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´^cm-1 at åmax = 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 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´^cm-1 at åmax = 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.

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

If the absorbance for the solution was 0.432, calculate the equilibrium concentration of iron(III) thiocyanate in the solution. Report your answer in mM with three places after the decimal.
A student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate yes red purple calcium acetate forms lithium acetate lithium hydroxide No precipitate none colourless lithium permanganate none forms White precipitate yes red colourless forms No precipitate yes red colourless forms No precipitate forms yellow- yes colourless red
1. Sodium oxalate crystals (0.1234 g, MM=134) required 15.67 mL of KMNO, solution to titrate. Find the molarity of the titrant. 2 MnO4¯ + 5 C,0,² + 16 H* = 2 Mn²+ + 10 CO, + 8 H,O %3D
Consider the calibration data in the table below. Construct the equilibrium concentration of FeSCN2+ if the absorbance of an unknown solution is 0.460. [FeSCN2+] (M) Absorbance 0.250 x 10-4 0.120 0.500 x 10-4 0.240 1.00 x 10-4 0.481 1.60 x 10-4 0.770 1.00 x 10-4 M 8.00 x 10-5 M 9.58 x 10-5 M 9.54 10-5 M
Determination of the concentration of Zn(II) in a sample of river water was carried out by the standard addition method. A standard solution of 20 ppm Zn(II) was prepared and added to the filtered river water sample. The prepared series of solutions were then measured for absorbance with AAS and the results were as follows: 1. Fe(lII) 20 ppm (ml) Sample (ml) H2O (ml) A 0,0 1 0.111 0,2 1 8 0.167 0,4 7 0.223 0,6 1 6. 0.286 0,8 1 0.347 1,0 1 0.401 a. Draw a calibration curve for the volume of Zn(II) vs. absorbance and concentration Zn(II) vs. absorbance b. Based on the available data, what is the concentration of Zn(II) in the sample
Measurement of the concentration of Fe 3+ ions in a saturated solution of Iron(III) chloride was found to be 0.35 M. Calculate the Ksp of Iron(III) chloride.
If the absorbance for the solution was 0.698, calculate the equilibrium concentration of iron(III) thiocyanate in the solution. Report your answer in mM with three places after the decimal.
I need help calculating the following.
A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+
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?
For the aqueous [Hg14] complex K₁=6.76 × 10²⁹ at 25 °C. 2+ Suppose equal volumes of 0.0066M Hg(NO3), solution and 0.78M KI solution are mixed. Calculate the equilibrium molarity of aqueous Hg²+ ion. Round your answer to 2 significant digits. M x10 X ? Ś
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