Multiple Choice
Given a solution of 4.0 × 10⁻² M Ba(NO₃)₂, what is the minimum concentration of NaF required to cause precipitation of BaF₂, assuming the Ksp of BaF₂ is 1.7 × 10⁻⁶?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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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.
A
2.52 x 10^-8 M
B
6.3 x 10^-9 M
C
1.575 x 10^-9 M
D
1.575 x 10^-8 M
Verified step by step guidance1
Identify the dissolution reaction for CuBr: CuBr(s) ⇌ Cu⁺(aq) + Br⁻(aq).
Write the expression for the solubility product constant (Ksp) for CuBr: Ksp = [Cu⁺][Br⁻].
Recognize that the solution already contains 0.4 M Br⁻ from KBr, which will affect the solubility of CuBr due to the common ion effect.
Let the molar solubility of CuBr be 's'. Then, [Cu⁺] = s and [Br⁻] = 0.4 + s. Since s is very small compared to 0.4, approximate [Br⁻] ≈ 0.4 M.
Substitute the concentrations into the Ksp expression: 6.3 x 10^-9 = s * 0.4. Solve for 's' to find the molar solubility of CuBr in the solution.
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