Use the volume of Iron solution (which is 10.0mL) and the moles of Fe( which is 0.0007  moles) to find the concentration of the Fe in the unknown sample.

Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
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Question #6)

Use the volume of Iron solution (which is 10.0mL) and the moles of Fe( which is 0.0007  moles) to find the concentration of the Fe in the unknown sample. 

Titration #1
10,0mL
Volume of unknown iron (II) solution
0.0m L
odot
6.80m C
Initial buret reading of KMNO4 (aq)
Final buret reading of KMNO4 (aq)
%3D
Titration #2
10.0mL
Volume of unknown iron (II) solution
0.0mL
- 6.75mC
Initial buret reading of KMNO4 (aq)
Final buret reading of KMNO4 (aq)
Titration #3
alom or T
10.0mL
0.OmL
6.90mC
Volume of unknown iron (II) solution
Initial buret reading of KMNO4 (aq)
%3D
Final buret reading of KMNO4 (aq)
%3D
0.020M
Spotassium
51
Transcribed Image Text:Titration #1 10,0mL Volume of unknown iron (II) solution 0.0m L odot 6.80m C Initial buret reading of KMNO4 (aq) Final buret reading of KMNO4 (aq) %3D Titration #2 10.0mL Volume of unknown iron (II) solution 0.0mL - 6.75mC Initial buret reading of KMNO4 (aq) Final buret reading of KMNO4 (aq) Titration #3 alom or T 10.0mL 0.OmL 6.90mC Volume of unknown iron (II) solution Initial buret reading of KMNO4 (aq) %3D Final buret reading of KMNO4 (aq) %3D 0.020M Spotassium 51
Post-lab Questions (show all calculations):
1. Determine the oxidation number (state) of manganese in MnO4.
Xtq(-2)=-1
X = I/X=7
2. Complete the following half reactions by filling in the appropriate number of
electrons (as reactants or products) that are lost or gained in the redox
reaction. Identify each half reaction as being an oxidation or a reduction.
ox dation> SFE² (aq)
reduction-> MnO;(aq)
SFe*(aq) +Je
Mn²"(aq) = MnDy +Se-7 Mn2+
3. Average the volume of 0.020M KMN04 (aq) solution needed to reach the
equivalence point for the three runs.
fug volume of kMnO {6.82mc
(6 80t6.75+6.90)=2045mL
ud Inni
3.
4. Use the averaged volume of 0.020M KMNO4 (aq) solution to calculate the
number of moles of KMNO4 needed to reach the equivalenee point.
,0 Dx0.DO52 Oi moles Xi00
lo00 mL -Tt re
volme
6,82mL=o.0066a16
5. The mole ratio of potassium permanganate to iron (II) is 1 mol KMNO4 = 5
mol Fe2+ for this reaction. Using the number of moles of KMNO4 and the mole
ratio, calculate the number of moles of Fe2+.
moles=1.4x104
MO
5x14x104
0 000 Tmoles Fe9 t
6. Finally, using the volume of iron (II) selution and moles of Fe2*, eałculate the
concentration of the Fe2+ in the unknown sample.
52
Transcribed Image Text:Post-lab Questions (show all calculations): 1. Determine the oxidation number (state) of manganese in MnO4. Xtq(-2)=-1 X = I/X=7 2. Complete the following half reactions by filling in the appropriate number of electrons (as reactants or products) that are lost or gained in the redox reaction. Identify each half reaction as being an oxidation or a reduction. ox dation> SFE² (aq) reduction-> MnO;(aq) SFe*(aq) +Je Mn²"(aq) = MnDy +Se-7 Mn2+ 3. Average the volume of 0.020M KMN04 (aq) solution needed to reach the equivalence point for the three runs. fug volume of kMnO {6.82mc (6 80t6.75+6.90)=2045mL ud Inni 3. 4. Use the averaged volume of 0.020M KMNO4 (aq) solution to calculate the number of moles of KMNO4 needed to reach the equivalenee point. ,0 Dx0.DO52 Oi moles Xi00 lo00 mL -Tt re volme 6,82mL=o.0066a16 5. The mole ratio of potassium permanganate to iron (II) is 1 mol KMNO4 = 5 mol Fe2+ for this reaction. Using the number of moles of KMNO4 and the mole ratio, calculate the number of moles of Fe2+. moles=1.4x104 MO 5x14x104 0 000 Tmoles Fe9 t 6. Finally, using the volume of iron (II) selution and moles of Fe2*, eałculate the concentration of the Fe2+ in the unknown sample. 52
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