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

Taryn Lambert

Chemistry

8 February, 21:00

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.

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Answers (1)

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Amare Grimes · Answer 1

The first step to determine the molarity is to find the volume used in the solution.

1.0 mL + 3.0 mL + 2.0 mL = 6.0 mL

3.34 mmol : 6.0 mL = 0.5567 mol/L

The molarity of copper in the solution is 0.5567 mol/L.