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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].   6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. the answer you provided (299) was not correct

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].   6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. the answer you provided (299) was not correct

Physical Chemistry
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter5: Introduction To Chemical Equilibrium
Section: Chapter Questions
Problem 5.16E: 5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of...
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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].

 

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

the answer you provided (299) was not correct

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