Homework Answers
Let us take the molar absorbity constant for Fe+3 be 0.11 * 10^4 (M^-1 cm^-1).
Then using equation of Beer's law as follows:
A = eLc
0.169 = 0.11 * 10^4 (M^-1 cm^-1) * 550.8 * 10^-7 cm * c
=> c = (0.169 * 10^3)/(0.11 * 550.8) M
=> c = 2.78933 M
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3. A simulated water sample is determined to have an absorbance of 0.169 at 550.8 nm....
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Answer 2) To measure the concentration of phosphorous in a water sample, Phosphorous was first converted...
Answer
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The figure below depicts the absorbance of the antibiotic Ampicillin at 610 nm as a function...
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Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
Chloride in a water sample can be determined indirectly by
atomic absorption spectrometry by precipitating chloride as AgCl(s)
with a measured amount of AgNO3 that is excess of the chloride
content of the sample. The AgNO3 is added and the sample is
centrifuged. The remaining Ag+ in the solution (supernatant) is
quantified and the chloride is measured by assuming that chloride
was quantitatively precipitated.
Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
Two analytes, X and Y, have overlapping absorbance spectra for 200 nm <^ < 800 nm. None the less, determine the concentration of each analyte in an unknown mixture, using the information from absorbance measurements at two a’s. For calibration, individual standards of X and Y were analyzed at a concentration of 2.0 x 10-4M. A 1.0 cm pathlength cell was used. The following data were obtained: Sample Absorbance at 22 Absorbance at 2#1 350 nm 650 nm Unknown Mixture...
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Answer
2) To measure the concentration of phosphorous in a water sample, Phosphorous was first converted into a color complex in the presence of ammonium molybdate and SnClo. The absorbance of a series of standard phosphorous solutions was measured by a spectrophotometer and gave the calibration curve y 1.150 x, where y is the absorbance of phosphorous complex at 690 nm while x is the concentration of P in ppm. An unknown natural water sample was collected. 10.00 mL of...
20.00 mL unknown sample is diluted to 250.0 mL. Absorbance is 0.2430 Absorbance for 70.00 ppm std is .950 What is ppm concentration in the original undiluted sample?
The figure below depicts the absorbance of the antibiotic Ampicillin at 610 nm as a function of its concentration (in ug/mL). The equation for the line of best fit was: y 0.01054+0.1606 Determine the concentration of an unknown sample of Ampicillin, if its absorbance at 610 nm was 0.450 0.5 0.45 0.4 0.35 0.3 0.25 0.2 15 20 Concentration ug /ml 25 10 Absorbance
The figure below depicts the absorbance of the antibiotic Ampicillin at 610 nm as a function of its concentration (in pg/mL). The equation for the line of best fit was: y = 0.01054x + 0.1606 Determine the concentration of an unknown sample of Ampicillin, if its absorbance at 610 nm was 0.350. 0.5 0.45 Absorbance 10 25 30 15 20 Concentration ug/ml Select one: O a. 5.79 x 104 pg/mL Ob. 17.0 pg/mL O c.0.164 ug/mL O d. 18.0 pg/mL
Chloride in a water sample can be determined indirectly by
atomic absorption spectrometry by precipitating chloride as AgCl(s)
with a measured amount of AgNO3 that is excess of the chloride
content of the sample. The AgNO3 is added and the sample is
centrifuged. The remaining Ag+ in the solution (supernatant) is
quantified and the chloride is measured by assuming that chloride
was quantitatively precipitated.
Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
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