1) A Chem 102 Student prepared a cobalt coordination compound. Parts "a-c" refer to this problem. a) Next, she analyzed the cobalt content of the compound by preparing a series of known concentration cobalt solutions and prepared a Beer's law graph of absorbance (Y) versus concentration(X). The equation of the line was determined using Excel to be: Y=7.50 X the coordination compound and ultimately diluted it to a total volume of 100.0 mL and measured its absorbance to be 0.310. Calculate the percent cobalt (by mass) in the compound. Where X is concentration in Molarity. She weighed 1.1050 g of
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- Ligand X forms a complex with both cobalt and copper, each of which has a maximum absorbance at 510 nm and 645 nm, respectively. A 0.256 g sample containing cobalt and copper was dissolved and diluted to a volume of 100.0 mL. A solution containing ligand X was added to a 50.0 mL aliquot of the sample solution and diluted to a final volume of 100.0 mL. The measured absorbance of the unknown solution was 0.484 at 510 nm and 0.354 at 645 nm, when measured with a 1.00 cm cell. The molar absorptivities of the cobalt and copper complexes at each wavelength are shown in the table. Molar Absorptivity (e, M-¹cm-¹) Wavelength λ, nm 510 645 [Co²+] = What is the concentration of cobalt and copper in the final diluted solution? [Cu²+] = Co 36437 1241 wt% Co²+ = Cu 5526 17520 What is the weight percent of cobalt (FM = 58.933 g/mol) and copper (FM = 63.546 g/mol) in the 0.256 g sample? wt% Cu²+ == M M %Ligand X forms a complex with both cobalt and copper, each of which has a maximum absorbance at 510 nm and 645 nm. respectively. A 0.243 g sample containing cobalt and copper was dissolved and diluted to a volume of 100.0 mL. A solution containing ligand X was added to a 50.0 mL aliquot of the sample solution and diluted to a final volume of 100.0 mL. The measured absorbance of the unknown solution was 0.503 at 510 nm and 0.368 at 645 nm, when measured with a 1.00 cm cell. The molar absorptivities of the cobalt and copper complexes at each wavelength are shown in the table. Molar Absorptivity (c. M-'cm-¹) Wavelength [Co² = A, nm [Cu²+] = 510 645 3.125 x10-5 Incorrect Co 2.867 x10-5 3.7630 x 10² What is the concentration of cobalt and copper in the final diluted solution? 1282 Cu 5707 18090 M MIn optical analysis, what are the methods used to calculate the concentration ofa solution from the absorbance measurements of colorimeters?
- A series of standard iron-phenanthroline [Fe(phen)3]2+ complex ion solutions were prepared. The absorbance of each solution was measured at a wavelength of 510 mm. A calibration curve of absorbance vs. concentration was then plotted to obtain a linear equation of y = 0.0018x+0.0749. The absorbance of an unknown [Felphenly solution was measured to be 0.326. Calculate the concentration of the complex ion. NOTE! Report your answer as a WHOLE #. Type your answer...A solution containing 1.00mg iron (as the thiocyanate complex) in 100mL was observed to transmit 70.0% ofthe incident light compared to an appropriate blank. (a) What is the absorbance of the solution at thiswavelength? (b) What fraction of light would be transmitted by a solution of iron four times as concentrated?A solution of copper(II) sulfate is observed to be blue in color. The maximum absorbance is expected to occur in what wavelength range? 500-560 nm (green) 380-435 nm (violet) 610-750 nm (red) 580-595 nm (yellow) 435-480 nm (blue)
- Roberta decided to find out the content of nickel (Ni) in a sample. She dissolved the 0.0882 g sample in about 30 mL of nitric acid, and after adding an excess of 8- hydroxyquinolinol (HQL), she diluted the solution with deionized water to a final volume of 250 mL. This final solution showed an absorbance of 0.694 at 365 nm, the wavelength of maximal absorbance of the Ni (HQL) complex, when measured in a 1.00 cm cuvette. Knowing that the trendline from the calibration curve for the Ni(HQL) complex at 365 nm is y = 1500x + 0.029 and that the atomic mass of nickel is 58.693 g/mol, calculate the percent content of Ni by mass in the sample. What is the % nickel by mass in the sample? (a) 5.31 percent (b) 7.38 percent. (c) 7.70 percent. (d) 7.4 percent. (e) None of theseA solution containing 1.00 mg ion (as the thiocyanate complex) in 100 mL was observed to transmit 70 % of the incident light compared to an appropriate blank. (a) What is the absorbance of this solution at this wavelength? (b) What fraction of light would be transmitted by a solution of iron four times as concentrated?When preparing a solution containing 1.00 mg of iron (as thiocyanate complex) in 100 mL, it is found to transmit 85.0% of the incident light, compared to an appropriate blank. What will be the % transmittance of a solution three times more concentrated in iron?
- . A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cell . A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cell0.718g sample of [Cr(acac)3] was converted completely to CrO42 solution in 500 ml flask. 10 ml of this solution was diluted with water to 500 ml and the absorbance of this solution was found to be 0.345 at A = 350nm. Another standard solution of Cro4 2 with 5.25 x10-5 M concentration has an absorbance of 0.215 at the same wave length. The percentage of chromium in the sample is: (Atomic mass of Cr = 52 g/mol) * 5A transition metal ion, M, forms a coloured complex with a monodentate ligand L. Portions of a 0.05 mol dm-³ solution of M are mixed with portions of a solution containing 0.05 mol dm-³ of L so that the total volume of the resulting mixture is always 10 cm³. The colour intensity of the complex in each mixture is measured using a colorimeter. The graph of the results is 0 1 2 3 3 4 5 6 7 8 9 10 cm³ of M 10 9 8 7 6 5 4 3 2 1 0 - cm³ of L What is the formula of the complex? A ML B ML₂ C ML₂ с D D ML4 Colour intensity 7:2