*13-7_ A solution containing the complex formed between Bi(III) and thiourea has a molar absorptivity of9.32 X 10³ L mol¹ cm¹ at 470 nm.00.5701 X00.A1910 919juloa wotWhat is the absorbance of a 4.25 × 10-5 M :I solution of the complex at 470 nm in a 1.00-cm cell?(a) W(b)(alios mo-00.1)What is the percent transmittance of the solution described in (a)?(c)200What is the molar concentration of the complex in a solution that has the absorbance described inTorito or tovo(a) when measured at 470 nm in a 2.50-cm cell?(non?+ 1rd

The value of absorbance according to the Beer-Lambert law is calculated as: A=εcl......(1) Where, c…

A solution containing the complex formed between Bi(III) and thiourea has a molar absorptivity of 9.32 x 10³ L mol¹ cm¹ at 470 nm. 01 00. gaivlozalb vd b918919 19 anoitulos 1004 (a) What is the absorbance of a 4.25 X 105 M solution of the complex at 470 nm in a 1.00-cm cell? 00.5. a com (b) What is the percent transmittance of the solution described in (a)? 02 doro 101 (allo mo-00.1) comm (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 2.50-cm cell? 1910 911 1970

A solution containing the complex formed between Bi(III) and thiourea has a molar absorptivity of 9.32 x 10³ L mol¹ cm¹ at 470 nm. 01 00. gaivlozalb vd b918919 19 anoitulos 1004 (a) What is the absorbance of a 4.25 X 105 M solution of the complex at 470 nm in a 1.00-cm cell? 00.5. a com (b) What is the percent transmittance of the solution described in (a)? 02 doro 101 (allo mo-00.1) comm (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 2.50-cm cell? 1910 911 1970

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter13: An Introduction To Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 13.8QAP: At 580 nm, which is the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar...

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The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1
Zinc(II) and the ligand L form a 1:1 complex that absorbs strongly at 600 nm. As long as the molar concentration of L exceeds that of zinc(II) by a factor of 5, the absorbance depends only on the cation concentration. Neither zinc(II) nor L absorbs at 600 nm. A solution that is 1.59 10-4 M in zinc(II) and 1.00 10-3 M in L has an absorbance of 0.352 in a 1.00-cm cell at 600 nm. Calculate (a) the percent transmittance of this solution. (b) the percent transmittance of this solution in a 2.50-cm cell. (c) the molar absorptivity of the complex.
The molar absorptivity (ε) of the FeSCN2+ complex ion is 4700 M-1 · cm-1 at a wavelength of 450 nm. Using a 1-cm sample tube, you measure the absorbance as (2.0x10-1). What is the concentration of FeSCN2+? What is your answer? _____________x10^_____
The molar absorptivity (ε) of the FeSCN2+ complex ion is 4700 M-1 · cm-1 at a wavelength of 450 nm. Using a 1-cm sample tube, you measure the absorbance as (2.0x10-1). What is the concentration of FeSCN2+?
A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580
The formation constant for the complexation of Mg2+ by EDTA is logKflogKf = 8.79. The conditional formation constant (Kf’) at pH 8 (αY4−αY4−= 4.2 x 10-3) is: 0.037 2.6 x 106 5.14 1.5 x 1011 6.4
Calculate the conditional formation constant (K'' NiY) of the [NiY]2- complex in 0.050 M NH3 and 0.090 M NH4Cl buffer solution. The formation constants of nickel amine complexes are respectively K1 = 102.75, K2 = 102.20, K3 = 101.69, K4 = 101.15, K5 = 100.71, K6 = 10-0.01. (KNiY = 4.2x1018, KNH3 = 1.74x10-5)
The complex formed between Cu(I) and 1,10- phenanthroline has a molar absorptivity of 7000 L cm-1 mol-1 at 435 nm, the wavelength of maximum absorption. What is the the absorbance of a 6.17 x 10-5 M solution of the complex when measured in a 1.00-cm cell at 435 nm.
The observed absorption band of the M2+ ion in the electronic spectrum of the hexaaqua complex is 7500 cm-1. How many kJ / mol is the crystal field cleavage of the tetraaqua complex of the same ion? (h = 6,626x10-34Js, c = 3x108ms-1)
A metal complex with a Molecular mass of 820 g mol−1 was dissolved and the solution made up to 25 mL in a volumetric flask. 1 mL was withdrawn, placed in a 100 mL volumetric flask and diluted to the mark. The absorbance (at 457 nm) of this solution (in a 1 cm cuvette) was 0.245. The extinction coefficient for this compound at 457 nm (ε530) = 11715 M-1cm-1.(a) calculate the concentration of the compound in the cuvette.(b) calculate the concentration of the compound in the 25mL volumetric flask(c) determine the mass of compound used to make the 25mL solution
[Ni(H2O)6]2+ Three peaks are observed at 9000, 14500, 24500 cm-1 in the UV-Vis spectrum. What is the crystal field stability energy of this complex in kJ/mol? (Ni:28) (h=6.625.10-34Js; c=3.108m/s; 1kJ/mol =83.6 cm-1) A. -293 B. -108 C. -129 D. -211 E. -352
The observed absorption band of the M2 + ion in the electronic spectrum of the hexaakua complex is 7500 cm-1. How many kJ / mol is the crystal field cleavage of the tetraakua complex of the same ion? (h = 6,626x10-34Js, c = 3x108ms-1) A. 142.63 B. 25.95 C. 2698.56 D. 39.88 E. 3333.33