A mixture is prepared by combining 10.72 mL of 2.52 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.76 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.25 x 10-4 M. Complete the following ICE table Fe3+ + SCN- ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I)

A mixture is prepared by combining 10.72 mL of 2.52 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.76 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.25 x 10-4 M. Complete the following ICE table Fe3+ + SCN- ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I)

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

Chapter9: Atomic Absorption And Atomic Fluorescence Spectrometry

Section: Chapter Questions

Problem 9.1QAP

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A mixture is prepared by combining 11.34 mL of 2.36 x 103 M Fe(NO3)3 with 10.00 mL of 1.66 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FESCN2*] at equilibrium is found to be 2.20 x 10-4 M. Complete the following ICE table Fe3+ SCN 1t FESCN2+ initial (M) (A) (B) (C)0 change (M) (D) (E) (F) equilibrium (M) (G) (H) (1) What is the value of K?
You did not allow enough time for the solution to reach equilibrium before measuring its absorbance. Explain how this will affect the reported value of Kc.
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?
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...
Calculate the equilibrium concentration of FeSCN^2 Please explain.
A student wants to determine the concentration of iron ion in a 15.000 gram solid that contains iron. The sample is crushed and 1.534 grams are dissolved into 100.0 mL of acid. A complexing agent is added to the solution to give it measurable color. The extinction coefficient, ɛ, for this iron species is 1.68 x 103 M-1cm-1 at Amax = 528 nm. If the final solution has an absorbance of A = 0.645 at 528 nm (using a 1.00 cm cuvette), what is the observed color of the solution and the mass of iron in the original 15.000 gram sample? O The solution is red and there are 0.210 grams of Fe in the 15.000 g solid. O The solution is red and there are 0.0210 grams of Fe in the 15.000 g solid. O The solution is green and there are 0.00214 grams of Fe in the 15.000 g solid. O The solution is green and there are 0.0210 grams of Fe in the 15.000 g solid. O The solution is red and there are 0.00214 grams of Fe in the 15.000 g solid.
A standard solution was put through appropriate dilu tions to give the concentrations of iron shown in the ac companying table. 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 (see color plate 15). The absorbances in the table (1.00-cm cells) were recorded at 510 nm Fe(II) Concentration in Original Solution, ppm Aşie 4.00 0.160 0.390 10.0 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580 (a) Plot a calibration curve from these data. (b) Use the method of least squares to find an equa tion relatin g absorbance and the concentration of iron(II). (c) Calculate the standard deviation of the slope and intercept.
The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4⁢x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?
1. A student collects the following data for the absorbance of a complex measured in 1.00 cm spectrophotometric cells. The molar absorptivity (ɛ) of the complex under investigation is 0.750 L/mol·cm. Calculate the concentration of the solution at each time of the reaction. Measured Complex Concentration Time (min) Absorbance (M) 0.000 1.500 10.000 1.313 20.000 1.125 30.000 0.938 40.000 0.750
The sodiuṁ salt of 2-quinizarinsulfonic acid (NaQ) forms a complex with Al3+ that absorbs strongly at 560 nm. From the data of the absorbance, find formula of the complex. In all solutions, [A3+]=3.7x105 M and the cell length is 1.00 cm. (Apply the molar-ratio method.) ca/M A(560) mol ratio [Al3+]/[Q] 1,00E-05 0,131 2,00E-05 0,265 3,00E-05 0,396 4,00E-05 0,468 5,00E-05 0,487 6,00E-05 0,498 8,00E-05 0,499 1,00E-04 0,5 OH NaQ
5- A 5.0 mL solution containing 3.36 pm Fe(Ill) ions is diluted to 50.0 mL by first treating with an excess of an appropriate amount of KSCN solution. The molar absorptivity of the FeSCN^2+ complex formed at 580 nm is given 7.0x10^3 L/cm.mol. Which of the following values is the absorbance of this solution as measured with a 2.0 cm cell? Fe:56 A. 0.168 B. 0042 C. 0,084 D. 0.126