Determination of Concentration Using the Spectronic 20
Abstract:
The purpose of this experiment was to determine the concentration of an unknown amount of copper sulfate using the spectronic 20. Four solutions of different concentrations of H₂O and CuSO₄ were put into the spectronic 20 to observe their absorption of light. Then, a graph was created to plot down the measurements. Using the calibration curve of the graph, the concentration of the unknown substance was found out to be .12M.
Background/Introduction:
Beer’s law (which states that by holding the pathlength of a particular substance- in this case, CUSO₄ - constant, the absorption of light is directly proportional to the concentration of the substance) was used in this experiment to find the absorption measurement of the concentration of an unknown amount of copper sulfate.
Procedure:
Four different concentrated solutions of CuSO₄ (0.13M, 0.11M, 0.090M, and 0.070M) were prepared by crushing the copper sulfate with a mortar and pestle. The copper sulfate was then added into different volumetric flasks with 10.0 mL of distilled water. Also, 10 drops of concentrated nitric acid were added to the solutions. By placing each solution in the spectronic 20 device, the absorption measurements were noted down and graphed.
Data Collection:
M = mol/vol CuSO₄ + 5H₂O CuSO₄ = 249.5896g
0.13M 0.13M = mol/ 0.100L = 0.013 mol (249.5896g) = 3.245g
0.11M 0.11M = mol/0.100L = 0.011 mol (249.5896g) = 2.745g
0.090M 0.090M = mol/0.100L = 0.009 mol (249.5896g) = 2.246g
0.070M 0.070M = mol/0.100L = 0.007 mol (249.5896g) = 1.747g
Concentration (M) Wavelength Determination (Trial One) Wavelength Determination (Trial Two)
0.13M 50%T 49%T
0.11M 55%T 54%T
0.090M 62%T 59%T
0.070M 68%T 67%T
Concentration (M) Absorbance Measurements (Trial One) 2-log(%T) Absorbance Measurements (Trial Two) 2-log(%T)
0.13M 0.30M 0.30M
0.11M 0.26M 0.27M
0.090M 0.21M 0.23M
0.070M 0.17M 0.17M
Unknown amount of CuSO₄: 52.0%T
2-log (%T)
2-log (52.0) =
The purpose of this experiment was to determine the concentration of an unknown amount of copper sulfate using the spectronic 20. Four solutions of different concentrations of H₂O and CuSO₄ were put into the spectronic 20 to observe their absorption of light. Then, a graph was created to plot down the measurements. Using the calibration curve of the graph, the concentration of the unknown substance was found out to be .12M.
Background/Introduction:
Beer’s law (which states that by holding the pathlength of a particular substance- in this case, CUSO₄ - constant, the absorption of light is directly proportional to the concentration of the substance) was used in this experiment to find the absorption measurement of the concentration of an unknown amount of copper sulfate.
Procedure:
Four different concentrated solutions of CuSO₄ (0.13M, 0.11M, 0.090M, and 0.070M) were prepared by crushing the copper sulfate with a mortar and pestle. The copper sulfate was then added into different volumetric flasks with 10.0 mL of distilled water. Also, 10 drops of concentrated nitric acid were added to the solutions. By placing each solution in the spectronic 20 device, the absorption measurements were noted down and graphed.
Data Collection:
M = mol/vol CuSO₄ + 5H₂O CuSO₄ = 249.5896g
0.13M 0.13M = mol/ 0.100L = 0.013 mol (249.5896g) = 3.245g
0.11M 0.11M = mol/0.100L = 0.011 mol (249.5896g) = 2.745g
0.090M 0.090M = mol/0.100L = 0.009 mol (249.5896g) = 2.246g
0.070M 0.070M = mol/0.100L = 0.007 mol (249.5896g) = 1.747g
Concentration (M) Wavelength Determination (Trial One) Wavelength Determination (Trial Two)
0.13M 50%T 49%T
0.11M 55%T 54%T
0.090M 62%T 59%T
0.070M 68%T 67%T
Concentration (M) Absorbance Measurements (Trial One) 2-log(%T) Absorbance Measurements (Trial Two) 2-log(%T)
0.13M 0.30M 0.30M
0.11M 0.26M 0.27M
0.090M 0.21M 0.23M
0.070M 0.17M 0.17M
Unknown amount of CuSO₄: 52.0%T
2-log (%T)
2-log (52.0) =