EXERCISE I -3.1. How many mL of 0.250 N TI3* is needed to react quantitatively with 10.00 mL of 0.175 M Sn*.The redox products are TI* and Sn**2. A 0.2586 g sample contains only pure NazC2O4 ( MW = 134.00) and pure KHC204 (MW = 128.13).It required 48.39 mL of 0.01660M KMNO4 for titration to the equivalence point in an acid solutionwhere the MnO4 was reduced to Mn2+ and the C20,- oxidized to CO2. How much KHC204 waspresent in the mixture?

This is a multiple type question. According to bartleby guidelines I have to solve only first…

EXERCISE I -3. 1. How many mL of 0.250 N TI3* is needed to react quantitatively with 10.00 mL of 0.175 M Sn*. The redox products are TI* and Sn*+

EXERCISE I -3. 1. How many mL of 0.250 N TI3* is needed to react quantitatively with 10.00 mL of 0.175 M Sn. The redox products are TI and Sn*+

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

EXERCISE I -3.
1. How many mL of 0.250 N TI3* is needed to react quantitatively with 10.00 mL of 0.175 M Sn*.
The redox products are TI* and Sn**
2. A 0.2586 g sample contains only pure NazC2O4 ( MW = 134.00) and pure KHC204 (MW = 128.13).
It required 48.39 mL of 0.01660M KMNO4 for titration to the equivalence point in an acid solution
where the MnO4 was reduced to Mn2+ and the C20,- oxidized to CO2. How much KHC204 was
present in the mixture?

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