Unknown Concentration

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The objective of this lab was to find the concentration of iron in a solution with an unknown concentration. Through the use of the Beer-Lambert Law and spectrophotometry, one can find the absorbance of solutions with known concentrations of iron and create a calibration curve that can be used find the concentration of the unknown solution, which was calculated to being 10.5ppm Fe. This value is somewhat precise due to its relative standard deviation of 1.65%, and the errors were kept to a minimum to increase accuracy.

I. Introduction
The purpose of this lab was to identify the unknown concentration of iron in a solution by qualitatively measuring the absorbance of electromagnetic radiation by the molecules in a solution. To examine
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Then the lab quest and spectrophotometer were prepared by setting the wave length to 508nm, the units to % transmittance, and the mode to “Events with Entry” and then the spectrophotometer was calibrated with a cuvette of solution A. Now that the lab quest was ready, the % transmittance was calculated for solutions B-I and recorded. Then the lab supplies were cleaned and put away.

III. Results and Discussion
Data:
Unknown Solution: Fe0257
Mass of ferrous ammonium sulfate: 0.0154
Concentration of the stock iron solution: 10.5 ppm Fe

Calibration Curve:

Solution
Volume of Stock Iron Soln. used (mL)
Conc. Fe in Calibration Solns. A-F (ppm)
Measured %T
Calculated Absorbance
A
0.00
0.000
99.993
0.00003040
B
2.00
0.110
98.861
0.004975
C
5.00
0.274
88.145
0.05480
D
10.00
0.548
80.123
0.09624
E
25.00
1.37
55.128
0.2586
F
50.00