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Spectrophotometric Analysis of CopperExperiment 1Make a plot of absorbance readings for each of the solutions, absorbance vs. wavelength. Use the following table to keep track of your absorbances. Your plots/graphs should look similar to the ones given below.Wavelength (x axis)Absorbance CuSO4 (y axis) graph #1Absorbance COCl2(y axis) graph #14000.000.004200.000.104400.000.074600.000.074800.000.165000.000.235200.000.225400.000.135600.020.075800.050.046000.090.006200.140.006400.220.006600.350.006800.500.007000.630.00What was the highest absorbance for the CuSO4?_______ Make sure the spectrometer is setto this wavelength for Experiment 2.Experiment 2I have already calculated the actual concentration of Cu2+ ion in your samples. This is a simple dilution using the following equation: (conc. of original solution )*(volume of standard Cu2+) = (concentration of dilute solution)*(total solution volume)CuSO4(mL)HNO3(mL)Cu+2 Concentration(Mol/L)(x axis)Absorbance(y axis)Cuvette 146(0.06)(4)/(10)= 0.024Cuvette 273(0.06)(7)/(10)= 0.042Cuvette 310(0.06)(10)/(10)= 0.06Make a plot(graph) of absorbance as a function of the copper (II) concentration [M] in each of the standards. Similar to the one below.Experiment 3Determine the copper concentrations in your two unknown samples from the calibration plot. (Find the concentration that matches the measured absorbance of each sample.)Record this information.AbsorbanceEstimated ConcentrationUnknown 10.37Unknown 20.52