1. The problem statement, all variables and given/known data I have worked these two problems to the best of my knowledge and I keep getting the wrong answer (I'm not sure what the right answer is). Here are the questions: 1. At a certain temperature the solubility of barium chromate (BaCrO4) is 1.9×10-5 mol/L. What is the Ksp of BaCrO4 at this temperature? 2. What is the molar solubility of silver phosphate (Ag3PO4) in water? Ksp = 1.8×10-18. 2. Relevant equations The relevant equations are Ksp=([products]/[reactants]) 3. The attempt at a solution For question 1: BaCrO4⇔Ba2+ + CrO42- Ksp=[Ba2+][CrO42-]/1 (since it is a solid) Ksp=[x][x]=x2 Ksp=[1.9x10-5]2=3.61x10-10 = 3.6x10-10 For question 2: Ag3PO4⇔3Ag+ + PO43- 1.8x10-18 = ([Ag+]3[PO43-])/1 1.8x10-18 = [3x]3[x] 1.8x10-18 = [27x4] then divide both sides by 27 6.6666667x10-20 = x4 then do the fourth root on both sides x = 1.6068568x10-5 = 1.6x10-5 I would very much appreciate any insight into this. Thank you!