# Problem: The Ksp of CaF2 at 25 °C is 4 x 10-11. Consider a solution that is 1.0 x 10-4 M Ca(NO3)2 and 2.0 x 10-4 M NaF.a. Q = Ksp and a precipitate will not form.b. Q &gt; Ksp and a precipitate will form.c. Q &gt; Ksp and a precipitate will not form.d. Q &lt; Ksp and a precipitate will form.e. Q &lt; Ksp and a precipitate will not form.

###### FREE Expert Solution

We’re being asked to determine if a precipitate will form in a solution that is 1.0 x 10-4 M Ca(NO3)2 and 2.0 x 10-4 M NaF.

For this, we need to compare the reaction quotient (Q) vs. the solubility product constant (Ksp)

Recall that when:

• Q > Ksp: the solution is supersaturated and a precipitate will form. Reactants are favored.

• Q = Ksp: the solution is at equilibrium and no precipitate will form.

• Q < Ksp: the solution is unsaturated and no precipitate will form. Products are favored.

The expected precipitate is CaF2. The dissociation of CaF2 in water is as follows:

CaF2(s)  Ca2+(aq) + 2 F(aq)

99% (37 ratings)
###### Problem Details

The Ksp of CaF2 at 25 °C is 4 x 10-11. Consider a solution that is 1.0 x 10-4 M Ca(NO3)2 and 2.0 x 10-4 M NaF.

a. Q = Ksp and a precipitate will not form.
b. Q > Ksp and a precipitate will form.
c. Q > Ksp and a precipitate will not form.
d. Q < Ksp and a precipitate will form.
e. Q < Ksp and a precipitate will not form.