You need to make a stock solution of a known copper concentration for your experiment. You start by weighing out a piece of pure copper wire which has a mass of 0.211 g. You then add 1.0 mL of 12 M HNO3, 3.0 mL of H2O and 2.0 mL of 12 M NH4OH to dissolve the copper metal.
The moles of copper that are in the solution = 0.00332 mols. Now I need to find the final molarity of copper in the solution.

Question

You need to make a stock solution of a known copper concentration for your experiment. You start by weighing out a piece of pure copper wire which has a mass of 0.211 g. You then add 1.0 mL of 12 M HNO3, 3.0 mL of H2O and 2.0 mL of 12 M NH4OH to dissolve the copper metal. 
The moles of copper that are in the solution = 0.00332 mols. Now I need to find the final molarity of copper in the solution.

aaronq · Answer

divide the moles by the total volume (in liters) of solution