Name:Date:Section:Data Report Sheet: Determination of Iron by Reaction with Permanganate: ATitrationUnknown #We 01 X ETrial ITrial IIIII [BLMass of Unknown0.512Initial Burette mL0.00 mLFinal Burette mL20.5mLmL0.2Total MnO, AddedMoles MnO, AddedMoles Fe?+ PresentGrams Fe²* PresentWeight % FeAverage Weight % Fe in Sample

Answered: Image /qna-images/answer/308c243f-e028-4728-81ef-58a28f6d6714.jpg

Answered: mL mL Moles MnO, Added Moles Fe?+…

Science

Chemistry

mL mL Moles MnO, Added Moles Fe?+ Present Grams Fe2* Present g Weight % Fe Average Weight % Fe in Sample

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

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.2QAP: A 0.4740-g pesticide sample was decomposed by wet ashing and then diluted to 200.0 mL in a...

See similar textbooks

Similar questions

For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 4. Why is it necessary to carry out the reduction of iron and then the titration, before going on to the next sample 5. If you look carefully, there are pieces of tin metal on the bottom of the SnCl2 reagent solution. Why is it there?
For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 1. What is the purpose of the phosphoric acid in this experiment? Please be specific. 2. How does the Diphenylamine sulfonate indicator work? What chemical reaction causes the color change? How is an indicator chosen in a redox reaction?
For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 3. How would you prepare a complete anlaysis procedure using KMnO4 as the oxidant instead of K2CrO7? Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular what is the purpose of the Zimmerman Reinhardt Reagent?
What is the oxidation state for KMnO4? Please show or explain calculation
A risk is a source of potential damageChemical safety is a condition of being safe from the occurrence of chemical incidentsEnthalpy is shown in TCE'sTorrefaction is the process used in making a charcoalA.) If all 4 statements are trueB.) If 3 of the 4 statements are trueC.) If 2 of the 4 statements are trueD.) If only 1 of the 4 statements is trueE.) If none of the 4 statements is true
A sample of impure KI weighing 0.600 g is dissolved in water, the solution acidified, and 25.00 mL of 0.0400 M KIO3 (an excess ) is added. The iodate is reduced to I2 and the iodide is oxidized to I, The I2 is boiled off, the solution cooled, and an excess of pure KI is added to react with the unused KIO3. The I2 produced is titrated with 40.38 mL of 0.1053 N thiosulfate. Write the equations for the reactions which occurred and calculate the percentage of KI in the sample.
A sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00mL of 6.00 N H2SO4 and 0.900 g of H2C2O4.2H2O. The excess oxalate then requires24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II)in 0.03058 g FeSO4.7H2O, what is the oxidizing power of the sample in terms of MnO2?84.33%
3. Determine the oxidationnumber for the indicated elementin each of the followingsubstances: (a) S in SO2 , (b) Cin COCl2 , (c) Mn in MnO4- ,(d)N in N2H4 , (e) N in HNO2 ,(f) Cr in Cr2O72-
(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000g is treated with 0.6000g of pure H2C2O4•2H2O and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+→ Mn2++ 2CO2 + 2H2O), the excess oxalic acid requires 26.26ml of 0.1000N KMnO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?
35.A sample of pyrolusite weighs 0.5000 g. To this is added 0.6674 g of As2O3 and dilute acid. After solvent action has ceased, the excess three-valent arsenic is titrated with 45.00 mL of 0.1000 N KMnO4. Calculate the oxidizing power of the pyrolusite in terms of percemtage MnO2. 36. A solution of Iodinebia such concentration that 20.0 mL are required to titrate the antimony in a 0.100 g sample containing 84.93% Sb2S3(339.7 g/mol). What is the value of 1.00 mL of this Iodine in terms of grams sulfue in tiration?
You are tasked with creating a pourboix diagram of selenium speciation. The relevent reactions are H2SeO3 <-> HSeO3- , HSeO3- <-> SeO32-, SeO42- <-> H2SeO3, SeO42- <-> HSeO3-, and SeO42- <-> SeO32-. Set and balence the redox reactions needed for this question and explain how you landed on those reactions.
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.