1. A sample of pure sodium oxalate, Na,C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C, requiring 45.12 mL of a KMNO4 solution. The end poin is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C,0,2 + 2 MnO4 + 10H* → 10CO2 + 2MN2+ + 8H20
1. A sample of pure sodium oxalate, Na,C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C, requiring 45.12 mL of a KMNO4 solution. The end poin is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C,0,2 + 2 MnO4 + 10H* → 10CO2 + 2MN2+ + 8H20
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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![EXERCISE II - 3
1. A sample of pure sodium oxalate, Na,C204 , weighing 0.2856 g is dissolved in water, sulfuric acid
is added, and the solution titrated at 70°C, requiring 45.12 mL of a KMNO4 solution. The end point
is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid.
Calculate the normality of the KMNO4 solution.
Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in
oxidation state by determining the balanced redox reaction:
+ 10H*
5C,0, +
2 MnO4
10CO2
+ 2MN2+
+ 8H20
->
2. A sample of pure sodium chloride (MW = EW = 58.44 ) weighing 0.2286 g is dissolved in water
and exactly 50.00 mL of silver nitrate solution is added to precipitate AgClI. The excess Ag*
is titrated with 12.56 mL of a 0.0986 N solution of KSCN. Calculate the normality of the AgNO,
solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0389d20-ac4c-4836-97d6-0535c0a39d85%2Ffa5168e8-3f96-42be-a862-5cfede60da6a%2F2tu3n8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:EXERCISE II - 3
1. A sample of pure sodium oxalate, Na,C204 , weighing 0.2856 g is dissolved in water, sulfuric acid
is added, and the solution titrated at 70°C, requiring 45.12 mL of a KMNO4 solution. The end point
is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid.
Calculate the normality of the KMNO4 solution.
Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in
oxidation state by determining the balanced redox reaction:
+ 10H*
5C,0, +
2 MnO4
10CO2
+ 2MN2+
+ 8H20
->
2. A sample of pure sodium chloride (MW = EW = 58.44 ) weighing 0.2286 g is dissolved in water
and exactly 50.00 mL of silver nitrate solution is added to precipitate AgClI. The excess Ag*
is titrated with 12.56 mL of a 0.0986 N solution of KSCN. Calculate the normality of the AgNO,
solution.
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