Hydrogen peroxide solutions can casily 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 surgical grade hydrogen peroxide solution is 1.11g.cm". • 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. • 25.00 ml portion of this diluted solution is pipetted into a conical flask, and titrated with a 0.372 M KMNO, 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 KMNO, solution. The reaction stoichiometry is as follows: 2KMN0, (aq) + 3H,so,(aq) + 5H,0, (aq) - 2MNSO, (aq) + K,s0, (aq) + 8H,0(f) + 50, (B) 1.1 Determine the percentage of the hydrogen peroxide in the solution sample. 1.2 Naturally occurring manganese consists of only the "Mn isotope. Determine the moles of the manganese sulphate in the product solution, and then calculate the total number of neutrons present in all the manganese ions in the final solution.
Hydrogen peroxide solutions can casily 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 surgical grade hydrogen peroxide solution is 1.11g.cm". • 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. • 25.00 ml portion of this diluted solution is pipetted into a conical flask, and titrated with a 0.372 M KMNO, 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 KMNO, solution. The reaction stoichiometry is as follows: 2KMN0, (aq) + 3H,so,(aq) + 5H,0, (aq) - 2MNSO, (aq) + K,s0, (aq) + 8H,0(f) + 50, (B) 1.1 Determine the percentage of the hydrogen peroxide in the solution sample. 1.2 Naturally occurring manganese consists of only the "Mn isotope. Determine the moles of the manganese sulphate in the product solution, and then calculate the total number of neutrons present in all the manganese ions in the final solution.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 98AP
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Transcribed Image Text: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 surgical grade hydrogen peroxide solution is 1.1lg.cm.
• 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 KMNO, 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 KMNO, solution.
The reaction stoichiometry is as follows:
2KMN0, (aq) + 3H, so,(aq) + 5H,0, (aq)
2MnSo, (aq) + K2So, (aq) + 8H,0(f) + 50, (g)
1.1 Determine the percentage of the hydrogen peroxide in the solution sample.
1.2 Naturally occuring manganese consists of only the $"Mn isotope. Determine the moles of the manganese
sulphate in the product solution, and then calculate the total number of neutrons present in all the
manganese ions in the final solution.
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