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The observed absorbance of the sample of serum is 0.200 and the absorbance of the blank is 0.049. The corrected absorbance of the serum sample = (0.200 – 0.049) = 0.151.
Use the regression equation
Absorbance = 0.0670*(µg iron in initial sample) + 0.0015
=====> µg iron in the initial sample = (0.151 – 0.001)/(0.067) = 2.23.
Note that we took 1.00 mL of the serum sample and diluted to a final volume of 5.00 mL. The micrograms of iron in the sample of serum will remain fixed, irrespective of the dilution. Hence, the concentration of iron in the serum sample = (micrograms of iron in the initial sample)/(volume of serum sample) = (2.23 µg)/(1.00 mL) = 2.23 µg/mL (ans).
please make an easy way to solve this problem??!! Step 3 Transfer4.00 mDof supe to a...
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3. A standard solution of Fe(II) [10.0 ppm) was prepared, the appropriate reagents were added, and a series of standard solutions were prepared and the transmittance of the solutions were read out as follows: Vol. of std solution (ml) Final vol. (mL) %T 0.00 100.0 100.0 5.00 100.0 77.7 25.00 100.0 30.2 50.00 100.0 10.4 (a) (3 pts) plot a calibration curve and find out the slope and y-intercept for the linearly related Absorbance with concentration. (b)...
3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium molar con- centration of FeNCS is assumed to equal the initial molar concentration of the SCN in the reaction mixture. Why is this assumption valid? A. A Set of Standard Solutions to Establish a The set of standard solutions is used to determine the absorbance of known molar con- centrations of FeNCS2. A plot of the data, known as a calibration curve, is used...