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 equilbrium ratio of [I3-] to [I2].

1. 5.00×10-2 mol of I2 is added to 1.00 L of 5.00×10-1 M KI solution.

2. The solution above is diluted to 12.00 L.

Question

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 equilbrium ratio of [I3-] to [I2].


1.   5.00×10-2 mol of I2 is added to 1.00 L of 5.00×10-1 M KI solution.


2.   The solution above is diluted to 12.00 L.