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Lab: Analysis of Hydrogen Peroxide Solutions

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Fill a burette with 50 mL of 0.2M potassium permanganate solution. Add 10 mL of NEW hydrogen peroxide and 2 mL of 6M sulfuric acid to a flask. Titrate the hydrogen peroxide with the KMnO4 solution to the purple endpoint of excess MnO4- ion.

Questions:
(a) Volume of potassium permanganate used in each titration (mL):50mL
(b) The volume of potassium permanganate required to titrate 10 mL of the new hydrogen peroxide (mL):20mL
(c) Calculate the concentration of H2O2 from the volume of KMnO4 used and the stoichiometry of the reaction (MW of H2O2 is 34.01).

In these calculations I got lost.
-I found 0.12655 mol KMnO4. Is this the amount in mol of KMnO4 which reacted? So now how I get the concentration of the H2O2?
-2(C2x0.02L)KMnO4=5(34.01xV1)H2O2. What is C2 and V1?

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https://brainmass.com/chemistry/acid-and-base-organic-chemistry/lab-analysis-hydrogen-peroxide-solutions-399278

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Lab: Analysis of Hydrogen Peroxide Solutions
Fill a burette with 50 mL of 0.2M potassium permanganate solution. Add 10 mL of NEW hydrogen peroxide and 2 mL of 6M sulfuric acid to a flask. Titrate the hydrogen peroxide with the KMnO4 solution to the purple endpoint of excess MnO4- ion.

Questions:
(a) Volume of potassium permanganate used in each titration (mL):50mL
(b) The volume of potassium permanganate required to titrate ...

Solution Summary

An analysis of hydrogen peroxide solutions are examined.

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Analysis of Hydrogen Peroxide Solutions

Molarity of KMnO4: .2 M
Volume of H2O2: 10 mL

Titration of KMnO4 and new H2O2
Trial 1(Rough) Trial 2(Fine) Trial 3(Fine)
Initial volume 12.00mL 12.00mL 12.00mL
Final volume 13.98mL 12.10mL 12.05mL

Titration of KMnO4 and old H2O2 (Fine Titrations Only)
Trial 1(Rough) Trial 2(Fine) Trial 3(Fine)
Initial volume 12.00mL 12.00mL 12.00mL
Final volume 12.99mL 12.10mL 12.05mL

Calculations/Interpretations: Show all math performed (give the formula, show your setup, and give the result. Use proper significant figures and include proper labels. Also, answer ALL questions asked in the lab.

Trial 2 Trial 3 Average
Volume of KMnO4 (new H2O2):
Volume of KMnO4 (old H2O2):

Moles KMnO4 (new H2O2):
Moles KMnO4 (old H2O2):

Balanced equation:
2 KMnO4 + 5 H2O2 + 3 H2SO4  K2SO4 + 2 MnSO4 + 8H2O + 5 O2

Using the average values from trials 2 and 3 and the balanced equation, calculate the following:
Moles H2O2 (new):
Moles H2O2 (old):

Molarity H2O2 (new):
Molarity H2O2 (old):

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