn (s) + Cu^2+ (aq) ===> Cu(s) + Zn^2+ (aq)
or would this be more appropriate?: Zn (s) + CuSO4 (aq) ==> ZnSO4 (aq) + Cu(s) and bring this into net ionic form.
Test for completion of the reduction by pipetting the solution with 6M NH3 (aq). Simultaneously test CuSO4 with NH3
Equations: 1. Cu^2+ (aq) + 4 NH3 (aq) ==> Cu(NH3)4^2+ (aq)
(I cant see the blue solution with the zinc with NH3 unless zinc sulphate reacts with it so):
2. ZnSO4 (aq) + NH3 (aq) ==> Zn(OH)2 (s) + ??
All Help is greatly appeciated again