CaF2(s)⇄Ca2+(aq)+2F−(aq) Ksp=3.9×10−11
HF(aq)⇄H+(aq)+F−(aq) Kc=6.8×10−4
The dissolution of calcium fluoride is represented by the equilibrium system above at 25°C. The F− ion is produced when the weak acid HF dissociates. If solid calcium fluoride is added to equal volumes of the following solutions at 25°C, in which solution will the most calcium fluoride dissolve?

A) Pure distilled water

B) 1MHNO3(aq)

C) 1MNaOH(aq)

D) A saturated aqueous CaF2 solution

A system in equilibrium is subjected to change (change in concentration/pressure of reactants/products, temperature, etc.) according to Le Châtelier's principle.

To counterbalance the change and restore equilibrium, the System advances in a direction.

In solution, HNO is a strong acid that will dissociate fully to generate H+ and No3-.

This increasing concentration of H+ will cause the second equilibrium reaction in question to reverse direction, resulting in the production of additional HF.

As a result of the drop in F- concentration, the dissolution equilibrium process of Caf2 moves forward, dissolving more valid CaF2 to produce Ca2+ and F_ and thereby boosting Caf2 solubility.

Thus, HNO3 (B) is the correct option.

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