Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H₂O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction: 2KMnO4 (aq) + H₂O2 (aq) + 3H2SO4 (aq) → 302(g) + 2MnSO4 (aq) + K₂SO4 (aq) + 4H₂O(1) A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H₂O2 was dissolved if the titration required 14.3 mL of the KMnO4 solution?
Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H₂O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction: 2KMnO4 (aq) + H₂O2 (aq) + 3H2SO4 (aq) → 302(g) + 2MnSO4 (aq) + K₂SO4 (aq) + 4H₂O(1) A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H₂O2 was dissolved if the titration required 14.3 mL of the KMnO4 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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Question
![Part A
A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the
KOH solution if 17.2 mL of 1.50 M H₂SO4 was needed? The equation is
2KOH(aq) + H₂SO4 (aq) →K₂SO4 (aq) + 2H₂O(1)
Express your answer with the appropriate units.
► View Available Hint(s)
molarity =
Submit
Part B
μÀ
Value
Submit
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H₂O2, can be
titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:
Units
μᾶ
mass of H₂O₂ = Value
?
A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H₂O₂ was dissolved if the
titration required 14.3 mL of the KMnO4 solution?
Express your answer with the appropriate units.
► View Available Hint(s)
2KMnO4 (aq) + H₂O2 (aq) + 3H₂SO4 (aq) →
302(g) + 2MnSO4 (aq) + K₂SO4 (aq) + 4H₂O(1)
Units
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3caf0467-ca0e-4770-b0d8-25bdaac915d0%2Ff766b418-0944-481e-bcfb-10e4fa71de73%2Fcw24h3_processed.png&w=3840&q=75)
Transcribed Image Text:Part A
A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the
KOH solution if 17.2 mL of 1.50 M H₂SO4 was needed? The equation is
2KOH(aq) + H₂SO4 (aq) →K₂SO4 (aq) + 2H₂O(1)
Express your answer with the appropriate units.
► View Available Hint(s)
molarity =
Submit
Part B
μÀ
Value
Submit
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H₂O2, can be
titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:
Units
μᾶ
mass of H₂O₂ = Value
?
A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H₂O₂ was dissolved if the
titration required 14.3 mL of the KMnO4 solution?
Express your answer with the appropriate units.
► View Available Hint(s)
2KMnO4 (aq) + H₂O2 (aq) + 3H₂SO4 (aq) →
302(g) + 2MnSO4 (aq) + K₂SO4 (aq) + 4H₂O(1)
Units
?
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