Final answer:
The molar solubility of CuX can be calculated using the solubility product constant (Ksp). In pure water, the molar solubility is approximately 1.13 × 10⁻¹⁸ M. In the presence of 0.24 M CuCl₂, the molar solubility is approximately 5.29 × 10⁻³ M.
Step-by-step explanation:
The molar solubility of CuX can be calculated using the solubility product constant (Ksp). The general form of the reaction is CuX(s) ⇌ Cu²⁺(aq) + X⁻(aq), where Cu²⁺ and X⁻ represent the ions in solution.
a. To calculate the molar solubility in pure water, we assume that the concentration of X⁻ is equal to the molar solubility of CuX. Therefore, x² = Ksp, and x = √(Ksp). Substituting the given Ksp value (1.27 × 10⁻³⁶) into the equation, the molar solubility of CuX in pure water is approximately 1.13 × 10⁻¹⁸ M.
b. In the presence of 0.24 M CuCl₂, the concentration of Cu²⁺ is 0.24 M. Since Cu²⁺ combines with X⁻ to form CuX and the concentration of X⁻ is equal to the molar solubility of CuX, the equation becomes Cu²⁺(0.24 M) × X⁻ = Ksp. Solving for X⁻, the molar solubility of CuX in 0.24 M CuCl₂ is approximately 5.29 × 10⁻³ M.