18. Aqueous Equilibrium

Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3. The Ksp for Ag2CrO4 is 2.0 × 10^-12.

Determine the molar solubility of BaF2 in pure water given that the Ksp for BaF2 is 2.45 × 10⁻⁵.

Determine the molar solubility of CuBr in a solution containing 0.4 M KBr, given that the solubility product constant Ksp for CuBr is 6.3 x 10^-9.

Given the solubility product constant (Ksp) of NiS is 3.0 x 10^-15, determine the molar solubility of NiS in 0.052 M K2C2O4.

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

What is the expression for the solubility product constant (Ksp) for the dissolution of Ba3(PO4)2 in water?

If the molar solubility of CaF2 at 35°C is 1.24×10⁻³ mol/L, what is the Ksp at this temperature?

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

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.

NiS has a Ksp of 4.0 x 10^-20. What is the solubility of NiS in mol/L?

The Ksp of CuI(s) is 1.1 × 10^-12. Calculate the value of E° for the half-reaction CuI(s) + e^- → Cu(s) + I^-(aq).

The concentration of fluoride ions in a saturated solution of barium fluoride (BaF2) is ________ M. The solubility product constant (Ksp) of BaF2 is 1.7 x 10^-6. What is the concentration of fluoride ions?

The molar solubility of Ca(OH)₂ was experimentally determined to be 0.020 M. Based on this value, what is the Ksp of Ca(OH)₂?

The molar solubility of Ba3(PO4)2 is 8.89 × 10^-9 M in pure water. Calculate the Ksp for Ba3(PO4)2.

The molar solubility of manganese (II) hydroxide, Mn(OH)2, is 3.48 × 10^-3 M. What is the Ksp of Mn(OH)2 at this temperature?