3: In the second part of the experiment, a solution containing 1.60x10-³ M Fe³+ and 4.00x10-4 M SCN was created, and the absorbance was recorded as 0.242 once the solution reached equilibrium. on, calculate the equilibrium concentration of FeNCS²+ present. 4: Using an ICE table, determine the equilibrium concentrations of Fe³+ and SCN in the previous question. Then, use the equilibrium concentrations of Fe³+, SCN", and FeNCS²+ to calculate Keq for the chemical reaction.

3: In the second part of the experiment, a solution containing 1.60x10-³ M Fe³+ and 4.00x10-4 M SCN was created, and the absorbance was recorded as 0.242 once the solution reached equilibrium. on, calculate the equilibrium concentration of FeNCS²+ present. 4: Using an ICE table, determine the equilibrium concentrations of Fe³+ and SCN in the previous question. Then, use the equilibrium concentrations of Fe³+, SCN", and FeNCS²+ to calculate Keq for the chemical reaction.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

See similar textbooks

Similar questions

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?
A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? The Fe concentration of the water sample is higher than 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. The Fe concentration of the water sample is lower than 100 ppm. The Fe concentration of the water sample is equal to 100 ppm.
The absorbance value for the Standard was 0.625 and [FeSCN^ 2+ ] std is 2.00E 4M Calculate the [FeSCN^ 2+ ] in the equilibrium mixture, report the answer to the correct significant figures. The absorbance of the equilibrium solution was 0.451
The absorbance of a solution containing 5.0 x 10^-3 g/L of a solute in a 1.00 m cell is 1.00. Calculate the absorptivity and the molar absorptivity if the molecular mass of the solute is 1.25.
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) What is the value of Kc?
Calculate the molar absorptivity of a solute when its measured absorbance is 1.050 with a concentration of 1.45 x 10-3 M. Assume the path length of the cell is 1.0 cm.
A student prepared a calibration curve by measuring of the absorbance of five standard solutions of a compound at 300 nm. A cuvette with a path length of 5 cm was used . if the slope of the curve was 300 L/mol. the molar absorptivity of the compound is…….. 60 L mol-1cm-1 1500 L mol-1cm-1 0.20 L mol-1cm-1 5.0 L mol-1cm-1
The nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm1. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL. It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NANO2 (69 g/mol) in the original sample
A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. 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. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580
Suppose that a solution has an absorbance of 0.226 at a wavelength of 450 nm. If the concentration of the solution is 24 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette.
Determine the concentration of [Fe(SCN)2+_std] if the standard solution was made using 18 mL of 0.2M Fe(NO3)3 and 2 mL of 0.002 M KSCN and has an absorbance of 0.921.
4. determine the amount in mg of the amount of Ag present from ICP mass digested: 1.0821g/L dilution of 10ml stock solution to 100ml volumetric flask X=0.98 (intensity)