1. The problem statement, all variables and given/known data Is it possible to make an aqueous solution with strontium hydroxide, Sr(OH)2, that gives a pOH of 10.54? Explain why or why not. 2. Relevant equations [OH-] = 10-pOH 3. The attempt at a solution [OH-] = 10-pOH = 10-10.54 = 2.88 x 10-11 mol/L OH- Every mole of Sr(OH)2 produces 2 moles of OH-. So the concentration of Sr(OH)2 is (2.88 x 10-11 mol/L) / 2 = 1.4 x 10-11 mol/L Sr(OH)2 My data table says Sr(OH)2 falls in the category of 'slightly soluble' (solubility less than 0.1 mol/L). Since the amount of Sr(OH)2 needed to make this solution is so tiny, it seems like this should work. Am I on the right track? I am confused about what this question is getting at.