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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 = 710. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2].   1a) 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. 1b)The solution above is diluted to 11.00 L. how do i do this? is an icetable required?

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 = 710. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2].   1a) 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. 1b)The solution above is diluted to 11.00 L. how do i do this? is an icetable required?

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 = 710.

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

 

1a) 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution.

1b)The solution above is diluted to 11.00 L.

how do i do this? is an icetable required?

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