The ultimate purpose of this lab is to find how much copper is in brass using the visible spectroscopy, in addition to the introduction of Beer’s law, a physical law that can be utilized to determine the unknown concentration of a metal ion in a solution if its absorbance is calculated; you can accurately measure it by means of a standard graph called a calibration curve. Also colorimetry, a technique “used to determine the concentration of colored compounds in solution” (Housecroft, Catherine) is also an objective that was designed to be introduced. Lastly, determine the concentration of a solution with a previously unknown concentration using a calibration curve and plot it with different standard solutions. In order to accomplish this, the
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Foremost, I displayed the absorbance of brass that was contained in each milliliter of concentrated nitric acid by saying how much brass was in each milliliter Cu(NO₃)₂. Next, I used the molarity formula M= mol/L to intently calculate the grams of copper within each specified concentration of brass (i.e. 0.1M = 0.0127). Furthermore, using the newly found grams of brass, I needed to create my calibration curve graph by plotting my known values in the graph. Lastly, using one of the points of my absorbance (0.2 abs, .121M), I solved for my total amount of copper in brass. Likewise, I substituted my molarity into my linear equation (y= 1.711x-0.004 → 0.121=1.711x-0.004) solved by using stoichiometry (shown above in the lower right-hand corner of page 1) and found the total amount of copper in brass. In the midst of our data/results and our prolonged contemplation of an appropriate method of resuming our lab, we some possible sources of error that might occur in an experiment are letting the copper (II) nitrate dilute too much by adding too much water to the solution. This could be a feasible threat to the accuracy of the lab, for it can lead to inaccurate molarities on the calibration curve graph and therefore, result in a wrong quantity of copper in brass. Also, an insufficient transfer of the diluted Cu(NO₃)₂ could consequently, induce defective evidence given from the spectrometer which is crucial to the success of the lab. Finally, not following instructions given from the teacher could also confirm the failure from the lab from the
Foremost, I displayed the absorbance of brass that was contained in each milliliter of concentrated nitric acid by saying how much brass was in each milliliter Cu(NO₃)₂. Next, I used the molarity formula M= mol/L to intently calculate the grams of copper within each specified concentration of brass (i.e. 0.1M = 0.0127). Furthermore, using the newly found grams of brass, I needed to create my calibration curve graph by plotting my known values in the graph. Lastly, using one of the points of my absorbance (0.2 abs, .121M), I solved for my total amount of copper in brass. Likewise, I substituted my molarity into my linear equation (y= 1.711x-0.004 → 0.121=1.711x-0.004) solved by using stoichiometry (shown above in the lower right-hand corner of page 1) and found the total amount of copper in brass. In the midst of our data/results and our prolonged contemplation of an appropriate method of resuming our lab, we some possible sources of error that might occur in an experiment are letting the copper (II) nitrate dilute too much by adding too much water to the solution. This could be a feasible threat to the accuracy of the lab, for it can lead to inaccurate molarities on the calibration curve graph and therefore, result in a wrong quantity of copper in brass. Also, an insufficient transfer of the diluted Cu(NO₃)₂ could consequently, induce defective evidence given from the spectrometer which is crucial to the success of the lab. Finally, not following instructions given from the teacher could also confirm the failure from the lab from the