18. Aqueous Equilibrium

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?

A 120.0 mL sample of a solution that is 2.8 × 10^-3 M AgNO3 is mixed with 225.0 mL of a solution that is 0.10 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+ remains?

Given the molar solubility of Pd(SCN)₂ in pure water is 2.22×10⁻⁸ M, what is the solubility product constant (Ksp) for Pd(SCN)₂?

Given that the solubility product constant (K_{sp}) of C_2D_3 is 9.14 × 10^{-9}, what is the molar solubility (S) of C_2D_3 in pure water?

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.

Determine the molar solubility of Fe(OH)₂ in pure water given that the Ksp for Fe(OH)₂ is 4.87 × 10⁻¹⁷.

In water, the solubility of Bi(OH)3 is 2.87 × 10⁻⁷ M. Calculate the solubility product constant (Ksp) for Bi(OH)3.

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

Which of the following is the correct Ksp expression for the compound C2D3 in terms of its molar solubility x?

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

Ksp = 2 × 10^(-19) for LaF3. Calculate the solubility of LaF3 in grams per liter in a solution that is 0.013 M in KF.

Given the molar solubility of BaCrO₄ in pure water is 1.08×10⁻⁵ M, what is the solubility product constant (Ksp) for BaCrO₄?

The solubility of Ni₃(PO₄)₂ in water at a particular temperature is 8.0 × 10⁻⁶ M. What is the solubility product constant (Ksp) for Ni₃(PO₄)₂?