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Use the attached pictures to help fill in the rest of the data. Please note that I used 0.79g of KMnO4 to prepare 250ml of 0.02M solution to titrate the ferrous ammonium sulfate. The approximate 1g of ferrous ammonium sulfate contained 25ml of distilled water and 10ml of 1M H2SO4 : H3PO4 to help dissolve the mixture for part one. For part two, the same steps were used however, we are to determin the amount of Fe in the sample. Please show and explain your work for each trail. Thank you!

Use the attached pictures to help fill in the rest of the data. Please note that I used 0.79g of KMnO4 to prepare 250ml of 0.02M solution to titrate the ferrous ammonium sulfate. The approximate 1g of ferrous ammonium sulfate contained 25ml of distilled water and 10ml of 1M H2SO4 : H3PO4 to help dissolve the mixture for part one. For part two, the same steps were used however, we are to determin the amount of Fe in the sample. Please show and explain your work for each trail. Thank you!

EBK A SMALL SCALE APPROACH TO ORGANIC L
EBK A SMALL SCALE APPROACH TO ORGANIC L
4th Edition
ISBN:9781305446021
Author:Lampman
Publisher:Lampman
Chapter13: Isolation Of Eugenol From Clov
Section: Chapter Questions
Problem 9Q
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Use the attached pictures to help fill in the rest of the data. Please note that I used 0.79g of KMnO4 to prepare 250ml of 0.02M solution to titrate the ferrous ammonium sulfate. The approximate 1g of ferrous ammonium sulfate contained 25ml of distilled water and 10ml of 1M H2SO4 : H3PO4 to help dissolve the mixture for part one. For part two, the same steps were used however, we are to determin the amount of Fe in the sample. Please show and explain your work for each trail. Thank you!

Part One: Standardization Mass of hydrated Fe(NH4)2(SO4)2 Initial buret reading Final buret reading Volume of KMnO4 used Molarity of KMnO4 Average Molarity Part Two: Analysis Mass of unknown Initial buret reading Final buret reading Volume of KMnO4 used Mass of Fe in unknown Percent Fe in unknown Average % iron (Fe) Trial 1 1.0003 0.01 25.43 25.42 M 1. 0007 0.00 14.01 14.01 8 1.0005 Trial 2 mL 0.00 mL ML 25.46 mL mL 25.46 mL 25.36 M M 8 1.0008 g % % 8 1₁0003 0.01 25.37. Standard deviation mL mL 14.23 mL mL 14.21 _mL. Trial 3 0.02 mL g 1.0007 g mL 13.99 mL 13.98 mL mL 0.01 g __% 8 mL mL mL M %
Transcribed Image Text:Part One: Standardization Mass of hydrated Fe(NH4)2(SO4)2 Initial buret reading Final buret reading Volume of KMnO4 used Molarity of KMnO4 Average Molarity Part Two: Analysis Mass of unknown Initial buret reading Final buret reading Volume of KMnO4 used Mass of Fe in unknown Percent Fe in unknown Average % iron (Fe) Trial 1 1.0003 0.01 25.43 25.42 M 1. 0007 0.00 14.01 14.01 8 1.0005 Trial 2 mL 0.00 mL ML 25.46 mL mL 25.46 mL 25.36 M M 8 1.0008 g % % 8 1₁0003 0.01 25.37. Standard deviation mL mL 14.23 mL mL 14.21 _mL. Trial 3 0.02 mL g 1.0007 g mL 13.99 mL 13.98 mL mL 0.01 g __% 8 mL mL mL M %
wtre cmpd / MW Fe cmpd = 5 × MMO- × V₁ MnO4™ When completing the data sheet, along with sample (example) calculations on the back, bear in mind the following two items. 1. Using equation [2-2], and given the molecular weight (MW, or molar mass) of hydrated ferrous ammonium sulfate as 392.14 g/mol, [2-2] calculate the molarity of the potassium permanganate solution for each trial completed, as well as the average molarity. Also, calculate the standard deviation. This is a measure of the precision of your results, or how close they are to each other. 2. Calculate the weight of iron in each of the samples titrated, using the atomic weight of 55.85 g/mol for iron (in place of the MW of the sulfate).
Transcribed Image Text:wtre cmpd / MW Fe cmpd = 5 × MMO- × V₁ MnO4™ When completing the data sheet, along with sample (example) calculations on the back, bear in mind the following two items. 1. Using equation [2-2], and given the molecular weight (MW, or molar mass) of hydrated ferrous ammonium sulfate as 392.14 g/mol, [2-2] calculate the molarity of the potassium permanganate solution for each trial completed, as well as the average molarity. Also, calculate the standard deviation. This is a measure of the precision of your results, or how close they are to each other. 2. Calculate the weight of iron in each of the samples titrated, using the atomic weight of 55.85 g/mol for iron (in place of the MW of the sulfate).
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