35.00 mL of a solution of KIO3 reacted with exactly 35.00 mL of a 0.1000 M solution of KI in acid medium according to the equation I03 I + H* » I2 + H2O (a) Balance the equation and calculate the molarity of the KIO3 solution. (b) 50.00 mL of this KIO3 is treated with excess pure KI in acid solution and the liberated I, is 'itrated with 0.1000 N Na2S2O3. What volume of titrant is required?

35.00 mL of a solution of KIO3 reacted with exactly 35.00 mL of a 0.1000 M solution of KI in acid medium according to the equation I03 I + H* » I2 + H2O (a) Balance the equation and calculate the molarity of the KIO3 solution. (b) 50.00 mL of this KIO3 is treated with excess pure KI in acid solution and the liberated I, is 'itrated with 0.1000 N Na2S2O3. What volume of titrant is required?

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

35.00 mL of a solution of KIO3 reacted with exactly 35.00 mL of a 0.1000 M solution of KI in acid
medium according to the equation
I03 + I + H*
» I2 + H2O
(a) Balance the equation and calculate the molarity of the KIO3 solution. (b) 59.00 mL of this
KIO3 is treated with excess pure KI in acid solution and the liberated I, is itrated with
0.1000 N Na2S2O3. What volume of titrant is required?

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