39. The determination of copper in brass
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1 Microscale Chemistry The determination of copper in brass Topic Level Timing Description Metals chemical analysis. Post min. Apparatus (per group) In this experiment students dissolve some brass in nitric acid and compare the colour of the solution against standard copper solutions in a well-plate. This experiment has possibilities for use as an assessed practical. Two versions of the student worksheet are given (versions A and B). In version A students are guided through the calculations at the end. This version could be used to assess skills in doing the experiment/following instructions. In version B no help is given with the calculations. This version could be used to assess skills in treatment of results. Chemicals (per group) One student worksheet and one sheet of white paper Access to a balance Access to a fume cupboard One 10 cm 3 beaker One 10 cm 3 volumetric flask One plastic well-plate (24 well) eg Sigma ref: M9655 One plastic pipette eg Aldrich ref: Z13,503-8, fine-tip. Solutions contained in plastic pipettes, see p. 2 Nitric acid 5 mol dm 3 Deionised water Copper nitrate solution 0.50 mol dm 3 Brass turnings Observations The brass dissolves quickly to form a blue solution. This colour is due to the copper present in the brass. (This part of the experiment must be done in a fume cupboard since nitrogen dioxide is formed.) The intensity of the colour of this solution should lie within the range of intensities of colour of the standard solutions. Students find the nearest colour match and then calculate the copper content of the brass.
2 164 Microscale Chemistry Discussion Reference Safety Most brass contains about 60% copper (the remainder being zinc). Brass forms an interesting subject for a discussion on the structure of metals and alloys. Copper metal has a face-centered cubic structure (fcc) while the structure of zinc is hexagonal. As zinc is added to copper it substitutes in the lattice to form a distorted fcc structure (zinc atoms are ca 13% larger than copper). This distorted structure is difficult to deform and accounts for the greater strength of brass compared to pure copper. When the zinc content reaches about 36% a new body centered cubic phase appears and the strength increases markedly although the ductility is reduced. The optimum properties of strength and ductility for most uses of brass occur at about 40% zinc. A. Street and W. Alexander, Metals in the service of man, 10th edn. London: Penguin, Students must wear eye protection. It is the responsibility of the teacher to carry out a risk assessment.
3 Microscale Chemistry The determination of copper in brass Version A Instructions In this experiment you will be finding out how much copper there is in brass (an alloy of copper and zinc). You will dissolve the brass in nitric acid and compare the colour of the solution with that of solutions of various concentrations of copper. Part A Part B Preparing the brass solution 1. Weigh out, accurately, about 0.3 g of brass in a 10 cm 3 beaker. 2. Put the beaker in a fume cupboard. 3. Add 10 drops of nitric acid. 4. When the reaction subsides add a further 10 drops of nitric acid. 5. Repeat until all the brass has dissolved. 6. Using the pipette, transfer the solution to a 10 cm 3 volumetric flask. Add drops of water to the beaker to rinse and then transfer the washings to the flask. Make the volume in the flask up to the line with more water. Stopper the flask and then invert it a few times to mix. Preparing the standard copper solutions A B C D 1. Fill the well plate with solutions as indicated in the table below. Well No A1 A2 A3 A4 A5 A6 C1 C2 C3 C4 C5 C6 Drops of 0.50 mol dm 3 copper nitrate solution Drops of water
4 72 Microscale Chemistry Calculations Questions Version B Instructions Part A There should be a total of 40 drops in each well. Add 40 drops of the brass solution to well B3 (see diagram). Compare the intensity of the colour of your brass solution with the wells around it. The well that matches the intensity of colour of your brass solution represents the copper concentration in your brass solution eg if well A6 matches the colour of your brass solution then the copper concentration will be 0.50 x 18/40 mol dm Calculate the number of moles of copper in 10 cm 3 (the volume of the brass solution). 2. Multiply the value you obtained in (1) by the relative atomic mass of copper (63.5) to give the mass of copper in the brass solution. 3. Divide by the mass of brass used and express the result as a percentage. 1. Does the zinc interfere in any way in this analysis? Give reasons for your answer. 2. Can you suggest any way to improve the accuracy of this experiment? In this experiment you will be finding out how much copper there is in brass (an alloy of copper and zinc). To do this you will dissolve the brass in nitric acid and compare the colour of the solution with that of solutions of various concentrations of copper. Preparing the brass solution 1. Weigh out, accurately, about 0.3 g of brass in a 10 cm 3 beaker. 2. Put the beaker in a fume cupboard. 3. Add 10 drops of nitric acid. 4. When the reaction subsides add a further 10 drops of nitric acid. 5. Repeat until all the brass has dissolved. 6. Using a pipette, transfer the solution to the 10 cm 3 volumetric flask. Add drops of water to the beaker to rinse and then transfer the washings to the flask. Make the volume in the flask up to the line with more water. Stopper the flask and then invert it a few times to mix.
5 Microscale Chemistry 73 Part B Preparing the standard copper solutions A B C D 1. Fill the well plate with the solutions as indicated in the table below. Well No A1 A2 A3 A4 A5 A6 C1 C2 C3 C4 C5 C6 Drops of 0.50 mol dm 3 copper nitrate solution Drops of water Questions There should be a total of 40 drops in each well. Add 40 drops of your brass solution to well B3 (see diagram). Compare the intensity of the colour of your brass solution with the wells around it. From your results, calculate the copper content of your brass expressing your answer as a percentage. 1. Does the zinc interfere in any way in this analysis? Give reasons for your answer. 2. Can you suggest any way to improve the accuracy of this experiment?
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