0.35 μΜ Determine the molar absorptivity of has an absorbance of 0.42 at 610 nm in a 3.000-cm cell. 4.00×105 M¹ cm¯¹ -1 4.0×106 M¹ cm -1 4.0×105 M¹ cm -1 4.0×10³ M¹ cm -1 dichromate solution which

0.35 μΜ Determine the molar absorptivity of has an absorbance of 0.42 at 610 nm in a 3.000-cm cell. 4.00×105 M¹ cm¯¹ -1 4.0×106 M¹ cm -1 4.0×105 M¹ cm -1 4.0×10³ M¹ cm -1 dichromate solution which

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...

See similar textbooks

Similar questions

The absorbance of known concentration of a metal complex is obtained by UV-vis spectrophotometer. The results are tabulated: conc 0.2 0.3 04 0.5 Calculate the concentration of an unknown sample of the complex that has an absorbance of 0.43 0.31 b. 0.37 abs 0.27 0.41 0.55 0.69 c. 0.33 d. 0.35 e. 0.39
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 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
(d) The л/A behaviour for stearic acid (solid line) and oleic acid (dotted line) are shown below. Account clearly for the difference in behaviour for the two surface active materials. 60 50 40 Surface pressure 30 (mN/m) 20 10 0 0.1 0.2 0.3 0.4 area per molecule (nm²) 0.5 0.6 [7 marks]
The following data were obtained for a complex of nickel at 575 nm in a 1.00 cm cell. Using Microsoft Excel or some other graphing program, construct a calibration plot and accurately calculate the molar absorptivity (ε) for the nickel-complex at 575 nm. Standard # 1 2 3 4 A. 0.184 M-¹cm-1¹ B. 0.002 M-¹cm-¹ C. 5.425 M-¹cm-¹ Nickel Complex Concentration (M) 0.01 0.02 0.04 0.06 D. Not Enough Information to Determine Absorbance 0.058 0.109 0.220 0.328
What is the molar extinction coefficient at 625 nm for this copper (II) acetate solution? How was it determined? Standard Solution Concentration (M) Absorbance 1 0.025 0.049 2 0.050 0.153 3 0.100 0.242 4 0.200 0.499 5 0.250 0.694
c. Use the Table to answer the questions below Concentration (M) Absorbances 0.20 0.36 0.40 0.50 0.60 0.65 0.80 0.75 Plot the graph and attach your plot. Use the table to answer the following question i. If 1.1 cm cell was used. Calculate the molar absorptivity of Cr(Il). ii. What is the concentration of a compound with absorbance 0.60, if 2 cm cell is used.