1. The problem statement, all variables and given/known data What is the solubility (gram/liter) of Cr(OH)3 (103.02 g/mol) in a solution buffered at pH = 8.673? The pKsp of Cr(OH)3 is 30.220. 2. Relevant equations Ksp = [Cr][OH]^3 Cr(OH)3 -> Cr + 3OH 3. The attempt at a solution I have already solved that Ksp = 6.0256 E -31, but i'm not entirely sure what to do with the buffer pH. I tried using it to find the pOH and subsequently [OH], but for some reason I'm not getting the right answer. Do I plug [OH] into the Ksp equation after finding out the concentration using the pH or is there a step i'm missing?