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1. Fill a burette with the potassium permanganate solution of unknown concentration. 2. Into a 250-mL beaker, use a pipette to precisely add 10.00 mL of the 0.250 M Fe(NH4)2(SO4)2, ferrous ammonium sulfate (FAS) solution. 3. Next, use a graduated cylinder to add 5.0 ml of 3M H2SO4, sulfuric acid, and 3.0 mL of conc. H3PO4, phosphoric acid to the FAS solution. Titrate the FAS solution with the MnO4, permanganate, solution. (Very slowly and carefully add the permanganate to the FAS until a color change is observed. You must stop the addition at just the instance that the color change is observed otherwise you will have passed the stoichiometric endpoint and you will have an excess of permanganate.) 4. 0.00ML 5.33ML Initial volume of MnO4- in the burette Final volume of MnO4- in the burette Volume of MnO4- added

1. Fill a burette with the potassium permanganate solution of unknown concentration. 2. Into a 250-mL beaker, use a pipette to precisely add 10.00 mL of the 0.250 M Fe(NH4)2(SO4)2, ferrous ammonium sulfate (FAS) solution. 3. Next, use a graduated cylinder to add 5.0 ml of 3M H2SO4, sulfuric acid, and 3.0 mL of conc. H3PO4, phosphoric acid to the FAS solution. Titrate the FAS solution with the MnO4, permanganate, solution. (Very slowly and carefully add the permanganate to the FAS until a color change is observed. You must stop the addition at just the instance that the color change is observed otherwise you will have passed the stoichiometric endpoint and you will have an excess of permanganate.) 4. 0.00ML 5.33ML Initial volume of MnO4- in the burette Final volume of MnO4- in the burette Volume of MnO4- added

Chemistry
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
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 101AE: You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final...
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Find the volume of MnO4^1- added

1. Fill a burette with the potassium permanganate solution of unknown concentration. 2. Into a 250-mL beaker, use a pipette to precisely add 10.00 mL of the 0.250 M Fe(NH4)2(SO4)2, ferrous ammonium sulfate (FAS) solution. 3. Next, use a graduated cylinder to add 5.0 ml of 3M H2SO4, sulfuric acid, and 3.0 mL of conc. H3PO4, phosphoric acid to the FAS solution. Titrate the FAS solution with the MnO4, permanganate, solution. (Very slowly and carefully add the permanganate to the FAS until a color change is observed. You must stop the addition at just the instance that the color change is observed otherwise you will have passed the stoichiometric endpoint and you will have an excess of permanganate.) 4. 0.00ML 5.33ML Initial volume of MnO4- in the burette Final volume of MnO4- in the burette Volume of MnO4- added
Transcribed Image Text:1. Fill a burette with the potassium permanganate solution of unknown concentration. 2. Into a 250-mL beaker, use a pipette to precisely add 10.00 mL of the 0.250 M Fe(NH4)2(SO4)2, ferrous ammonium sulfate (FAS) solution. 3. Next, use a graduated cylinder to add 5.0 ml of 3M H2SO4, sulfuric acid, and 3.0 mL of conc. H3PO4, phosphoric acid to the FAS solution. Titrate the FAS solution with the MnO4, permanganate, solution. (Very slowly and carefully add the permanganate to the FAS until a color change is observed. You must stop the addition at just the instance that the color change is observed otherwise you will have passed the stoichiometric endpoint and you will have an excess of permanganate.) 4. 0.00ML 5.33ML Initial volume of MnO4- in the burette Final volume of MnO4- in the burette Volume of MnO4- added
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