the solubility of CuCl2 is 2×10mol.dm³ what is the solubility product constant KSP, for CuCl2?
Is the solubility really 20 mols/L? Is this a "made up" problem? I wouldn't think CuCl2 has a Ksp.
To determine the solubility product constant (Ksp) for CuCl2, we need the concentration of Cu2+ and Cl- ions in the saturated solution of CuCl2. The molar solubility of CuCl2 can be used to calculate these concentrations.
Given that the molar solubility of CuCl2 is 2 × 10 mol.dm³, we can assume that the dissolution of CuCl2 is stoichiometric, meaning that one mole of CuCl2 will produce one mole of Cu2+ ions and two moles of Cl- ions.
Therefore, the concentration of Cu2+ ions in the saturated solution is 2 × 10 mol.dm³, and the concentration of Cl- ions in the saturated solution is 2 × (2 × 10) = 4 × 10 mol.dm³.
The solubility product constant (Ksp) can be calculated by multiplying the concentrations of the Cu2+ and Cl- ions:
Ksp = [Cu2+][Cl-]
Ksp = (2 × 10)(4 × 10) = 8 × 10² = 800
Hence, the solubility product constant (Ksp) for CuCl2 is 800.