Q: what parameters and quality control measures are needed in spectrophotometer?
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Q: why does the choice and use of a blank matter for Spectrophotometry?
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explain the principle on how to determine the concentration of syrup using hand refractometer
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- During your experiment, you measure the absorbance of a sample to be 1.362. You have to convert thisabsorbance to methylene blue concentration (in ppm) using the absorbance measurements of two standardsolutions of known concentration:5 ppm: Absorbance 0.55510 ppm: Absorbance 1.211What is, in ppm, the concentration of your sample? Report using 3 decimal figures. Your answer must becorrect to 0.02 ppmpermanganate solution using the color wheel. ART II: INVESTIGATING ABSORBANCE AND PATHLENGTH 12. Based on Beer's law (A = ɛlC, A = absorbance, ɛ = molar absorptivity, I pathlength and C = concentration), what do you predict is the relationship between pathlength and absorbance? What about pathlength and transmittance?Give at least two reasons for using very dilute solutions when doing fluorescence spectrometry
- After determining the absorbance of several standards of known concentration, the trendline for a calibration curve (AKA a standard curve) plotting absorbance (y-axis) against concentration (M, x-axis) is determined to be y = 4.586x + -0.0010 %3D The absorbance of a solution of unknown concentration is determined to be 0.68. Calculate the concentration of the unknown solution in M. Give your answer to thrėe decimal places.A student mixed 5.00mL of 0.0020M Fe(NO3)3, 3.00mL of 0.0020M KSCN, and 3.00mL of distilled water. The mixture reacted to form a reddish solution indicating that FeSCN2+ was formed, according to the equation below. An absorbance of 0.21 was measured for this solution in a Spectrophotometer set at a wavelength of 447nm. Fe³+ (aq) + SCN (aq) FeSCN2+ (aq) A calibration curve was used to find the equilibrium concentration of the product of this reaction: y = 1895x + 0.027 Calculate the equilibrium concentration of the Fe³+ Report your answer to 4 sig figsA protein’s concentration can be determined spectrophotometrically by mixing it with an indicator called a Bradford reagent and measuring the amount of light absorbed by the protein. Use the plot below to determine the mass of protein (in micrograms, μμg ) in 100.0 mL of the solution if its absorbance is 0.398. A. 52 B. 3.1 C. 2.4 D. 0.52 E. 0.031
- A standard curve of absorbance vs. concentration has a linear trendline of y = 0.56x + 0.987. Use this trendline to calculate the concentration of an unknown sample that has an absorbance of 1.245.The data in the table are used to create a calibration curve for the determination of RNA from its absorbance at 260 nm. Use a spreadsheet and the least-squares method to determine the slope and y-intercept of the best straight line fit to the calibration curve. Do not subtract the blank reading when creating the calibration curve. m = b = RNA (µg) 0.00 10.67 21.34 32.01 42.68 mass= Absorbance at 260 nm 0.224 0.512 0.769 1.145 1.465 Using the slope and intercept of the calibration curve, determine the quantity of RNA in a sample that gives an absorbance of 0.636. µg µgYou measure a sample in your spectrophotometer that has an absorbance of 1.00. What is the concentration of your sample in M.
- The data in the table are used to create a calibration curve for the determination of RNA from its absorbance at 260 nm. Use a spreadsheet and the least-squares method to determine the slope and y-intercept of the best straight line fit to the calibration curve. Do not subtract the blank reading when creating the calibration curve. m= RNA (µg) 0.00 10.29 20.58 30.87 41.16 mass= Absorbance at 260 nm 0.227 0.452 0.786 1.078 1.296 Hg-1 Using the slope and intercept of the calibration curve, determine the quantity of RNA in a sample that gives an absorbance of 0.523. µg2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?Application Questions: Answer the following questions. Show all work for calculations and include units and the correct number of significant figures. 1. A solution of cobalt (III) chloride was analyzed using a UV/Vis spectrometer and produced the spectra shown in Fig. 4. What is the best wavelength to use for analyzing the samples? Best wavelength to analyze sample: Absorbance 0.600 0.500 0.400 0.300 0.200 0.100 0.000 375 400 450 425 475 500 525 550 Wavelength (nm) Molarity of FD&C #2 0.000 0.115 0.225 0.350 575 Figure 4. UV/Vis spectra of a cobalt (III) chloride solution for determination of the best wavelength for analysis. 8 600 625 2. Create a graph in Excel and add a linear trendline using the data given below. Calculate the molarity of a solution (to 3 significant digits) with an absorbance of 0.576 using the trendline equation from this graph. Show your work in the box below. DO NOT ATTACH THE FIGURE. Abs 0.002 0.187 0.442 0.699 650 675