Chapter 16 - Acid-Base Equilibria and Solubility Equilibria - Questions & Problems - Page 767: 16.57

$K_{sp}=3.3\times10^{-93}$

Find solubility in mol/L $n=m/M$ $n=3.6\times10^{-17}/288$ $n=1.25\times10^{-19}$ Write Ksp formula $K_{sp}=(2x)^2(3x)^3$ $K_{sp}=(2(1.25\times10^{-19}))^2(3(1.25\times10^{-19}))^3$ $K_{sp}=3.3\times10^{-93}$