18. Aqueous Equilibrium

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?

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?

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

Given the molar solubility of Ag2SO3 in pure water is 1.55 x 10^-5 M, what is the solubility product constant (Ksp) for Ag2SO3?

Given the molar solubility of Ag2SO3 in pure water is 1.55×10⁻⁵ M, what is the solubility product constant (Ksp) for Ag2SO3?