Synthesis of Copper Compounds - Copy

Synthesis of Copper Compounds - Copy - Synthesis of Copper...

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Synthesis of Copper Compounds Introduction
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This laboratory report aims to summarize and discuss the experiment in which regular metallic copper metal was used to synthesis various different copper compounds with the aim of ultimately recovering the initial copper at the end. The metallic copper was subjected to a variety of solutions and compounds which resulted in chemical reactions that formed new copper compounds. The initial metallic copper was obtained in the form of a wire which was weighed in order to keep track of the amount of copper that was recovered at the conclusion of the experiment. The copper wire was dissolved in concentrated nitric acid (HNO 3 ), a colourless highly corrosive and toxic strong acid, to form copper (II) nitrate (Cu(NO 3 ) 2 ). Sodium hydroxide was added to form Copper (II) Hydroxide in the form of an alkaline gelatinous solution. Copper (II) hydroxide (Cu(OH) 2 ) was then formed by heating to decompose the gelatinous solution and recover the copper as black Copper (II) oxide. Then using vacuum filtration, the Copper (II) oxide was isolated from the aqueous solution. With the addition of Sulphuric acid (H 2 SO 4 ), the black copper (II) oxide dissolved to form a blue solution called copper (II) sulphate pentahydrate (CuSO 4 ·H 2 O). Finally, with the addition of hydrochloric acid and zinc to displace the copper ions from the solution, the copper settles and can then be extracted and heated to isolate copper the copper metal. The copper is then weighed at the end and the percent recovery is calculated by comparing the initial mass with the final mass. Through this report, the experiment will be elaborated upon through the observations and results obtained relating to the specific chemical reactions that occurred to take copper from one form to the next. Ultimately, the entire experiment is summarized through this flow equation: Cu Cu(NO 3 ) 2 Cu(OH) 2 CuO CuSO 4 ·H 2 O Cu
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Procedure The experimental procedure used for this experiment was outlines in the CHEM 120L lab manual, Experiment #1. All steps were followed without deviation. The metallic copper wire had an initial weight of 1.1589g. In order to measure the final mass of copper recovered the evaporating dish was first weighed and found to be 49.3357g. The evaporating dish and remaining copper combined weighed 51.4912g which gave a final mass of 2.1555g of copper. The percent recovery of copper was therefore: % Cu Recovery = Final Mass = 2.1555g = 1.859 x 100 = 186% Initial Mass 1.1589g 1. The reaction of Cu with nitric acid Cu (s) + 4HNO 3(aq) Cu(NO 3 ) 2(aq) + 2NO 2(g) + 2H 2 O (l) For the synthesis of copper (II) nitrate, concentrated nitric acid was mixed with the
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This note was uploaded on 02/20/2009 for the course CHEM 120 taught by Professor Gilbert during the Fall '08 term at Waterloo.

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Synthesis of Copper Compounds - Copy - Synthesis of Copper...

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