Lab 6 lab report - Matthew Mueller Sept 28 2007 CHEM...

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Matthew Mueller Sept. 28, 2007 CHEM 207-01A THE COPPER CYCLE Objective This experiment involved the stepwise conversion of copper solid into various copper compounds, and eventually back to a copper solid. Part A – Oxidation Reduction Reaction Cu (s) + 4HNO 3(aq) Cu(NO 3 ) 2(aq) + 2H 2 O (l) + 2NO 2(g) Compound Amount M.W. Moles Other Cu 1.003 g 63.55 gmol 1.578 × 10 -2 mol N/A HNO 3 15 mL (concentrated) 63.02 gmol corrosive Procedure Observations 1. Weigh out about one gram of copper wire (approx. 30 1-cm strips), record mass, and put the copper in a 250 mL Erlenmeyer flask. Mass of Cu (s) = 1.003 g 2. In the fume hood carefully add 15 mL of concentrated nitric acid (HNO 3 ). Place the flask on a hot plate and heat till the copper is dissolved. (Add more nitric acid if it evaporates before all the copper has dissolved. -Copper dissolves into an initially green and eventually blue solution. -A brown gas is given off from the solution as the copper dissolves. 3. Take the flask off the hot plate after all the copper had
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dissolved and cool. Part B – Precipitation Reaction Cu(NO 3 ) 2(aq) + 2NaOH (aq) Cu(OH) 2(s) + 2NaNO 3(aq) Compound Amount M.W. Moles Other NaOH 30 mL (6 M) 40.00 gmol 0.18 mol Cu(NO 3 ) 2 187.57 gmol Procedure Observations 1. Add 40 mL of DI water to the solution of copper (II) nitrate. 2. Carefully and slowly add 30 mL of 6M NaOH while stirring gently. Add the NaOH till the solution turns basic. The pH of the solution can be tested by
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