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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 & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.6: Disturbing A Chemical Equilibrium
Problem 2.3ACP: A 0.64 g sample of the white crystalline dimer (4) is dissolved in 25.0 mL of benzene at 20 C. Use...
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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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