18. Aqueous Equilibrium

Solubility Product Constant: Ksp

Multiple Choice
What concentration of hydroxide ions (OH-) is needed to begin the formation of Pb(OH)2 in a solution with a [Pb2+] of 4.5 x 10^-5 M, given that the solubility product constant (Ksp) of Pb(OH)2 is 8.0 x 10^-15?
Open Question
The solubility of Ag₂SO₄ in water at 25°C is 0.0155 m. What is K_sp for Ag₂SO₄?
Multiple Choice
What is the molar solubility of Fe(OH)2 at 25°C if the Ksp of the compound is 7.9 × 10⁻¹⁶?
Multiple Choice
An ionic compound with the formula Q2Z has a molar solubility of 1.01 × 10⁻² M. What is the value of Ksp for this compound?
Multiple Choice
Determine the molar solubility of Fe(OH)₂ in pure water given that the Ksp for Fe(OH)₂ is 4.87 × 10⁻¹⁷.
Multiple Choice
Determine the molar solubility of CaCO₃ in a solution of 0.500 M Na₂CO₃. K_sp for CaCO₃ is 4.96 × 10⁻⁹.
Multiple Choice
What is the molar solubility of PbBr₂ in pure water? K_sp for PbBr₂ is 4.67 × 10⁻⁶.
Multiple Choice
Solubility of Sn(OH)₂ was found to be 1.11 x 10^-9 M; calculate K_sp of this compound.
Multiple Choice
If a saturated solution of Ag₂CO₃ contains 2.56 × 10⁻⁴ M of Ag⁺ ions, determine its solubility product constant.
Multiple Choice
What is the solubility of CN⁻ ions in a solution of 5.5 M Hg₂(CN)₂, with a K_sp of 5.0 × 10⁻⁴⁰?
Open Question
Calcium oxalate, CaC₂O₄ (m = 128.1), dissolves to the extent of 0.67 mg L^–1 . What is its K_sp?
Open Question
What is the solubility of La(IO₃)₃ in water? (K_sp of La(IO₃)₃₃ is 7.5 × 10^-12)
Open Question
Which of the following is the correct expression for K_sp for Zn₃(PO₄)₂?
Open Question
Which of the following is the correct expression for K_sp for Zn₃(PO₄)₂?
Open Question
Enter the K_sp expression for C₂D₃ in terms of the molar solubility x.