In the experiment "Beer-Lambert's Law and Spectrophotometry", you prepared a calibration plot similar to the one pictured below. What is the approximate concentration of a solution whose absorbance is 0.35? Calibration Plot 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1 0. 0.02 0.03 0.04 0.05 0.01 Absorbance
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- A student measures the absorbance of a solution in lab a total 4 times and obtained the following results:0.219, 0.224, 0.206, 0.223a. Using the Grubbs test, decide whether any values should be rejected at the 95% confidence level.b. What should the student report as the 95% confidence interval for the absorbance of the solution?Test Tube Number Cobalt Chloride Concentration (mol/mL) Absorbance at 510 nm 1 0.000 0.000 2 0.009 0.042 3 0.018 0.92 4 0.027 0.139 5 6 0.036 0.045 0.190 0.236 7 (Unknown) 0.151 1. what is the concentration of unknown cobalt chloride solution? 2. why is the absorbance at the absorption peak ?A Beer’s Law plot has a slope of 0.0222ppm-1 with an intercept of zero. Determine the concentration of a solution that has an absorbance of 0.851. Show your work.
- "[FeSCN2+]eq is calculated using the formula: [FeSCN2+]eq = Aeq/Astd? [FeSCN2+]std where Aeq and Astd are the absorbance values for the equilibrium and standard test tubes, respectively. [FeSCN2+]std is calculated assuming all moles of SCN- go to form [FeSCN2+]std as shown below. " My question is; what do they mean by standard test tubes respectively? Are they talking about the container it's being held in? For me it's 10[FeSCN2+]eq is calculated using the formula: [FeSCN2+]eq = Aeq/Astd? [FeSCN2+]std where Aeq and Astd are the absorbance values for the equilibrium and standard test tubes, respectively. [FeSCN2+]std is calculated assuming all moles of SCN- go to form [FeSCN2+]std as shown below. My question is; what do they mean by standard test tubes respectively? Are they talking about the container it's being held in? For me it's 10 ml.A calibration curve was created to determine the quantity of protein in a solution. The calibration curve has the form of a straight line with the equation ?=0.0182?+0.007 where ? is the corrected absorbance of the solution and ? is quantity of protein in the solution in units of micrograms (μg). Determine the quantity of protein in a solution that has an absorbance of 0.305. A blank solution has an absorbance of 0.060. The answer (Quantity of protein) should be in units of (μg)
- Calculate the molar concentration for a sample dye solution with a measured absorbance of 0.304. (Hint: Use linear regression analysis.). Final answer in 3 significant figures.Experiment: UV-Vis Spectrophotometry and Beer’s Law Absorption of Light of Dyes in Beverages A calibration curve for the orange dye in a soft drink was obtained by plotting absorbance against concentration (M) for a series of solutions of known concentration. The slope of the calibration curve was 226 L/mol and the intercept was -0.011. The absorbance of an unknown soft drink was found to be 0.333 under the same conditions as the calibration curve. Calculate the concentration of the orange dye in the soft drink.pls answer letter d,e , and f
- state if true or false 1. Prior to a fixed point or wavelength reading, spectral scanning can be done to determine the maximum absorbance wavelength of a sample. 2. The purpose of a diffraction grating is the same as that of a prism. 3. In any UV-VIS spectrophotometer, the light is filtered first to a single wavelength or narrow range before it hits the sample 4. In any UV-VIS spectrophotometer setup, the detector always comes right after the sample container. 5. It is necessary to set the blank before each reading even if the only difference between the sample solutions is the amount of analyte. 6. Prior to a fixed point/wavelength reading, spectral scanning can be done to determine the maximum absorbance wavelength of a sample.explain the results of this experimet Table 2 Absorbance vs CoCl2 concentration Test Tube Number Cobalt Chloride Concentration (mol/mL) Absorbance at 510 nm 1 0.000 0.000 2 0.009 0.024 3 0.018 0.055 4 0.027 0.085 5 6 0.036 0.045 0.112 0.138 7 (Unknown) 0.088A student completed Test Solution 1: 2.5 mL of 2.00×10−32.00×10−3 M Fe(NO3)3Fe(NO3)3 mixed with 0.5 mL of 2.00×10−32.00×10−3 M NaSCNNaSCN and topped with 2.0 mL of 0.1 M HNO3HNO3 to make a total of 5.0 mL solution. The absorbance of the solution was measured, and the calibration curve was used to calculate [FeSCN2+][FeSCN2+] at equilibrium. Concentration of [FeSCN2+][FeSCN2+] at equilibrium was 7.5×10−57.5×10−5 M. Complete the given chart and the calculation that follows. initial [Fe3+], M2= initial SCN[Fe3+], M2= M Fe3+Fe3+ + SCN−SCN− ↽−−⇀↽−−⇀ FeSCN2+FeSCN2+ Initial Change Equilibrium Calculate the equilibrium Kc for this reaction (to two significant figures