A 110.0-mL sample of spring water was treated to convert any iron present to Fet. Addition of 25.00-mL of 0.002525 M K2C1207 resulted in the reaction6Fe?+ + Cr2 O7²- + 14H+ → 6Fe+ + 2Cr³+ + 7H2OThe excess K2C12 07 was back-titrated with 8.05 mL of 0.00951 M Fe-t solution. Calculate the concentration of iron in the sample in parts per million.Concentration of ironppm

A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.002525 M K2 Cr2 O, resulted in the reaction 6Fe?+ + Cr2O,²- + 14H+ → 6Fe³+ + 2Cr³+ + 7H2O The excess K2Cr2O7 was back-titrated with 8.05 mL of 0.00951 M Fe²+ solution. Calculate the concentration of iron in the sample in parts per million. Concentration of iron= ppm

A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.002525 M K2 Cr2 O, resulted in the reaction 6Fe?+ + Cr2O,²- + 14H+ → 6Fe³+ + 2Cr³+ + 7H2O The excess K2Cr2O7 was back-titrated with 8.05 mL of 0.00951 M Fe²+ solution. Calculate the concentration of iron in the sample in parts per million. Concentration of iron= ppm

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

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.9QAP

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A 100.0 mL sample of spring water was treated to convert any iron Fe2+. Addition of 25.00 mL of 0.002017 M K2Cr2O7, resulted in the oxidation of Fe2+. The excess K2Cr2O7 was back-titrated with 7.47 mL of a 0.00797 M Fe2+ solution. Calculate the parts per million of iron in the sample.
A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid. The Fe3+ is reduced with SnCl2, HgCl2 is added, and the Fe2+ titrated with 0.1667 M K2Cr2O7 solution, requiring 12.96 mL. What was the formula of the original oxide?
A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+.Titration with 35.00-mLof 0.002345 M K2Cr2O7 resulted in the reaction6Fe2+ + Cr2O72- + 14H+  6Fe3+ 1 2Cr3+ + 7H2OThe excess K2Cr2O7 was back-titrated with 8.32 mL of 0.00897 M Fe2+ solution.Calculate the concentration of iron in the sample in parts per million.
A sample of iron ore weighing 0.6248 g is dissolved in acid, the iron reduced to Fe²⁺, and the solution titrated with 33.60 mL of a 0.1502 N solution of K₂Cr₂O₇. (Fe²⁺ ⟶ Fe³⁺; Cr₂O₇²⁻ ⟶ 2 Cr³⁺). a) Calculate the percentage of iron, Fe (FW 55.847) in the sample. b) Express the percentage as Fe₂O₃ (FW 159.69).
1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution.
1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
A 350 mg sample containing KClO3 was carefully reduced and treated with excess AgNO3. The resulting AgCl (MW = 143 g/mole) weighed 185 mg. Calculate the percentage of KClO3 (MW = 122 g/mole) in the sample
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.
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. Calculate the iron content of the ore as%w/w Fe2O3
A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?
A 1.000 g sample containing chlorides, iodides and inert materials was treated with dilute nitric acid followed by AgNO3. A precipitate of AgCl (143.32) and AgI (234.77) was produced and weighs 0.9238 g. On heating in a current of Cl2, the AgI is converted to AgCl, and the resulting product weighs 0.7238 g. Find the percentage of a) NaI (149.89) and b) NaCl (58.44) in the sample