Question

Aqueous solutions containing approximately 3 percent(w/w) H2O2 are sold in drug stores as a disinfectant. Determination of the actual concentration of H2O2 in a bottle of peroxide solution was done by diluting 1.50 mL to 100 mL with water, acidifying with dilute H2SO4 and titrating with a 0.01411 M KMnO4 solution. 32.17 mL of the permangate solution was needed to reach the end point of the titration. What is the actual molar concentration of the H2O2 solution]

Answer 1

The actual molar concentration of the H₂O₂ solution is calculated using titration data and stoichiometry, resulting in a concentration of 0.0756 M.

Step-by-step explanation:

To determine the actual molar concentration of the H₂O₂ solution, we can use the following stoichiometry steps based on the information given and the balanced chemical equation for the reaction between H₂O₂ and KMnO₄.

1. Calculate the moles of KMnO₄ used in the titration: moles = Molarity x Volume = 0.01411 M x 0.03217 L = 4.537 x 10-4 moles.
2. The balanced equation for the reaction is 2MnO₄- + 6H+ + 5H₂O₂ → 2Mn2++ 8H₂O + 5O₂, which means 5 moles of H₂O₂ react with 2 moles of KMnO₄.
3. Calculate the moles of H₂O₂: (5/2) x 4.537 x 10-4 moles = 1.134 x 10-3 moles
4. Calculate the molarity of the diluted solution: Moles / Volume = 1.134 x 10-3 moles / 0.1 L = 0.01134 M
5. Calculate the molarity of the original solution before dilution: Molarity after dilution x Dilution Factor = 0.01134 M x (100 mL / 1.5 mL) = 0.0756 M

The actual molar concentration of the H₂O₂ solution in the drugstore bottle is 0.0756 M.

Answer 2

0.01804 M KMnO4 Solution.

Step-by-step explanation:

3 Percent(w/w) H2O2 Are Sold In Drug Stores As A Disinfectant. ... H2O2 In A Bottle Of Peroxide Solution Was Done By Diluting 1.50 ML To 100 ML With Water, Acidifying With Dilute H2SO4 And Titrating With A 0.01804 M KMnO4 Solution.