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What do you think would happen if 0.5M K+ was used first to elute the sample in an ion exchange chromatography experiment? Why?
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- Four lab groups completed the experiment listed in the lab diluting lul of FCF dye into 1ml of water. The A625 values are listed below. For brilliant blue FCF, ɛ =97000 M-1cm–1 MW = 792.8 g/mol %3D Group # A625 % solution (in original stock sample) Percent ror (True value of Stock=0.2%) 1 0.244 0.199 0.5 0.209 0.170 15 3 0.306 0.250 25 4 0.187 0.153 0.235 a. Which group was more accurate? b. What are possible reasons group 3 had a much higher Absorbance than the others? c. What are possible reasons group 4 had a much lower Absorbance than the others?Below is a Beer's Law Plot for the concentration of a specific colored compound x. A solution of compound X is measured with the spectrophotometer to have an optical density of 0.60. a) What is the concentration of compound X in this solution. Answers must contain proper units for full credit. b) The absorbance of this compound was measured at 540 nm. Why was this absorbance chosen? 0.9 0.8 0.7 0.6 805 4 0.4 0.3 0.2 Absorbance at 540 mWe want to test different concentrations of an antibiotic to see how well it can kill bacteria on a petri dish. However, we have no idea how much (what concentration) of the antibiotic to use. Therefore, we are creating a dilution series in which we dilute the antibiotic 1:10 in PBS. Our stock solution of antibiotic is 200mg/mL and our stock concentration of PBS is 0.5M. Each petri dish will get 100uL of the diluted antibiotics. How would you make the dilution series? How many tubes would you need to make to test down to a final concentration of 20ug/mL antibiotic? HINT: PBS concentration is a distraction.