18. Aqueous Equilibrium

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?

A saturated solution of PbCl2 has [Cl^-] = 2.86×10^-2 M. What is the concentration of Pb^2+? Given that Ksp = 1.17 × 10^-5.

A solution is 0.040 M in Pb²⁺. What minimum concentration of Cl⁻ is required to begin to precipitate PbCl₂? For PbCl₂, Ksp = 1.17×10⁻⁵.

At 25°C, calcium fluoride (CaF2) has a solubility product constant Ksp = 3.5 × 10^-11. What is the solubility of CaF2 in mol/L at this temperature?

C2D3 has a solubility product constant (Ksp) of 9.14×10⁻⁹. What is the molar solubility of C2D3 in mol/L?

C2D3 has a solubility product constant (Ksp) of 9.14 × 10⁻⁹. What is the molar solubility of C2D3 in mol/L?

Ca3(PO4)2 is being dissolved in water. If only 0.46 g of Ca3(PO4)2 will dissolve in 100 mL of water at 25°C, what is the solubility product, Ksp, of this salt at this temperature?

Given the solubility product constant (Ksp) for PbBr₂ is 6.3 x 10⁻⁶, calculate the maximum concentration of Br⁻ ions that can exist in 0.5 L of 0.1 M PbBr₂ solution.

Calculate the molar solubility of CuX in a 0.18 M Na2X solution, given that the solubility product constant (Ksp) for CuX is 1.27×10^-36.

Calculate the molar solubility of MgF2 in 0.15 M MgCl2 at 25 °C, given that the Ksp of MgF2 is 6.4 x 10^-9.

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

Calculate the molar solubility of barium fluoride (BaF2) in pure water, given that its solubility product constant (Ksp) is 2.45 x 10^-5.

What is the molar solubility of barium fluoride (BaF₂) in a 0.12 M Ba(NO₃)₂ solution, given that the solubility product constant (Ksp) for BaF₂ is 2.45 × 10⁻⁵?