What is the concentration of Al³⁺ ions in a saturated solution of Al(OH)₃ with a Ksp of 1.3 × 10⁻³³?

Which of the following is the correct solubility product expression (Ksp) for magnesium phosphate, Mg3(PO4)2, when it dissociates in water?

Determine the molar solubility of Zn(OH)₂ in a buffer solution with a pH of 11.5, given that the Ksp of Zn(OH)₂ is 4.0 x 10⁻¹⁷.

Determine the molar solubility of Al(OH)₃ in a solution containing 0.05 M AlCl₃. Ksp of Al(OH)₃ = 1.3 x 10⁻³³.

A solution containing Ca(NO3)2 is mixed with a solution of Li2S to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in sulfide ion. What will happen once these solutions are mixed? Ksp (CaS) = 2.3 × 10^-9.

What is the molar solubility of barium fluoride (BaF2) in a 0.15 M NaF solution, given that the solubility product constant (Ksp) for BaF2 is 2.45 × 10^-5?

Determine the molar solubility of CaCO₃ in a solution of 0.500 M Na₂CO₃. K_sp for CaCO₃ is 4.96 × 10⁻⁹.

What is the molar solubility of PbBr₂ in pure water? K_sp for PbBr₂ is 4.67 × 10⁻⁶.