**Experiment Details: Equilibrium Concentration Calculation**A solution in part C initially contains \(4.1000 \times 10^{-4}\) molar SCN\(^-\) and \(1.180 \times 10^{-1}\) molar Fe\(^{3+}\).This solution was then measured using the colorimeter, and an absorbance of \(5.150 \times 10^{-1}\) was recorded. The constant determined in part A of the experiment was found to be \(3.47 \times 10^{3}\).**Task:**Using the absorbance and constant provided, determine the equilibrium concentration of FeSCN\(^{2+}\), \([ \text{FeSCN}^{2+}]_E\).**Note:**Your answer is assumed to be reduced to the highest power possible.**Your Answer:**- Enter the answer in the format (number) × 10 (power).- Include appropriate units.[Input fields for the answer and units are provided in the image.]

Given that: absorbance = 5.150×10-1 initial concentration of Fe3+ = 1.180×10-1 M initial…

A solution in part C initially contains (4.1000x10^-4) molar SCN¯ and (1.180x10^-1) molar Fe3+. This solution was then measured using the colorimeter, and an absorbance of (5.150x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.47x10^3). Using the absorbance and constant provided, determine the equilibrium concentration of FESCN2+, [FESCN2+]e. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

A solution in part C initially contains (4.1000x10^-4) molar SCN¯ and (1.180x10^-1) molar Fe3+. This solution was then measured using the colorimeter, and an absorbance of (5.150x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.47x10^3). Using the absorbance and constant provided, determine the equilibrium concentration of FESCN2+, [FESCN2+]e. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

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

Suppose that a solution has an absorbance of 0.250 at a wavelength of 450 nm. If the concentration of the solution is 22 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette. molar absorptivity in (L cm^−1 mol^-1):
The absorbance of a 0.00105% m/v solution of tolbutamide in methanol when measured in a 1 cm path length cell was found to be 0.796 at 228 nm. Calculate the specific absorbance.
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
You wish to measure the iron content of the well water on the new property you are about to buy. You prepare a reference standard Fe3+ solution with a concentration of 7.22 × 10-4 M. You treat 11.0 mL of this reference with HNO, and excess KSCN to form a red complex and dilute the reference to 60.0 mL. The diluted reference is placed in a cell with a 1.00-cm light path. You then take 10.0 mL of the well water, treat with HNO, and excess KSCN, and dilute to 100.0 mL. This diluted sample is placed in a variable pathlength cell. The absorbance of the reference and the sample solutions match when the pathlength is 3.93 cm. What is the concentration of iron in the well water? For each solution, the zero is set with a blank. [Fe3+]well М Jwell water
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...
You want to determine the amount of iron(III) in acomplex salt. You make a 100.0 mL solution of the complex salt by dissolving 0.0670 g of complex salt with water to the mark on a 100.0 mL volumetric flask. You get an absorbance reading for the iron from the spectrometer of 0.334. The molar absorptivity is determined to be 17605 L/mole∙cm and the pathlength is 1.00 cm. Determine the molarity of iron(III) in solution. Determine the mass percentage of iron(III) in the complex salt.
If the absorbance for the solution was 0.342, calculate the equilibrium constant, Keq, with zero places after the decimal.
3. A solution is prepared by mixing 1.00 mmol of a weak acid (HA, pka =6.44) with an unknown amount of KOH. The solution is diluted to 1.00 L using deionized water. An aliquot of the solution is placed in a 1.00-cm cuvet. The absorbance of the solution at 285 nm is 0.7748. Using the measured absorbance value, calculate the concentrations of HA and A in the solution. Then calculate the pH of the solution. You may assume all activity coefficients are equal to unity. НА A- Molar absorptivity at 285 nm (M1 cm) 456 2050
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 sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.
15. Calculate the Kf of the [Fe(SCN)]2+ solution if 4 mL of 0.004M FENO3 is mixed with 6 mL of 0.004 M KSCN. The Absorbance is 0.400 and the equation of the calibration plot (Beer's Law) is y=7455.4x