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Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: Mal1ce on September 12, 2010, 12:12:28 AM

Title: Solubility Product Constant Problem
Post by: Mal1ce on September 12, 2010, 12:12:28 AM

The Problem:
The solubility-product constant for K₂PdCl₆ is 6.0 x 10^-6 (K₂PdCl₆ <--> 2K⁺ + PdCl^2-₆).  What is the K⁺ concentration of a solution prepared by mixing 50.0 mL of 0.400 M KCl with 50 mL of 0.100 M PdCl^2-₆.

The first thing I did was find the new concentrations of K⁺ and PdCl^2-₆, [K⁺] = 0.2 M and  [PdCl^2-₆] = 0.05 M. Here is where I am stuck.  I am assuming that these new concentrations are the initial concentrations and I need to find the equilibrium concentration of K⁺.  How do I use these initial concentration and the solubility-product constant to find the concentration of K⁺? Do I need to use the ICE box to solve this problem? If anyone could walk me through on how to solve this problem it would be greatly appreciated.  Thanks in advance.

Title: Re: Solubility Product Constant Problem
Post by: Borek on September 12, 2010, 03:27:32 AM

Limiting reagent.

Title: Re: Solubility Product Constant Problem
Post by: Mal1ce on September 12, 2010, 05:55:43 PM

I don't understand how this is a limiting reagent problem.

Title: Re: Solubility Product Constant Problem
Post by: Borek on September 12, 2010, 06:11:48 PM

Are they mixed in stoichiometric amounts?