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: StandardizationMass of hydratedFe(NH4)2(SO4)2Initial buret readingFinal buret readingVolume of KMnO4 usedMolarity of KMnO4Average MolarityPart Two: AnalysisMass of unknownInitial buret readingFinal buret readingVolume of KMnO4 usedMass of Fe in unknownPercent Fe in unknownAverage % iron (Fe)Trial 11.00030.0125.4325.42M1. 00070.0014.0114.018 1.0005Trial 2mL 0.00mLML 25.46mLmL 25.46 mL 25.36MM8 1.0008g%%8 1₁00030.0125.37.Standard deviationmLmL 14.23 mLmL 14.21 _mL.Trial 30.02 mLg 1.0007 gmL13.99 mL13.98 mLmL 0.01g__%8mLmLmLM% wtre cmpd / MWFe cmpd=5 × MMO- × V₁MnO4™When completing the data sheet, along with sample (example) calculationson the back, bear in mind the following two items.1. Using equation [2-2], and given the molecular weight (MW, or molarmass) of hydrated ferrous ammonium sulfate as 392.14 g/mol,[2-2]calculate the molarity of the potassium permanganate solution for eachtrial completed, as well as the average molarity.Also, calculate the standard deviation. This is a measure of theprecision of your results, or how close they are to each other.2. Calculate the weight of iron in each of the samples titrated, using theatomic weight of 55.85 g/mol for iron (in place of the MW of thesulfate).

Given: Titration of unknown Fe sample with KMnO4To calculate: 1. Molarity of KMnO4 2. Amount of Fe…

Answered: Use the attached pictures to help fill…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

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Problem 41PS

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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
%

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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