Asked by Esmerelda
What is the solubility product of CaF2 if 0.1 M Ca2+ and 0.02 M F- are in solution just before precipitation occurs?
4.0 × 10^-5
The solubility product cannot be determined.
1.6 × 10^-4
2.0 × 10^-3
4.0 × 10^-5
The solubility product cannot be determined.
1.6 × 10^-4
2.0 × 10^-3
Answers
Answered by
DrBob222
.....................CaF2 ==> Ca^2+ + 2F^-
Write the Ksp expression for CaF2, the problem gives you the value for Ca^2+ and for F^-, cubstitute those values and solve for Kp. NOTE: The problem tells you that the (F^-) is 0.02M. Do NOT mutiply that by 2.
Write the Ksp expression for CaF2, the problem gives you the value for Ca^2+ and for F^-, cubstitute those values and solve for Kp. NOTE: The problem tells you that the (F^-) is 0.02M. Do NOT mutiply that by 2.
Answered by
Rosé
It's 4.0 × 10^-5
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.