text: Given:\nKsp = 1.9 x 10-33 \ns_Al(OH)3 = 2 x 10-14\n[Al3+] = 3[OH-]= s_As(OH)3\n\nAl(OH)3--> Al^3+ + 3 OH^-\nFormula: Ksp = [Al] x [OH]^3 = 3[OH-]^4 = 1.9x10-33 you can solve then the [OH-] of the solution in H2O only; eqtn 1\nIF YOU WANT TO REDUCE SOLUBILITY, THEN COUNT ON THE COMMON ION EFFECT- YOU ARE TO ADD OH- IN YOUR SOLUTION;\n\nTherefore       OH\ninitial         from the Ksp value\nchange          +x\nequation       [OH-] value  +x            \n\n1.9 x 10-33 = 3([OH-] value + x)^4\n\nSolve for x then plug it in the equation below\n\npH = -LOG [H+] =14 - log ([OH-]+x)