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Help with a metal sulfide molar solubility question! :)

Calculate the molar solubility of a hypothetical metal sulfide, MS, in a solution saturated with H2S at 25C. The pH of the solution is 3.44. Kspa for MS is 1.7 x 10-3.
 
I know that I need to use the pH to find the H3O+ concentration... and I am pretty sure the rxn is:
MS + 2H3O <-> H2S + M + 2H2O
 
But I am not sure what to do once I have the [H3O+]... Thanks!

Comments

I'm curious. Chem is really not my specialty, but I wonder if the step you are missing is that the measured pH is 3.44, which means that [H3O+] is
 
10-3.44 = .00036
 
The ideal value is 1.7 x 10-3 = .0017
 
Hope this helps.
You are correct... but as I mentioned above "I know that I need to use the pH to find the H3O+ concentration...But I am not sure what to do once I have the [H3O+]". Thanks though! Good job for Chem not being your specialty

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