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 #110,0mLVolume of unknown iron (II) solution0.0m Lodot6.80m CInitial buret reading of KMNO4 (aq)Final buret reading of KMNO4 (aq)%3DTitration #210.0mLVolume of unknown iron (II) solution0.0mL- 6.75mCInitial buret reading of KMNO4 (aq)Final buret reading of KMNO4 (aq)Titration #3alom or T10.0mL0.OmL6.90mCVolume of unknown iron (II) solutionInitial buret reading of KMNO4 (aq)%3DFinal buret reading of KMNO4 (aq)%3D0.020MSpotassium51 Post-lab Questions (show all calculations):1. Determine the oxidation number (state) of manganese in MnO4.Xtq(-2)=-1X = I/X=72. Complete the following half reactions by filling in the appropriate number ofelectrons (as reactants or products) that are lost or gained in the redoxreaction. Identify each half reaction as being an oxidation or a reduction.ox dation> SFE² (aq)reduction-> MnO;(aq)SFe*(aq) +JeMn²"(aq) = MnDy +Se-7 Mn2+3. Average the volume of 0.020M KMN04 (aq) solution needed to reach theequivalence point for the three runs.fug volume of kMnO {6.82mc(6 80t6.75+6.90)=2045mLud Inni3.4. Use the averaged volume of 0.020M KMNO4 (aq) solution to calculate thenumber of moles of KMNO4 needed to reach the equivalenee point.,0 Dx0.DO52 Oi moles Xi00lo00 mL -Tt revolme6,82mL=o.0066a165. The mole ratio of potassium permanganate to iron (II) is 1 mol KMNO4 = 5mol Fe2+ for this reaction. Using the number of moles of KMNO4 and the moleratio, calculate the number of moles of Fe2+.moles=1.4x104MO5x14x1040 000 Tmoles Fe9 t6. Finally, using the volume of iron (II) selution and moles of Fe2*, eałculate theconcentration of the Fe2+ in the unknown sample.52

The concentration of the solution can be expressed in many ways like Molarity, Normality, Molality,…

Answered: Use the volume of Iron solution (which…

Introduction to Chemical Engineering Thermodynamics

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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

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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

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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