A student obtained a sample impure ASA sample. He hydrolyzedthe ASA with NaOH and heated the mixture to produce thesalicylate dianion:C6H4 (OCOCH3) (COOH) + 3OH- → C6H4 (0) (COO) + 2H₂O + CH3COONext the student then acidified the mixture with FeCl3-KCI-HCIsolution to produce the magenta complex oftetraaquosalicylatoiron (III) ion:C6H4 (0) (COO) + H3O+C6H4 (OH) (COO-) + H₂O3+C6H4 (OH) (COO) + Fe(H₂O) ³+ [C6H4 (O) (COO) Fe(H₂O)] ++ H₂O + H₂O* The complex ion is sensitive to pH, therefore the solution was buffered to pH 1.90 to avoidthe formation of di- and tri-salicylate complex of iron (III).Before the concentration could be determined through UV-Visspectroscopy, the student needs to know the wavelength of lightthat was most absorbed by the complex ion in order to set thespectrometer properly. The student calibrated the spectrometerby setting the transmittance to 100 % with FeCl3-KCI-HCI solutionas reference. The data is as follows:Wavelength(nm)580570560550540535530525520510500490Absorbance0.1190.1980.2030.2150.2200.2280.2400.2550.2470.2160.1990.073

A question based on absorption. A set of data obtained in UV-Visible spectroscopy is prescribed.…

C6H4 (OCOCH3) (COOH) + 3OH- → C6H4 (0) (COO) + 2 H₂O + CH3COO™ Next the student then acidified the mixture with FeCl3-KCI-HCI solution to produce the magenta complex of tetraaquosalicylatoiron (III) ion: C6H4 (0) (COO-) + H₂O + C6H4 (OH) (COO) + Fe (H₂O) 3+ C6H4 (OH) (COO) + H₂O [C6H4 (O) (COO) Fe(H₂O)6] + H₂O + H₂O* →

C6H4 (OCOCH3) (COOH) + 3OH- → C6H4 (0) (COO) + 2 H₂O + CH3COO™ Next the student then acidified the mixture with FeCl3-KCI-HCI solution to produce the magenta complex of tetraaquosalicylatoiron (III) ion: C6H4 (0) (COO-) + H₂O + C6H4 (OH) (COO) + Fe (H₂O) 3+ C6H4 (OH) (COO) + H₂O [C6H4 (O) (COO) Fe(H₂O)6] + H₂O + H₂O* →

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...

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Question

100%

A student obtained a sample impure ASA sample. He hydrolyzed
the ASA with NaOH and heated the mixture to produce the
salicylate dianion:
C6H4 (OCOCH3) (COOH) + 3OH- → C6H4 (0) (COO) + 2
H₂O + CH3COO
Next the student then acidified the mixture with FeCl3-KCI-HCI
solution to produce the magenta complex of
tetraaquosalicylatoiron (III) ion:
C6H4 (0) (COO) + H3O+
C6H4 (OH) (COO-) + H₂O
3+
C6H4 (OH) (COO) + Fe(H₂O) ³+ [C6H4 (O) (COO) Fe(H₂O)] ++ H₂O + H₂O*

The complex ion is sensitive to pH, therefore the solution was buffered to pH 1.90 to avoid
the formation of di- and tri-salicylate complex of iron (III).
Before the concentration could be determined through UV-Vis
spectroscopy, the student needs to know the wavelength of light
that was most absorbed by the complex ion in order to set the
spectrometer properly. The student calibrated the spectrometer
by setting the transmittance to 100 % with FeCl3-KCI-HCI solution
as reference. The data is as follows:
Wavelength
(nm)
580
570
560
550
540
535
530
525
520
510
500
490
Absorbance
0.119
0.198
0.203
0.215
0.220
0.228
0.240
0.255
0.247
0.216
0.199
0.073

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. 29) The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (a) TlCl: [Tl+] = 1.21 ×× 10–2 M, [Cl–] = 1.2 ×× 10–2 M (b) Ce(IO3)4: [Ce4+] = 1.8 ×× 10–4 M, [IO3−][IO3−] = 2.6 ×× 10–13 M (c) Gd2(SO4)3: [Gd3+] = 0.132 M, [SO42−][SO42−] = 0.198 M (d) Ag2SO4: [Ag+] = 2.40 ×× 10–2 M, [SO42−][SO42−] = 2.05 ×× 10–2 M (e) BaSO4: [Ba2+] = 0.500 M, [SO42−][SO42−] = 4.6 ×× 10−8 M
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