Asked by Christina
The mineral CaF2 has a solubility of 2.1 x 10^-4 M. What is the Ksp of CaF2?
a. 1.85x10^-11
b. 9.3x10^-12
c. 3.7x10^-11
d. 8.8x10^-3
a. 1.85x10^-11
b. 9.3x10^-12
c. 3.7x10^-11
d. 8.8x10^-3
Answers
Answered by
DrBob222
CaF2 ==> Ca^+2 + 2F^-
Ksp = (Ca^+2)(F^-)^2
You know solubility CaF2 = 2.1 x 10^-4; therefore, (Ca^+2) = 2.1 x 10^-4. Since (F^-) is twice that, (F^-) = 4.2 x 10^-4. Plug those values into the Ksp expression I wrote above and solve for Ksp. Post your work if you get stuck.
Ksp = (Ca^+2)(F^-)^2
You know solubility CaF2 = 2.1 x 10^-4; therefore, (Ca^+2) = 2.1 x 10^-4. Since (F^-) is twice that, (F^-) = 4.2 x 10^-4. Plug those values into the Ksp expression I wrote above and solve for Ksp. Post your work if you get stuck.
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.