Final answer:
When mixing Ca2+ and F- to form CaF2, if the reaction quotient (Qsp) is greater than the solubility product constant (Ksp), a precipitate will form. Calculate Qsp by finding the new concentrations of each ion after mixing and multiply them according to the stoichiometry of the reaction.
Step-by-step explanation:
When mixing solutions containing Ca2+ and F- ions, if the product of their concentrations exceeds the solubility product constant (Ksp) for their compound, calcium fluoride (CaF2), a precipitate will form. For the given problem, you first need to calculate the final concentrations of Ca2+ and F- ions after the solutions are mixed.
To calculate the new concentrations, you can use the formula C1V1 = C2V2. After mixing 0.16 L of 0.30 M Ca2+ with 0.301 L of 0.060 M F-, the concentrations will change due to the combined volume. Then, you calculate the reaction quotient (Qsp), which is the product of the concentrations of the ions: Qsp = [Ca2+][F-]2. If Qsp is greater than the Ksp, precipitation will occur. The set Ksp for calcium fluoride is 3.45 × 10-11.
To find the concentration of Ca2+ after dilution, we calculate (0.30 M)(0.16 L) / (0.16 L + 0.301 L) = [Ca2+]. For F-, the calculation is similar: (0.060 M)(0.301 L) / (0.16 L + 0.301 L) = [F-]. Then, plug these values into the Qsp equation to compare with Ksp.