Asked by Morgan
If the solubility of CaF2 (s) in water is 5.0 x 10^-3. The solubility will be
A. The same in 0.10 M NaF
B. less than 0.10 M NaF
C. Higher in 0.10 M NaF
D.None of the above
A. The same in 0.10 M NaF
B. less than 0.10 M NaF
C. Higher in 0.10 M NaF
D.None of the above
Answers
Answered by
DrBob222
Why can't you use the same screen name. It takes longer to answer when we must surf through different names. At least you're consistent;ie., I see all of the names start with the letter M.
........CaF2 ==> Ca^2+ + 2F^-
Ksp = (Ca^2+)(F^-)^2 = 5E-3
Then NaF --> Na^+ + F^-
Note NaF is 100^ ionized and 0.1M NaF gives 0.1M Na^+ and 0.1M F^-. So F^- is a common ion, that will increase F^- in the CaF2 equilibrium, the reaction will shift to the left and ........
........CaF2 ==> Ca^2+ + 2F^-
Ksp = (Ca^2+)(F^-)^2 = 5E-3
Then NaF --> Na^+ + F^-
Note NaF is 100^ ionized and 0.1M NaF gives 0.1M Na^+ and 0.1M F^-. So F^- is a common ion, that will increase F^- in the CaF2 equilibrium, the reaction will shift to the left and ........
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