If a molecule fluoresces, what are the advantages of using a fluorimeter instead of a molecular spectrophotometer to detect the fluorophore. How do these instruments differ from one another? How are they the same?
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If a molecule fluoresces, what are the advantages of using a fluorimeter instead of a molecular spectrophotometer to detect the fluorophore. How do these instruments differ from one another? How are they the same?
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- Many ions form colored solutions when dissolved in water. For example, aqueous Cu2+ solutions are light blue and aqueous Ni2+ solutions look light green. These metals in particularare often found in stainless steel. Would you expect their presence in your samples to interfere in the spectrophotometric analysis of permanganate at 525 nm? Why or why not? I think the answer is that I would expect the Cu2+ in my samples to interfere but not Ni2+ because the Ni2+ is green, signifying a higher wave length that the spectrometer wouldn't be able to pick up on because it was only set to 525 (blue-ish) where as the green is 530-ish. I just want to make sure thanks!0.1040 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water. The solution was then diluted by a factor of 20. The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 3.109 ppm, What is the weight percentage of copper in the original solid sample? Keep four significant figures in your final answer. Do not try to include the "%" in your answer. e.g. if your final answer is 10.01%, only write 10.01 in the box.Explain why the concentration of zinc cannot be determined directly using a spectrophotometer.
- Quantitative Analysis by External Standard Method Calcium in a juice sample is determined by atomic absorption spectrophotometry. A stock solution of calcium is prepared by dissolving 1.834 g of CaCl, 2H20 in water and diluting to 1000.0 mL. A substock calcium solution was prepared by transferring 10.00 mL of the stock to a 100.00 mL volumetric flask and diluting to the mark. Three standard solutions of calcium were prepared by transferring 2.500 mL. 5.00 mL and 10.00 mL of substock to 50.00 mL volumetric flasks and diluting to the mark. The sample is prepared by transferring 1.000 mL of fruit juice from the original bottle to a 25.00 mL flask and diluting to the mark. Strontium chloride is added to all solutions before dilution to avoid phosphate interference. Instrumental response of the standards is measured against the blank, and the following readings are recorded: 9.10, 18.6 and 37.0. The sampie reading is 28.1. Using the multipoint method, find the concentration of calcium in…0.1120 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water. The solution was then diluted by a factor of 25. The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 2.982 ppm, What is the weight percentage of copper in the original solid sample? Keep four significant figures in your final answer.why does the choice and use of a blank matter for Spectrophotometry?
- If the standard addition intercept is the major source of uncertainty, find the uncertainty in the concentration of Sr in tooth enamel in parts per million. Find the 95% confidence interval for Sr in tooth enamel.In order to measure riboflavin in a breakfast cereal, a 5.00-gram sample of the cereal was extracted with acetic acid and filtered. The extract was transferred to a 50.0 mL volumetric flask and diluted to the mark. The sample was transferred to a cuvette and the fluorescence was measured. The instrument read 59 units (Fluorescence units –an arbitrary scale). 24.00 mL of the cereal extract was sample was mixed with 1.0 mL of a riboflavin standard that was 0.500 ug/mL. The fluorescence of this mixture was measured and read 94 fluorescence units. Calculate the concentration of riboflavin per gram of cereal (use µg/gram of cereal).10. The concentration of haemoglobin in a blood sample was determined by spectrophotometry. A standard curve of the absorbance at 412 nm of several solutions of known haemoglobin concentrations was created. The data for the standard curve is shown below. a. Calculate the linearity coefficient (r), y-intercept and slope. b. What is the concentration (in ug/mL) of haemoglobin in your sample if the absorbance obtained at 412 nm was 0.303? Absorbance Concentration of standard solution (pg/ml) (412nm) 0.069 1 0.113 2 0.201 4 0.377 8. 0.730 16
- A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.144. Assuming that the best fit linear line of the standard curve was y=0.04144x+0.01521 (μgmL), calculate the percent protein by mass in the original protein powder.3. The lead in a swab sample, lead standards, together with a blank were made up in 5.00 mL volumetric flasks using 0.2 % HNO3. 20 μL aliquots of these solutions were injected into the spectrophotometer and the absorbance measured at 217 nm. The following results were obtained. lead / ppb Absorbance 0 0.0591 10.00 0.0858 50.00 0.1926 100.0 0.3260 150.0 0.4594 200.0 0.5929 Swab sample 0.3700 (a) Determine the amount of lead in the swab sample in μg.How did you decide on the wavelength at which you will read the absorbance of the diluted solutions? What is the importance of reading the absorbance of diluted solutions at λmax? What will vary if you chose a wavelength 20 nm lower or higher than your chosen wavelength? (Minimum of 8 sentences)
