Please help with both A and B parts

3. In Part 2 sodium hydroxide solution is added to the copper(II) nitrate solution to precipitate copper(II) hydroxide. Not only do we need to add enough sodium hydroxide to precipitate all of the copper ion, but, as you should have shown in Problem 2, there is excess nitric acid present and we must add sufficient sodium hydroxide to neutralize this as well. Show that NaOH(aq) was added in excess by completing the following calculations. a. Calculate the volume (in mL ) of 3.5mol/LNaOH(aq) needed to completely precipitate 0.510gNaCu2+ in solution. b. Calculate the volume (in mL ) of 3.5mol/LNaOH(aq)neededtocompletelyneutralizetheexcessnitricacid. Assume that the concentration of nitric acid, after it has reacted with copper, is 8.5 mol/L and the volume of the solution is 4.5mL. 3. In Part 2 sodium hydroxide solution is added to the copper(II) nitrate solution to precipitate copper(II) hydroxide. Not only do we need to add enough sodium hydroxide to precipitate all of the copper ion, but, as you should have shown in Problem 2, there is excess nitric acid present and we must add sufficient sodium hydroxide to neutralize this as well. Show that NaOH(aq) was added in excess by completing the following calculations. a. Calculate the volume (in mL ) of 3.5mol/LNaOH(aq) needed to completely precipitate 0.510gNaCu2+ in solution. b. Calculate the volume (in mL ) of 3.5mol/LNaOH(aq)neededtocompletelyneutralizetheexcessnitricacid. Assume that the concentration of nitric acid, after it has reacted with copper, is 8.5 mol/L and the volume of the solution is 4.5mL