2. For the first part of the lab, the following graph was produced. 0.6 Absorbance Curves for BCG basic forn bacidic form 0.5 0.4 0.3 0.2F 0.1 0.0 0.350 700 450 500 wavelength (nm) 400 550 600 650 max: Wavelength of maximum absorbance for base form a. The graph shows that the basic form has a maximum absorption at Amax, while the acidic has its minimum absorption at Amax. Explain why the basic form and acidic form have opposite absorptions at this specific wavelength. b. What is the importance of determining the Amax? Mixed (absorbance)

2. For the first part of the lab, the following graph was produced. 0.6 Absorbance Curves for BCG basic forn bacidic form 0.5 0.4 0.3 0.2F 0.1 0.0 0.350 700 450 500 wavelength (nm) 400 550 600 650 max: Wavelength of maximum absorbance for base form a. The graph shows that the basic form has a maximum absorption at Amax, while the acidic has its minimum absorption at Amax. Explain why the basic form and acidic form have opposite absorptions at this specific wavelength. b. What is the importance of determining the Amax? Mixed (absorbance)

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

A student makes a Beer's Law plot of A vs [Fe(SCN)2+] in the first part of the equilibrium constant lab, and gets the following information from the trendline. y = 50.7x R² = 0.9999 If the student measures a absorbance of 0.167 for a solution in the second part of the lab, what equilibrium concentration of [Fe(SCN)²+ would be reported?
2) In an experiment similar to ours, an FeSCN2+ standard curve was prepared (pictured below) and used to extrapolate the FeSCN²+ concentrations from three solutions of unknown [FeSCN²+] that were prepared at the same time. The standard curve was found to have a slope of 1950 M¹ and the three solutions of unknown [FeSCN²+] were found to have absorbances of 0.196, 0.281 and 0.365. Based on these data, what was the [FeSCN2+] in each solution? Absorbance at 460 nm [FeSCN²*] (M)
Calculate the initial concentrations for the Fe3+ and SCN- for the data provided in the table.
3. Using the graph provided, find the concentration of a solution that had an absorption of 0.269 when measured at 460 nm in a 1.0 cm cuvette. Absorbance vs. Concentration 0.45 0.4- y = 4.07x - 0.0046 R = 0.99353 0.35- %3D 0.3- 0.25 0.2- 0.15 - 0.1- 0.05 0.000 0.020 0.040 0.060 0.080 0.100 0.120 Concentration (mM) Absorbance at 460 nm
Consider the fictional transition metal 'Gc' and the complex ions formed with it: [GcI.], [Gc(NH;).]*+, and [Gc(C:O.).]>- If the A of max absorbance for one of the solutions is 450 nm, what are the possible colors for each of the solutions? (A) [GcI]³ could appear yellow, [Gc(NH;).]+ could appear purple, and [Gc(C,O.):]}- could appear blue. (B) [GcI.]- appears purple, [Gc(NH;).]+ could appear yellow, and [Gc(C.O.);]- could appear blue. (C) [GcI6]3- could appear purple, [Gc(NH3)6]3+ could appear yellow, and [Gc(C204)3]3- could appear orange. (D) [GcI6]3- could appear yellow, [Gc(NH3)6]3+ could appear purple, and [Gc(C204)3]3- could appear orange. (E) Not enough info
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
Examine the given Beer's law standard curve for an unknown dye measured in a 1.0 cm cuvette. Absorbance of Unknown Dye at 542 nm 0.5 0.45 0.4 0.35 0.3 0.25 0.2 y = 15200x - 0.018. 0.15 0.1 5.00E-06 1.00E-05 1.50E-05 2.00E-05 2,50E-05 3.00E-05 3.50E-05 Concentration (M) What is the molar absorptivity (in M-1cm-1) of the unknown dye at 542 nm? Type answer: 0.25 Incorrect Absorbance at 542 nm
Following AAS analysis, a graph of absorbance versus ppm nickel standard gave a best-fit line y = 0.0428x + 0.0487 . Calculate the ppm nickel in the well water sample having an absorbance of 0.675. 0.13 15.91 0.08 14.60
A student measures k for a certain blue dye to be 600.4 M-¹ at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.204 at this wavelength? Ens nousior #inslo: Monia sin 8 foi 00.01 Par det id elsem. sow & netimuloa 51 (5) sonos silf et trawIm 00 001 et gauzulib im
A series of standard iron-phenanthroline [Fe(phen)3]2+ complex ion solutions were prepared. The absorbance of each solution was measured at a wavelength of 510 mm. A calibration curve of absorbance vs. concentration was then plotted to obtain a linear equation of y = 0.0018x+0.0749. The absorbance of an unknown [Felphenly solution was measured to be 0.326. Calculate the concentration of the complex ion. NOTE! Report your answer as a WHOLE #. Type your answer...
A simultaneous determination of Co and Ni can be based on absorption by their respective 8-hydroxyquinolinol complexes. Molar absorptivities corresponding to their absorption maxima are as follows: 365 nm 700 nm 428.9 | 10.2 Co 3529 Ni 3228 Calculate the molar concentration of Ni and Co in the following solution measured using 1.00 cm cell. Absorbance: 365 nm: 0.426 700 nm: 0.026
Ligand X forms a complex with both cobalt and copper, each of which has a maximum absorbance at 510 nm and 645 nm. respectively. A 0.243 g sample containing cobalt and copper was dissolved and diluted to a volume of 100.0 mL. A solution containing ligand X was added to a 50.0 mL aliquot of the sample solution and diluted to a final volume of 100.0 mL. The measured absorbance of the unknown solution was 0.503 at 510 nm and 0.368 at 645 nm, when measured with a 1.00 cm cell. The molar absorptivities of the cobalt and copper complexes at each wavelength are shown in the table. Molar Absorptivity (c. M-'cm-¹) Wavelength [Co² = A, nm [Cu²+] = 510 645 3.125 x10-5 Incorrect Co 2.867 x10-5 3.7630 x 10² What is the concentration of cobalt and copper in the final diluted solution? 1282 Cu 5707 18090 M M