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
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...
Related questions
Question
Hi can you help me with problem1 on the prelab?
![Chabot College
Chemistry 1A
**PRELAB**
**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:
Oxidation: \[ \text{H}_2\text{O}_2(\text{aq}) \rightarrow \text{O}_2(\text{g}) \]
Reduction: \[ \text{MnO}_4^-(\text{aq}) \rightarrow \text{Mn}^{2+}(\text{aq}) \]
Overall:
2. If 10.00 mL of a certain \[\text{H}_2\text{O}_2\] solution requires 22.55 mL of 0.01533 M \[\text{KMnO}_4\] for titration, what is the molarity of the \[\text{H}_2\text{O}_2\] solution?
3. If 1.39 g of \[\text{KMnO}_4(\text{s})\] is dissolved in water to make 500.0 mL of solution, what is the molar concentration of the permanganate ion, \[\text{MnO}_4^-\], 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?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5222c9e-84ca-49ca-a26b-1a6cb57ce931%2F2dd968cc-f0fd-4ede-8dee-04b75c17d551%2Fjs5jlq_processed.png&w=3840&q=75)
Transcribed Image Text:Chabot College
Chemistry 1A
**PRELAB**
**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:
Oxidation: \[ \text{H}_2\text{O}_2(\text{aq}) \rightarrow \text{O}_2(\text{g}) \]
Reduction: \[ \text{MnO}_4^-(\text{aq}) \rightarrow \text{Mn}^{2+}(\text{aq}) \]
Overall:
2. If 10.00 mL of a certain \[\text{H}_2\text{O}_2\] solution requires 22.55 mL of 0.01533 M \[\text{KMnO}_4\] for titration, what is the molarity of the \[\text{H}_2\text{O}_2\] solution?
3. If 1.39 g of \[\text{KMnO}_4(\text{s})\] is dissolved in water to make 500.0 mL of solution, what is the molar concentration of the permanganate ion, \[\text{MnO}_4^-\], 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?
Expert Solution
Step 1
Step by step
Solved in 2 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY