Okay, first thing I do is set up the Ksp expression since we're given a Ksp.
Ksp = [Ca] [F]^2 (Notice, CaF2 <-> Ca + 2F)
Now, they want to know at what concentration [F] will cause precipitate to form. We know that at Ksp, we're in equilibrium, so the reaction isn't going to be forming precipitate. So we need to figure out what [F] is at equilibrium, and see in our answers which one is immediately greater (le chatelier), because once a greater amount of [F] occurs, it will push the reaction to the left and form precipitate.
4*10^-11 = [0.1] [2x]^2
(Notice, [Ca] has a common ion effect from the Ca(NO3)2, so first it would be [x + 0.1] but since x is very small, we just use 0.1)
4*10^-10 = 4x^2 (I'm sure you can do the math)
1*10^-10 = x^2
1*10^-5 = x
Okay, so we now know that at equilibrium (Ksp), concentration of [F] is this number, so we see in our answers that (b) is the number most closely larger, so that is when precipitate will BEGIN to form (shift to the left, forming CaF2). Notice that choice (a) is also larger, and would also form precipitate (just that it would begin at the smaller number).
Hope this helps.
Edit: Btw, I don't think it's such an easy problem, they're asking for a strange thing (not just a Ksp, or concentration, etc), they threw in a common ion as well, and the balanced reaction uses a non 1:1 molar ratio.