The concentration of Fe2+ in a sample is determined by measuring the absorbance of its complex with ferroxine. The sample, measured in a 1.00 cm cuvette, has an absorbance of 0.254. The reagent blank in the same cuvette has an absorbance of 0.015. What would be the absorbance reading for each of these two solutions if measured in a 7.00 cm cuvette? A sample Areagent blank =

The concentration of Fe2+ in a sample is determined by measuring the absorbance of its complex with ferroxine. The sample, measured in a 1.00 cm cuvette, has an absorbance of 0.254. The reagent blank in the same cuvette has an absorbance of 0.015. What would be the absorbance reading for each of these two solutions if measured in a 7.00 cm cuvette? A sample Areagent blank =

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 4.14CYU

See similar textbooks

Similar questions

From experimental data, a plot of absorbance (in arbitrary units, a.u.) at a wavelength of 630 nm (on the y-axis) was plotted against the concentration (in mg/L) of Cu2+ (on the x-axis) in known solutions and a linear relationship was found with an equation of y = 7.22x+0.05. If an unknown solution had an absorbance of 1.20 a.u. at a wavelength of 630 nm, what is its concentration of Cu2+?
In an analytical laboratory a chemical compound namely Paracetamol (151.163 g/mol) is determined in a sample. A sample weighing 0.0295 g was dissolved in a solvent and diluted the solution to 1 L. The solution has λ max at 243 nm (ε=2.6×104 cm-1 mol-1 L). The solution exhibits an absorbance of 0.638 in a 2 cm cell. Calculate the percentage paracetamol in the sample.
The absorbance of 10 mL of 0.0005 M Co2+ solution is 0.35. 10 mL of this solution mixed with 10 mL of the sample solution produces an absorption of 0.52. Calculate the concentration of Co2+ in the sample
What is the concentration of copper ions in a solution within a cuvette that has an absorbance value of 0.697 and a molar absorbtivity of 6.833 x 103 L/mol cm? The pathlength of the cuvette is 1.00 cm.
What is the absorbance of a theoretical compound in a 5.26 x 10-5 M solution, a path length of 1.5 cm, and a molar absorptivity of 37.4 mol / L cm?
If a second brass washer of 0.6003 grams had been dissolved in nitric acid, diluted to 50.00 mL and then its absorbance measured at 0.450, what would be the concentration of Cu(NO3)2 in the solution? What would be the mass percent of copper in the second brass washer? Use equation of the line as y = 3.1295 x + 0.0055.
Absorbance measurements were taken on a series of Fe standards complexed with 1,10-phenanthroline. A plot of absorbance vs. concentration yielded a linear curve with the equation y=1.008e03x + 0.0395 (where y is the absorbance and x represents the Fe concentration in moles/L). Using this information calculate the Fe concentration (in ppm) in a 40.0-mL aliquot of ground water that produced an absorbance of 0.580.
Beryllium(II) forms a complex with acetylacetone (166.2 g/mol). Calculate the molar absorptivity of the complex, given that a 2.25 ppm solution has a transmittance of 37.5% when measured in a 1.00-cm cell at 295 nm, the wavelength of maximum absorption.
A solution of FeSCN2+ has an absorbance of 0.237. What is its concentration? 0.19 M 0.47 M 0.24 M 0.80 M 0.65 M
In the determination of iron in fortified cereals by atomic absorption, 0.9133 g of sample was weighed. After a previous treatment, it was dissolved and diluted to 100 mL, an aliquot of 25.0 mL was taken, this was diluted to 100 mL and this solution presented an absorbance reading of 0.251. A series of iron standards of the following concentrations were prepared: 0.0; 1.0; 2.0; 2.5 and 3.0 ppm. Whose absorbances were 0.0; 0.241; 0.405; 0.520 and 0.640. Determine the iron concentration in mg/100 g of sample.
If the solution #1 has an absorbance of 0.219 at equilibrium, calculate the [Fe(SCN)2+] in the solution using the line equation y=3189x-0.03392
A 20 ml aliquot of drinking water containing Fe(II) and Fe (III) is treated with hydroquinone to reduce all dissolved iron to Fe(II),0- phenanthroline is added and the aliquot is diluted to 50 ml and the absorbance in a 2.00 cm cell is 0.085 at 510 nm. Calculate the iron content of the water as ppm? ε = 1.11 x 104 L/mol cm