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Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:   I-(aq) + I2(aq)= I3-(aq) K = 693.   For each of the following cases calculate the equilibrium ratio of [I3-] to [I2].   A) 3.00×10-2 mol of I2 is added to 1.00 L of 3.00×10-1 M KI solution.   B)The solution above is diluted to 5.50 L.

Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:   I-(aq) + I2(aq)= I3-(aq) K = 693.   For each of the following cases calculate the equilibrium ratio of [I3-] to [I2].   A) 3.00×10-2 mol of I2 is added to 1.00 L of 3.00×10-1 M KI solution.   B)The solution above is diluted to 5.50 L.

Chemistry
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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Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:

 

I-(aq) + I2(aq)= I3-(aq) K = 693.

 

For each of the following cases calculate the equilibrium ratio of [I3-] to [I2].

 

A) 3.00×10-2 mol of I2 is added to 1.00 L of 3.00×10-1 M KI solution.

 

B)The solution above is diluted to 5.50 L. 

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