When measured in a 1.00 cm cuvette, a 4.1x10M solution of species X exhibited absorbances of 0.1025 and 0.533 at 530 nm and 325 nm, respectively. A 8.20x10M solution of species Y gave absorbances of 0.230 and 0.508 at 530 nm and 325 nm, respectively. Both species were dissolved in the same solvent, and the solvent'sabsorbance was 0.000 and 0.000 at 530 nm and 325 nm, respectively, in a 1 cm cuvette.Calculate the concentrations of X and Y in an unknown solution that yielded absorbance data of 0,683 at 530 nm and 1.351 at 325 nm in a 1.0 cm cuvetteA. X= 4.20 X10MY=3.20 x10+MO B. X1.25 X10MY= 4.20 x10-5MOCX-3.75X10MY-1 4x10MOD.X-3.80 x 10 MY 2.10K10M

The amount of a substance that dissolves in a specified volume of solvent to yield a solution is…

Answered: When measured in a 1.00 cm cuvette, a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The absorbance values observed during the determination of the complex stoichiometry with the Job method using the spectroscopic method were plotted and the following correct equations were obtained. According to this, what is the n value of the compound formed by Fe + 3 and SCN- ions?1. Line equation: y = 2.6188x + 0.1608 2. Line equation: y = -2.5963x + 2.7203
Molar absorptivity data for the cobalt and nickel complexes with 2,3-quinoxalinedithiol are εCo = 36400 and εNi = 5520 at 510 nm and εCo = 1240 and ε Ni = 17500 at 656 nm. A 0.361-g sample was dissolved and diluted to 150.0 mL. A 25.0-mL aliquot was treated to eliminate interferences; after addition of 2,3-quinoxalinedithiol, the volume was adjusted to 50.0 mL. This solution had an absorbance of 1.037 at 510 nm and 0.422 at 656 nm in a 1.00-cm cell. Calculate the concentration of nickel (in ppm) in the initial solution prepared by dissolving the sample.
Vanadium forms a complex with peroxide which absorbs at 460 nm. A 3.96 × 10 -4M solution of vanadium peroxide (Solution A) exhibited an absorbance of 0.624 at 460 nm in a 1.000-cm quartz cuvette; a blank solution containing only solvent had an absorbance of 0.029 at the same wavelength. a) Find the molar absorptivity of vanadium peroxide complex. b) An unknown solution of vanadium peroxide complex in the same solvent and cuvette had an absorbance of 0.375 at 460 nm. Find the concentration of vanadium peroxide in the unknown solution. c) A concentrated solution vanadium peroxide in the same solvent was diluted from an initial volume of 5.00 mL to a final volume of 25.00 mL (Solution C) had an absorbance of 0.733 in the same cuvette. What is the concentration of vanadium peroxide in the concentrated solution (Solution B)? Answer the following questions: 1. Molar Absorptivity (M³1 cm1) of vanadium peroxide complex from Solution A at 460 nm 2. Concentration of vanadium peroxide in unknown…
(b) The formula that relates the spin only magnetic moment (en) to the number of unpaired d-electrons (x) is: Heft = √√x(x+2) (1) For each of the following complexes, use this formula to calculate the number of unpaired electrons: Nan[Rh(CO)4], Hell0 BM Rb₂lMoBrn), Heft=2.83 BM (ii) Using the answers from part (b)(i): • Draw crystal field d-orbital energy level diagrams for each complex. • State the oxidation state of the metal in each complex. • Determine the value of n for each complex.
Most iron(III) compounds are very weakly colored, and do not lend themselves well to visible spectrometric analysis. Suggest a way in which their analyzability can be improved.
Molar absorptivity data for the cobalt and nickel complexes with 2,3-quinoxalinedithiol are εCo = 36400 and εNi = 5520 at 510 nm and εCo = 1240 and ε Ni = 17500 at 656 nm. A 0.361-g sample was dissolved and diluted to 150.0 mL. A 25.0-mL aliquot was treated to eliminate interferences; after addition of 2,3-quinoxalinedithiol, the volume was adjusted to 50.0 mL. This solution had an absorbance of 1.037 at 510 nm and 0.422 at 656 nm in a 1.00-cm cell. Calculate the concentration of cobalt (in ppm) in the initial solution prepared by dissolving the sample. Calculate the concentration of nickel (in ppm) in the initial solution prepared by dissolving the sample.
