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DETERMINATION OF HYDROGEN PEROXIDE BY REDOX TITRATION 1. Write the balanced net ionic equation for the reaction that takes place between hydrogen peroxide and permanganate ion in acidic solution. Oxidation: H₂O₂(aq) → O₂(g) Reduction: MnO4 (aq) overall: → Mn³* (aq)

DETERMINATION OF HYDROGEN PEROXIDE BY REDOX TITRATION 1. Write the balanced net ionic equation for the reaction that takes place between hydrogen peroxide and permanganate ion in acidic solution. Oxidation: H₂O₂(aq) → O₂(g) Reduction: MnO4 (aq) overall: → Mn³* (aq)

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
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Hi can you help me with problem1 on the prelab?

= Chemistry 1A Lab Manual (1).pdf Chabot College PRELAB 64 / 134 100% + A Reduction: MnO4 (aq) overall: Press F11 to exit full screen Name DETERMINATION OF HYDROGEN PEROXIDE BY REDOX TITRATION 1. Write the balanced net ionic equation for the reaction that takes place between hydrogen peroxide and permanganate ion in acidic solution. → O₂(g) Oxidation: H,Oz(aq) Chemistry 1A → Mn²+ (aq) 2. If 10.00 mL of a certain H₂O₂ solution requires 22.55 mL of 0.01533 M KMnO4 for titration, what is the molarity of the H₂O₂ solution? 3. If 1.39 g of KMnO4(s) is dissolved in water to make 500.0 mL of solution, what is the molar concentration of the permanganate ion, MnO4, in this solution? 4. In this experiment 10.00 mL of the unknown solution to be analyzed is diluted to 100.0 mL, and then 10.00 mL of that solution is titrated with the permanganate solution. Why not skip all this dilution business, and just pipet out 1.00 mL of the original unknown solution and titrate it directly? Assume the uncertainty in each pipet reading is ±0.02 mL. Hint: What are the relative uncertainties (in %) of 1.00 mL and 10.00 mL as measured by a pipet? ↓ |
Transcribed Image Text:= Chemistry 1A Lab Manual (1).pdf Chabot College PRELAB 64 / 134 100% + A Reduction: MnO4 (aq) overall: Press F11 to exit full screen Name DETERMINATION OF HYDROGEN PEROXIDE BY REDOX TITRATION 1. Write the balanced net ionic equation for the reaction that takes place between hydrogen peroxide and permanganate ion in acidic solution. → O₂(g) Oxidation: H,Oz(aq) Chemistry 1A → Mn²+ (aq) 2. If 10.00 mL of a certain H₂O₂ solution requires 22.55 mL of 0.01533 M KMnO4 for titration, what is the molarity of the H₂O₂ solution? 3. If 1.39 g of KMnO4(s) is dissolved in water to make 500.0 mL of solution, what is the molar concentration of the permanganate ion, MnO4, in this solution? 4. In this experiment 10.00 mL of the unknown solution to be analyzed is diluted to 100.0 mL, and then 10.00 mL of that solution is titrated with the permanganate solution. Why not skip all this dilution business, and just pipet out 1.00 mL of the original unknown solution and titrate it directly? Assume the uncertainty in each pipet reading is ±0.02 mL. Hint: What are the relative uncertainties (in %) of 1.00 mL and 10.00 mL as measured by a pipet? ↓ |
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