1. The problem statement, all variables and given/known data The solubility of a hydroxide M(OH)2 is .0090 g/liter. Molecular weight of M(OH)2 is 150. If 1.0 g of MSO4 is dissolved in 500 ml of water buffered at pH 8.5, will a precipitate form? 2. Relevant equations pOH + pH = 14 molarity = mol/liter 3. The attempt at a solution pOH must be 5.5, so the OH concentration is 10^-5.5 = 3.1623x10^-6. Solubility of M(OH)2 is .00006 mol/liter. I don't know where the buffer solution fits in to all of this and how to know if a precipitate forms or not. MSO4 <--> M + SO4 s s s Ksp = s^2 How can I find the solubility of MSO4? Is that even necessary?