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" You would like to increase the solubility of CaF2 in water. What would you add to the solution:
HBr : Correct
Can someone explain why Her is the best answer, and why each other answer is wrong? Thanks!
CaF2(s) ⇋ Ca^2+ + 2F^-
Ksp = [Ca^2+][F^-]^2
What would happen if you increased the [F^-] by adding NaF, It's called the common ion effect; Due to this concentration of [F^-] increases and it will bind more and more to Ca^2+ leading to the formation of CaF2 (s) itself.
A similar reason is for CaCl2 but instead of F- here [Ca2+] will gonna increase eading to the formation of CaF2 (s) itself.
For a reason we won't go into here HF is a weak acid.
F^- + H2O ⇋ HF + OH^-
So adding the strong acid HBr will shift the equilibrium in favor of increased dissolution of CaF2.
H3O^+ + OH^- → 2H2O
Now I bet that was the last one you were thinking about?
Adding a base i.e NH3 and KOH they would push the equilibrium towards the solid, opposition to the acid.
Hope you got your answer.
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