Experiment 12:Oxidation-Reduction Reactions19al delPotassium permanganate (KMNO4) is a very powerful oxidizing agent. It is often used in analyses foriron(II) salts because it quantitatively and rapidly oxidizes Fe* to Fe*. Write and balance the oxidation-reduction equation for the reaction of the permanganate ion (MnO4) with Fe in acidic aqueous solution,producing Mn" ion and Fe" ion. (Hint: "Acidic aqueous solution," implies that water and hydrogen ionsMoube-roitsbixt2+2+2+3+must be present, so may appear in your equation.)4.

We are given a solution of Fe2+. KMnO4 is added to the solution which oxidizes to Fe3+ and MnO4- is…

Answered: Potassium permanganate (KMNO4) is a…

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.21PAE

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Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
Hittorf cells with silver-silver chloride electrodes were filled with HCl solution with a molality of 0.0106 mol / kg. 2 mA strong current flowed into the cell for 3 hours. At the end of the experiment, the solution at the cathode contained 51.7169 g water and 0.0267 g HCl. Find the transport numbers H + and Cl-
Prepare a complete analysis procedure using KMnO4 as teh oxidant instead of K2CrO7 in the redox analysis of iron. Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular, what is the purpose of the Zimmermann-Reinhardt reagent?
1. How to verify the applicability of the acid sulfate solution in plating the different metals commonly used in. 2. Compare the mass change on the electrodes during electrolysis of an aqueous CuSO4 solution.
A cell was prepared by dipping a Cu wire and a saturated calomel electrode into 0.10 M CUSO4 solution. The Cu wire was attached to the positive terminal of a potentiometer and the calomel electrode was attached to the negative terminal. (a) Write a half-reaction for the Cu electrode. (b) Write the Nernst equation for the Cu electrode. (c) Calculate the cell voltage.
A solution of silver nitrate containing 0.0074 g AgNO3 per gram of water and silver electrodes were used to determine transference numbers. After the experiment, 25 g of the anode solution contained 0.2553 g AgNO3. A silver coulometer connected in series with the cell produced 0.0785 g of silver during the experiment. Calculate the transference number of the Ag+ and NO3- ions?[0.42, 0.58] The answers are written in the bracket. I would like to know how it is obtained. Thank you!
One method for determining whether an individual has recently fired a gun is to look for traces of antimony in the residue collected from the individual’s hands. Anodic stripping voltammetry at a mercury film electrode is ideally suited for this analysis. In a typical analysis a sample is collected from a suspect with a cotton-tipped swab wetted with 5% v/v HNO3. After returning to thelab, the swab is placed in a vial containing 5.0 mL of 4 M HCl that is 0.02 Min hydrazine sulfate. After allowing the swab to soak overnight, a 4.0-mL portion of the solution is transferred to an electrochemical cell along with 100 mL of 0.01 M HgCl2. After depositing the thin film of mercury and the antimony, the stripping step gives a peak current of 0.38 μA. After adding a standard addition of 100 μL of 5.00×102 ppb Sb, the peak current increases to 1.14 μA. How many nanograms of Sb were collected from the suspect’s
Show detailed solution. A cell was prepared by dipping a Cu wire and a saturated calomel electrode into 0.10 M CuSO4 solution. The Cu wire was attached to the positive terminal of a potentiometer and the calomel electrode was attached to the negative terminal.(a) Write a half-reaction for the Cu electrode.(b) Write the Nernst equation for the Cu electrode.(c) Calculate the cell voltage.
Explain why strong oxidizing agents interfere with this analysis and why an excess of hydroxylamine prevents such interferences from occurring?
Which is not true for electrogravimetric analysis? A. If the analyte has color in solution; The disappearance of the color indicates that the build-up is complete. B. If a qualitative test for a small sample of the analyte solution is positive, the analyte deposition is complete. C. The analyte is quantitatively deposited on an electrode by electrolysis. D. If the additional electrode surface is exposed to the solution and there is no further deposition, the deposition of the analyte is complete.
One method for determining whether an individual recently fired a gun is to look for traces of antimony in residue collected from the individual’s hands. Anodic stripping voltammetry at a mercury film electrode is ideally suited for this analysis. In a typical analysis a sample is collected from a suspect using a cotton-tipped swab wetted with 5% v/v HNO3. After returning to the lab, the swab is placed in a vial that contains 5.0 mL of 4 M HCl that is 0.02 M in hydrazine sulfate. After soaking the swab, a 4.0-mL portion of the solution is transferred to an electrochemical cell along with 100 μL of 0.01 M HgCl2. After depositing the thin film of mercury and the antimony, the stripping step gives a peak current of 0.38 μA. After adding a standard addition of 100 μL of 00×102 ppb Sb, the peak current increases to 1.14 μA. How many nanograms of Sb were collected from the suspect’s hand?
In order to draw Pourbaix Diagram for a metal, all possible electrochemical and chemical reactions have to be known and with the application of Nernst equation or solubility product constant, the E-pH diagram can be constructed. We have looked at the diagram for Fe. While the Pourbaix diagram of Fe is quite complex due to its two oxidation states +2 and +3, construct a simplified Pourbaix diagram for Fe considering only the following three reactions. Note: CFe+2 and CFe+3 can be taken as 10-6 M Fe ----- Fe+2 + 2e- 2Fe+2 + 3H2O ----- Fe2O3 + 6H+ + 2e- 2Fe+3 + 3H2O ----- Fe2O3 + 6H+

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