18. Aqueous Equilibrium

Calculate the molar solubility of MgF2 in 0.15 M MgCl2 at 25 °C, given that the Ksp of MgF2 is 6.4 x 10^-9.

What is the molar solubility of barium fluoride (BaF₂) in pure water if the solubility product constant (Ksp) is 2.45×10⁻⁵?

Calculate the molar solubility of barium fluoride (BaF2) in pure water, given that its solubility product constant (Ksp) is 2.45 x 10^-5.

What is the molar solubility of barium fluoride (BaF₂) in a 0.12 M Ba(NO₃)₂ solution, given that the solubility product constant (Ksp) for BaF₂ is 2.45 × 10⁻⁵?

Calculate the molar solubility of barium fluoride (BaF₂) in pure water, given that its solubility product constant (Ksp) is 2.45 × 10⁻⁵.

Calculate the molar solubility of calcium fluoride (CaF2) in g/L if its solubility product constant (Ksp) is 5.3×10^-11.

Calculate the molar solubility of magnesium fluoride (MgF2) in a solution that is 0.350 M in NaF. For magnesium fluoride, Ksp = 5.16 x 10^-11.

Calculate the molar solubility of tin(II) hydroxide (Sn(OH)₂) in pure water given that its solubility product constant (Ksp) is 5.45 x 10⁻²⁷.

Calculate the solubility (in grams per 1.00×10^2 mL of solution) of magnesium hydroxide in a solution buffered at pH = 12 given that the Ksp for Mg(OH)2 is 2.06×10^(-13).

Calculate the solubility (in grams per 1.00×10² mL of solution) of magnesium hydroxide, Mg(OH)₂, in a solution buffered at pH = 12, given that the Ksp of Mg(OH)₂ is 1.8 × 10⁻¹¹.

Calculate the solubility (in grams per 1.00×10² mL of solution) of magnesium hydroxide (Mg(OH)₂) in a solution buffered at pH = 10, given that the Ksp of Mg(OH)₂ is 1.8 × 10⁻¹¹.

Calculate the solubility of LaF₃ in grams per liter in pure water, given that the Ksp of LaF₃ is 2.0 x 10⁻¹⁹.

Which of the following is the correct Kₛₚ expression for the dissolution of Sr₃(PO₄)₂ in water?

Given a solution of 4.0 × 10⁻² M Ba(NO₃)₂, what is the minimum concentration of NaF required to cause precipitation of BaF₂, assuming the Ksp of BaF₂ is 1.7 × 10⁻⁶?

What is the minimum concentration of sulfate ions (SO₄²⁻) required to cause precipitation of calcium ions (Ca²⁺) from a 9.0×10⁻² M CaI₂ solution, given that the Ksp of CaSO₄ is 2.4×10⁻⁵?