1. Determine the percentage of hydrogen peroxide in the solution sample. 2. naturally occurring manganese consists of only the Mn55 isotope. determine the moles of the manganese sulphate in the product solution, then calculate the totally number of neutrons present in all the manganese ions in the final solution.
1. Determine the percentage of hydrogen peroxide in the solution sample. 2. naturally occurring manganese consists of only the Mn55 isotope. determine the moles of the manganese sulphate in the product solution, then calculate the totally number of neutrons present in all the manganese ions in the final solution.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Determine the percentage of hydrogen peroxide in the solution sample.
2. naturally occurring manganese consists of only the Mn55 isotope. determine the moles of the manganese sulphate in the product solution, then calculate the totally number of neutrons present in all the manganese ions in the final solution.
Transcribed Image Text:1
Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It is
therefore necessary to periodically determine the purity of the peroxide solutions.
This can be done via a redox titration as follows:
The density of a particular surgięal grade hydrogen peroxide solution is 1.11g.cm3.
Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficient
amount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark.
A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a
0.372 M KMNO4 solution.
The endpoint of the titration is determined when the colourless solution in the conical flask turns a
persistent bright pink due to the presence of excess permanganate ions.
The average titration value is 26.20 mL of the KMNO4 solution.
The reaction stoichiometry is as follows:
2KMN04(aq) + 3H2SO4(aq) + 5H202 (aq)
2MNSO,(aq) + K2SO, (aq) + 8H20(8) + 502 (g)
4
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