18. Aqueous Equilibrium

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?

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 the solubility product constant (Ksp) for AgI is 8.3 x 10^-17 and the formation constant (Kf) for Ag(CN)₂⁻ is 1.0 x 10^21, calculate the equilibrium constant for the reaction AgI(s) + 2CN⁻(aq) ⇌ Ag(CN)₂⁻(aq) + I⁻(aq).

Using the Ksp for calcium iodate hexahydrate, calculate the molarity of calcium ions in a saturated solution if the Ksp is 6.47 x 10^-6.

What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10⁻² M in the chloride ion, Cl⁻? The Ksp for lead(II) chloride is 1.17×10⁻⁵.

What is the molar solubility of CaCO3 in ocean water at pH 8.3, given that the solubility is pH dependent and the dissociation constants are Ka1(H2CO3) = 4.3x10^-7 and Ka2(H2CO3) = 5.6x10^-11?

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

Determine the molar solubility of Zn(OH)₂ in a buffer solution with a pH of 11.5, given that the Ksp of Zn(OH)₂ is 4.0 x 10⁻¹⁷.

Determine the molar solubility of Al(OH)₃ in a solution containing 0.05 M AlCl₃. Ksp of Al(OH)₃ = 1.3 x 10⁻³³.

A solution containing Ca(NO3)2 is mixed with a solution of Li2S to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in sulfide ion. What will happen once these solutions are mixed? Ksp (CaS) = 2.3 × 10^-9.

What is the concentration of Al³⁺ ions in a saturated solution of Al(OH)₃ with a Ksp of 1.3 × 10⁻³³?

What is the molar solubility of barium fluoride (BaF2) in a 0.15 M NaF solution, given that the solubility product constant (Ksp) for BaF2 is 2.45 × 10^-5?