A 5.020 g sample of dried spinach leaves was digested in 50 mL of 6 mol L-¹ nitric acid. The resulting solution was filtered into a 100.0 mL flask which was made up to volume with deionised water. When this solution was analysed for iron by flame atomic absorption spectroscopy (Flame AAS) at 248.3 nm it had an absorbance of 0.1042. A set of iron standards were also run on the Flame AAS instrument, and these gave a linear calibration curve with the equation absorbance = 0.0704[Fe] +0.0011, where the concentration of iron is in mg L-¹. Calculate the iron content of the dried spinach leaves in µg g¹. 35.5 µg g-1 146.4 µg g1 -1 29.8 µg g¹ 10.42 µg g 1 -1 29.2 µg g
A2+ forms a pink-yellow complex ion in solution at Amax = 396 nm, while a red-qreen complex of B2* in solution at Amay = 550 nm. The resulting r absorbance spectra of the ions significantly overlap. The table below shows the molar absorptivities (M-1 cm-1) for the metal complexes at the two wavelengths. Analyte E 550 E 396 A2+ 9970 84 B2+ 34 856 To determine the concentration of these analyte ions in a mixture, the mixture absorbance is analyzed in a cell with a pathlength of 1.00 cm at 550 nm and at 396 nm, yielding values of 0.183 and 0.109 respectively. What is the molar concentrations of A2* in the sample? (round off to 3 SF scientific notation, What are the molar concentrations of B2* in the sample? (round off to 3 SF scientific notation. Show your complete solution below (or may attach photo of the written solution)
(a) Three components in a mixture have varying distribution constants between the mobile phase and the stationary phase. One of the components has a very high distribution constant. Would this component likely elute first or last and how would you design an experiment or modify the components of the separation to make it perform in the opposite manner? (b) One way to dramatically increase the sensitivity of a quadrupole mass spectrometer is to use a technique called selected ion monitoring (SIM). Explain how this technique works and why it improves sensitivity. Explain what dwell time means. Be sure to draw a diagram and describe how this analysis scheme works. Also, is there a compromise between a wide range of masses scanned and SIM? Explain in easy details.
Looking at a d6 Tanabe-Sugano diagram needed to assign the electronic transistion that corresponds to (lambda)max off 550 nm. Give that the Racah parameter for the iron complex in this complex is 848 cm^-1, determine the lighand field parameter in cm^-1 for the complex in the spin-state associated with lambda max. complex: [Fe(NH2trz)3]Cl2·2H2O
The DPD colorimetric method is used to determine the amount of residual chlorine in the sample. In this method, the free chlorine in the sample oxidizes the colorless amine N,N-diethyl-p-phenylenediamine to a colored compound that absorbs strongly at 520 nm. The analysis of a set of calibration standards gave the following results:ppm Cl2 Absorbance0.00 0.00310.50 0.12321.00 0.32411.50 0.54382.00 0.76422.50 0.95513.00 1.1565A 10.00 mL water sample from a public water supply was diluted to 250 mL and analyzed for free chlorine residual, giving an absorbance of 0.3210.A. Find the equation of the line.B. What is the molar absorptivity of Cl2 (FW = 70.9) at 250 nm?C. Calculate the free chlorine residual of the sample as ppm Cl2.D. Calculate ppm BaCl2 (FW = 208.2)?
A 0.402 g sample of a Ni() complex (molar mass of the complex is 294.96 g/mol) dissolved in 100.0 ml solution shows three absorption maxima in the visible region at A = 731 nm (A = 0.0830), A2 = 646 nm (A= 0.1375), and at Ag = 445 (A = 0.1265) The molar absorptivity (extinction coefficient, ca ) of the band at 731 nm is: %3! O o. 10.1 O b.5.4 O c. IL.8 O d. 9.0 O e. 6.09

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