I am currently stuck on a chem solubility question any help would be appreciated. "What is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.78? The equilibrium is Ag2O(s) + H2O(l) 2Ag+(aq) + 2OH-(aq); Kc = 2.0*10^-8" Thank you.

Question

I am currently stuck on a chem solubility question any help would be appreciated. "What is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.78? The equilibrium is Ag2O(s) + H2O(l) <--> 2Ag+(aq) + 2OH-(aq); Kc = 2.0*10^-8" Thank you.

aaronq · Answer

Write the Kc expression. The pH tells you $[OH^-]$ indirectly. Find the concentration of $Ag^+$.

jfraser · Answer

you have a dissociation equation, but it's also a common-ion effect problem, so the starting concentration of the hydroxide ion is NOT zero at the start, as in a simple ICE table. You use the same approach, as @aaronq suggests, but the numbers start off differently