To establish a standard curve for a Big standard curve using Biuret, the spectrophotometer wavelength is set on which value? the wavelength at which the copper(il) compiex's absorption value is the lowest A Big standard curve should not be drawn up using the Buiret method the wavelength at which the copper(l) complex's absorption value is the highest the wavelength at which the Big-Bluret complex's absorption value is the highest the wavelength at which the Big-Biuret complex's absorption value is the lowest

To establish a standard curve for a Big standard curve using Biuret, the spectrophotometer wavelength is set on which value? the wavelength at which the copper(il) compiex's absorption value is the lowest A Big standard curve should not be drawn up using the Buiret method the wavelength at which the copper(l) complex's absorption value is the highest the wavelength at which the Big-Bluret complex's absorption value is the highest the wavelength at which the Big-Biuret complex's absorption value is the lowest

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter12: Spectrochemical Methods

Section: Chapter Questions

Problem 16P

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Which statement is true regarding interligand charge-transfer (ICT or LL'CT) complexes? Group of answer choices In an ICT transition, an electron is promoted from a pi-acceptor ligand orbital to one on a pi-donor ligand ICT transitions are only observed for complexes that have tetrahedral geometries The metal center plays the most influential role an ICT transition For a given complex, the ICT molar absorptivity is at its maximum when the pi-donor and pi-acceptor ligands are co-planar
Why is the observed magnetic moment less than the spin only magnetic moment for a hexaureachromium (III) chloride complex?
An absorbance versus concentration data for the thiocyanatoiron(III) complex at 510 nm and makes a Beer's law plot.Based on the plot, what [Fe(SCN)2+] would the student report for a solution that has an absorbance of 0.300 at 510 nm? Also select all below closely matches the procedures to be followed in this experiment and why they are being carried out. 1) A Beer's law plot will be used as a means to determine the equilibrium concentration of the thiocyanatoiron(III) complex. 2)A Beer's law plot will be used to confirm known values of the equilibrium constant for the formation of the thiocyanatoiron(III) complex. 3)To make the Beer's law calibration graph, the formation equilibrium for the thiocyanatoiron(III) complex will be flooded with a large excess of thiocyanate ion. 4)To make the Beer's law calibration graph, the formation equilibrium for the thiocyanatoiron(III) complex will be flooded with a large excess of iron(III) ion.
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. What is the n value of the compound formed by Fe + 3 and SCN- ions? 1. Line equation: y = 2.6188x + 0.16082. Line equation: y = -2.5963x + 2.7203
Consider the solvatochromic complex, [Mo(bipy)(CO)4]. The complex has a MLCT peak in the UV-vis spectrum. This peak is at 533 nm in acetonitrile solvent and at 584 nm in benzene solvent. In a 50:50 acetonitrile:benzene mixture, the peak is at 559 nm. Is the mixture of acetonitrile and benzene immediately surrounding the [Mo(bipy)(CO)4] molecules less than, equal to, or greater than a 50:50 mixture (acetonitrile:benzene)? Justify your answer. (HINT: Do you need to convert the wavelengths to a more appropriate unit?)
The red color of soil is often due to the presence of iron. Metal ions are extracted from soil by stirring the soil in acid and then filtering the solution. One method for the analysis of Fe2+ is to form the highly colored Fe2+–thioglycolic acid complex. The complex absorbs strongly at 535 nm. Calibration standards of 1.00, 2.00, 3.00, 4.00, and 5.00 ppm are prepared by transferring appropriate amounts of a 10.0 ppm working solution of Fe2+ into separate 50-mL volumetric flasks, each of which contains 5 mL of thioglycolic acid, 2 mL of 20% w/v ammonium citrate, and 5 mL of 0.22 M NH3. After diluting to volume and mixing, the absorbances of the standards are measured. a)What is the effect on the reported concentration of iron in the sample if there is a trace impurity of Fe2+in the ammonium citrate?
The red color of soil is often due to the presence of iron. Metal ions are extracted from soil by stirring the soil in acid and then filtering the solution. One method for the analysis of Fe2+ is to form the highly colored Fe2+–thioglycolic acid complex. The complex absorbs strongly at 535 nm. Calibration standards of 1.00, 2.00, 3.00, 4.00, and 5.00 ppm are prepared by transferring appropriate amounts of a 10.0 ppm working solution of Fe2+ into separate 50-mL volumetric flasks, each of which contains 5 mL of thioglycolic acid, 2 mL of 20% w/v ammonium citrate, and 5 mL of 0.22 M NH3. After diluting to volume and mixing, the absorbances of the standards are measured. a)Use the data table below to prepare a calibration curve (absorbance versus concentration in ppm). Fit the data to straight line and find the equation for the straight line and the R2 value. (Hint: Think about what to do with the absorbance of the blank.)
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. 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 a) 1 b) 3 c) 0.5 d) 2 e) 5
The absorbance of a 0.1 M solution of a complex was 0.15 at max. What is the value of molar absorptivity for this complex? What is the geometry of this complex?
Titanium and vanadium form colored complexes when treated with hydrogen peroxide in 1 M sulfuric acid. The titanium complex has an absorption maximum at 415 nm, and the vanadium complex has an absorption maximum at 455 nm. A 1.00 × 10−3 M solution ofthe titanium complex exhibits absorbance of 0.816 at 415 nm and of 0.485 at 455 nm while a 2.00 × 10−3 M solution of the vanadium complex exhibits absorbances of 0.425 and 0.608 at 415 and 455 nm, respectively. A 1.000-g sample of an alloy containing titanium and vanadium was dissolved, treated with excess hydrogen peroxide, and diluted to a finalvolume of 1000 mL. The absorbance of the solution was 0.697 at 415 nm and 0.533 at 455nm. Calculate: a) The concentration of titanium and vanadium in the sample. b) The percentages of titanium and vanadium in the alloy.
You measured the absorbance values at selected wavelengths for one of the complexes above. Record those values below, as well as the identity of your chosen complex. Determine your estimate for the wavelength of maximum absorbance (λmax), and show your calculations for the energy of d-orbital splitting, Δ. 0.10 M Ni(NO)2 : 10 drops approximately 0.50 mL Chosen complex: (Ethylenediamine) C2H4(NH2)2 + Ni(NO)2 (10 drops, hot temperature, light purple color) Wavelength (λ) nanometers Absorbance 400 nm 0.438 450 nm 0.047 500 nm 0.094 550 nm 0.184 600 nm -0.043 650 nm -0.066 700 nm -0.0125 750 nm -0.121 800 nm -0.218
according to Werner, which valency is not ionisable in a complex compound, primary or secondary ?