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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: thisisvik on August 09, 2008, 06:52:25 PM

Title: Equilibrium Constant from Ksp / Kf / Ka
Post by: thisisvik on August 09, 2008, 06:52:25 PM

I could not find any method to approach this question.. it stumped me.. am I missing something simple?

Using the value of Ksp for Ag₂S, the Ka1 and Ka2 for H₂S, and the Kf for AgCl₂^-; calculate the equilibrium constant for the following reaction:

Ag₂S_(aq)+ 4Cl^-_(aq) + 2 H⁺_(aq) <---> 2 AgCl₂^-_(aq) + H₂S_(aq)

I know you can get the molar solubility for Ag₂S, and that the Kf for AgCl₂^- is 1.1 x 10⁵... but I have no idea how this helps me reach the equilibrium constant???

Any help is greatly appreciated..

Title: Re: Equilibrium Constant from Ksp / Kf / Ka
Post by: Yggdrasil on August 09, 2008, 07:14:05 PM

First write out the chemical reactions represented by each of the equilibrium constants.

Then find a way to combine those chemical reactions to obtain the desired reaction.