322 II. Calculations Show all of your work, where indicated, including any formulas, units, etc. Pay atten- tion to significant figures. A. Standardization of KMnO4 1. Using the two half-reactions in the introduction, balance the overall reaction which occurs between permanganate ion and iron(II). Show your method. Balanced eqn: 2. From your balanced equation, how many moles of iron(II) react per mole of MnO4? (This factor from the equation will be used in further calculations.) moles Fe2+/moles KMnO4 = 3. Calculation of the molarity of KMnO4. Show sample calculation-Trial 1. a. Moles ferrous ammonium sulfate in sample 1. b. Moles KMnO, required to react with Fe2+ in sample 1. C. Molarity of KMnO4 based on Trial 1. d. Results: Molarity KMnO4 Deviation Trial 1 Trial 2 Trial 3 Average
322 II. Calculations Show all of your work, where indicated, including any formulas, units, etc. Pay atten- tion to significant figures. A. Standardization of KMnO4 1. Using the two half-reactions in the introduction, balance the overall reaction which occurs between permanganate ion and iron(II). Show your method. Balanced eqn: 2. From your balanced equation, how many moles of iron(II) react per mole of MnO4? (This factor from the equation will be used in further calculations.) moles Fe2+/moles KMnO4 = 3. Calculation of the molarity of KMnO4. Show sample calculation-Trial 1. a. Moles ferrous ammonium sulfate in sample 1. b. Moles KMnO, required to react with Fe2+ in sample 1. C. Molarity of KMnO4 based on Trial 1. d. Results: Molarity KMnO4 Deviation Trial 1 Trial 2 Trial 3 Average
Chapter2: Basic Statistical Analysis With Excel
Section: Chapter Questions
Problem 12P
Related questions
Question
![I. Data
Record data with units.
A. Standardization of KMnO4
1. Mass of beaker/paper + ferrous ammonium sulfate
Empty Beaker
Beaker and Sample
Sample 1
7.40709
8. 4800g
Sample 2
7.4364g
9.19498
Sample 3
7.46.324
8.48993
2. Buret readings
Initial Reading
Final Reading
Sample 1
0.00mL
27.00m L
Sample 2
21.6 mL
29.5mL
Sample 3
33.5mL
29.3mL
Mass of Sample
1.0439
0.45269
1.0259
Volume KMnO
27.00mL
27.40 mL
25.8ML](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F739452bb-bec9-43d8-9372-35dc57efa9d5%2F661806a5-7f6e-4e74-8a92-91a092c39c21%2Fcuh0sas_processed.jpeg&w=3840&q=75)
Transcribed Image Text:I. Data
Record data with units.
A. Standardization of KMnO4
1. Mass of beaker/paper + ferrous ammonium sulfate
Empty Beaker
Beaker and Sample
Sample 1
7.40709
8. 4800g
Sample 2
7.4364g
9.19498
Sample 3
7.46.324
8.48993
2. Buret readings
Initial Reading
Final Reading
Sample 1
0.00mL
27.00m L
Sample 2
21.6 mL
29.5mL
Sample 3
33.5mL
29.3mL
Mass of Sample
1.0439
0.45269
1.0259
Volume KMnO
27.00mL
27.40 mL
25.8ML
![322
II. Calculations
Show all of your work, where indicated, including any formulas, units, etc. Pay atten-
tion to significant figures.
A. Standardization of KMnO4
1. Using the two half-reactions in the introduction, balance the overall reaction
which occurs between permanganate ion and iron(II). Show your method.
Balanced eqn:
2. From your balanced equation, how many moles of iron(II) react per mole of
MnO4? (This factor from the equation will be used in further calculations.)
moles Fe2+/moles KMnO4 =
3. Calculation of the molarity of KMnO4. Show sample calculation-Trial 1.
a. Moles ferrous ammonium sulfate in sample 1.
b. Moles KMnO, required to react with Fe2+ in sample 1.
c. Molarity of KMnO4 based on Trial 1.
d. Results:
Molarity KMnO4
Deviation
Trial 1
Trial 2
Trial 3
Average](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F739452bb-bec9-43d8-9372-35dc57efa9d5%2F661806a5-7f6e-4e74-8a92-91a092c39c21%2Fqqri876k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:322
II. Calculations
Show all of your work, where indicated, including any formulas, units, etc. Pay atten-
tion to significant figures.
A. Standardization of KMnO4
1. Using the two half-reactions in the introduction, balance the overall reaction
which occurs between permanganate ion and iron(II). Show your method.
Balanced eqn:
2. From your balanced equation, how many moles of iron(II) react per mole of
MnO4? (This factor from the equation will be used in further calculations.)
moles Fe2+/moles KMnO4 =
3. Calculation of the molarity of KMnO4. Show sample calculation-Trial 1.
a. Moles ferrous ammonium sulfate in sample 1.
b. Moles KMnO, required to react with Fe2+ in sample 1.
c. Molarity of KMnO4 based on Trial 1.
d. Results:
Molarity KMnO4
Deviation
Trial 1
Trial 2
Trial 3
Average
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