18-16. A compound with a molecular mass of 292.16 was dissolved in a 5-mL volumetric flask. A 1.00-mL aliquot was withdrawn, placed in a 10-mL volumetric flask, and diluted to the mark. The absorbance at 340 nm was 0.427 in a 1.000-cm cuvet. The molar absorptivity for this compound at 340 nm is ɛ340 = 6 130 M-1 cm-!. (a) Calculate the concentration of compound in the cuvet. (b) What was the concentration of compound in the 5-mL flask? (c) How many milligrams of compound were used to make the 5-mL solution?
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- A 5.00-mL sample of blood was treated with trichloroacetic acid to precipitate proteins. After centrifugation, the resulting solution was brought to pH 3 and extracted with two 5-mL portions of methyl isobutyl ketone containing the lead-complexing agent APCD. The extract was aspirated directly into an air/acetylene flame and yielded an absorbance of 0.527 at 283.3 nm. Five-milliliter aliquots of standard solutions containing 0.400 and 0.600 ppm of lead were treated in the same way and yielded absorbances of 0.396 and 0.599. Find the concentration of lead in the sample in ppm assuming that Beer’s law is followed.At 21 °C, a solution of 12 mL each of 0.00200 M Fe3+ and 0.001000 M SCN- was mixed and brought to 25.0 mL with 0.1 M HNO3. The absorbance at 450 nm was measured to be 0.350 (A450 = 0.350). This solution was then heated to 45 °C and the absorbance at 450 nm was measured to be 0.142 (A450= 0.142). Is the reaction: Fe3+(aq) + SCN -(aq) → FeSCN2+(aq) exothermic or endothermic? Explain.A 5.00-mL sample of blood was treated with trichloroacetic acid to precipitate proteins. After centrifugation, the resulting solution was brought to pH 3 and extracted with two 5-mL portions of methyl isobutyl ketone containing the lead-complexing agent APCD. The extract was aspirated directly into an air/acetylene flame and yielded an absorbance of 0.569 at 283.3 nm. Five-milliliter aliquots of standard solutions containing 0.400 and 0.600 ppm of lead were treated in the same way and yielded absorbances of 0.396 and 0.599. Please calculate the concentration of lead in the sample in ppm.
- A compound with a formula mass of 292.16 was dissolved in solvent in a 5-mL volumetric flask and diluted to the mark. A 1.00-mL aliquot was withdrawn, placed in a 10-mL volumetric flask, and diluted to the mark. The absorbance measured at 340 nm was 0.427 in a 1.000-cm cuvet. The molar absorptivity for this compound at 340 nm is 6 130 M21 cm21. (a) Calculate the concentration of compound in the cuvet. (b) What was the concentration of compound in the 5-mL flask? (c) How many milligrams of compound were used to make the 5-mL solution?The molar absorptivities of compounds X and Y were measured with pure samples of each: ε (M-1 cm-1) λ (nm) X Y 272 16,440 3,870 327 3,990 6,420 A mixture of compounds X and Y in a 1.00-cm cell had an absorbance of 0.957 at 272 nm and 0.559 at 327 nm. Find the concentrations of Y in the mixture. 4.43 x 10-5 M 3.03 x 10-6 M 5.95 x 10-5 M 3.56 x 10-4 MThe accuracy of a spectrophotometer can be evaluated by preparing a solution of 60.06-ppm K2Cr2O7 in 0.0050 M H2SO4 and measuring its absorbance at a wavelength of 350 nm using a cell with a pathlength of 1.00 cm. The absorbance should be 0.640. What is the molar absorptivity of K2Cr2O7 at this wavelength? 3134 cm-1 M-1
- 11. [15'] the molar absorptivity (extinction coefficient) of benzene (C6H6) equals 100 M-¹ cm¹ at 260 nm. (Assume that this number is independent of solvent or other effects) a) What concentration would give an absorbance of 1.0 in a 1 cm cell at 260 nm? b) If the density of pure, liquid benzene is 0.8 g cm²³, what 'thickness' of pure benzene would also give an absorbance of 1.0 at 260nm?A compound X is to be determined by UV-visible spectrophotometry. A calibration curve is constructed from standard solutions of X with the following results: 0.50 ppm, A = 0.24; 1.5 ppm, A = 0.36; 2.5 ppm, A = 0.44; 3.5 ppm, A = 0.59; 4.5 ppm, A = 0.70. A solution of unknown X concentration had an absorbance of A = 0.50. Find the slope and in te rcept of the calibration curve, the standard error in Y, the concentration of the solution of unknown X concentrat ion, and the standard deviation in the concentration of X. Construct a plot of the calibration curve and determine the unknown concentra tion by hand from the plot. Compare it to that obtained from the regression line.A juice concentrate was colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the sample solution and various concentrations of the standard glucose solution were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbances at 480 nm for distilled water, glucose standard, and for the sample are 0.052, 1.702, and 0.926, respectively. What is the reducing sugar concentration (mg/mL) in the juice concentrate? The equation of the line was plotted to be: y = 1.6656x - 0.0885 0.578 mg/mL 577.9 mg/mL 57.7 mg/mL 5.78 mg/mL
- Quinine in a 1.664 g antimalarial tablet was dissolved in sufficient 0.10 M HCl to give 500 mL of solution. A 15.00 mL aliquot was then diluted to 100.0 mL with the acid. The fluorescense intensity for the diluted sample at 347.5 nm provided a reading of 288 on an arbitrary scale. A standard 100 ppm quinine solution registered 180 when measured under conditions identical to those for the diluted sample. Calculate the mass in milligrams of quinine in the tablet.In spectrophotometric analysis, the relationship between the absorbance A and the analyte's concentration C is: A = ebC + Ablank What is the molar extinction coefficient I and its absolute uncertainty if A is 0.68 ± 0.06; Ablank is 0.06 ± 0.01; b is 1.00 cm; and C is (0.45 ± 0.03)x10-5 mol/L?The following volumes of a solution containing 1.10 ppm Zn2+ were pipetted into separatory funnels each containing 5.00 mL of an unknown zinc solution: 0.00, 1.00, 4.00, 8.00 and 12.00. Each was extracted with three 5 mL aliquots of CCl4 containing an excess of 8-hydroxyquinoline. The extracts were then diluted to 25.0 mL and their fluorescence measured with a fluorometer. The results for the standard addition calibration were as follows: Volume Std. Zn2+ / mL [Zn2+] / ppm Fluorometer Reading 0.00 6.12 1.00 7.41 4.00 11.16 8.00 15.68 12 20.64 a) Determine the concentration on Zn2+ ions in each of the standard solutions coming from the coming from the 1.10 ppm Zn2+ solutions, Please show your working