When measured in a 1.00 cm cuvette, a 4.1x10M solution of species X exhibited absorbances of O.1025 and 0.533 at 530 nm and 325 nm, respectively. A 8.20x10 M 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's absorbance 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 cuvette OAX=4.20 x10 M Y=3.20 X10M O B.X-1.25 X10M Y=4.20 x10-SM OCX-375x10 M Y=14x10M OD.X=380 x 10M Y-2.10x10M

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.

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

A simultaneous determination for cobalt (Co) and nickel (Ni) can be based upon absorption by their respective 8-hydroxyquinolinol complexes. Molar absorptivities corresponding to their absorption maxima are as follows: Molar Absorptivity, 8 365 nm 700 nm Со 3600 430 Ni 3200 10 The absorbances of a sample at 365 nm and 700 nm with a 1.00-cm cell are 0.600 and 0.040, respectively. Calculate the molar concentration of nickel (ex:) and cobalt (cco) in the sample. A. CN = 3.20 x 10$ M, cco = 3.60 x 10:5 M B. CNi = 3.60 x 10$ M, cco =3.20 × 10$ M C. CNi = 1.00 x 10³ M, cco = 4.13 x 10$ M D. CNi = 8.70 x 105 M, cco = 9.10 x 105 M CNi = 9.10 x 10$ M, cco = 8.70 x 10 M E.

The molar extinction coefficient of B (MW = 180) is 4×10° lit mol' cm'. One liter solution of C which contains 0.1358 g pharmaceutical preparation of B, shows an absorbance of 0.411 in a 1 cm quartz cell. The percentage (w/w) of B in the pharmaceutical preparation is: (a) 10.20 (b) 14.60 (c) 20.40 (d) 29.12

The accompanying absorption data were recorded at 390 nm in a 1.00 cm cells for a continuous variation study of the colored product formed between Cd and the complexing reagent R. 1. Solution Reagent volumes, mL A390 cCd = 1.25 x 104 M cR = 1.25 x 104 M 10.00 0.00 0.00 1 9.00 1.00 0.174 2 8.00 2.00 0.353 3 7.00 3.00 0.530 4 6.00 4.00 0.672 5 5.00 5.00 0.723 4.00 6.00 0.673 7 3.00 7.00 0.537 8. 2.00 8.00 0.358 9 1.00 9.00 0.180 10 0.00 10.00 0.000 Find the ligand-to-metal ratio in the product. b. Calculate an average value for the molar absorptivity of the complex and its uncertainty. Assume that in the linear portions of the plot the metal is completely complexed. Calculate Kf for the complex using the stoichiometric ratio determined in (a) and the absorption data at the point of intersection of the two extrapolated lines. а. c.