Using a value of ksp = 1.8 x 10-2 for the reaction pbcl2(s) pb+2(aq) + 2cl-(aq).
the concentration of the products yields a value of 2.1 x 10-2.

select the two statements that are true.

a) ions are recombining to form a solid precipitate.
b) the concentrations of pb+2(aq) and cl-(aq) are expected to decrease.
c) the concentrations of pb+2(aq) and cl-(aq) are expected to increase.
d) the concentration of pbcl2(s) is expected to increase.
e) it is not possible to have a system with ksp > 1.8 x 10-2.

Option A and Option B

Explanation:

The concentrations of Pb+2(aq) and Cl-(aq) are expected to decrease (because you have initially very high values of [Pb2+] and [Cl-], they should decrease so that you equilibrium is reestablished, so that Qsp = Ksp).

Solids aren't measured using concentrations but the AMOUNT of PbCl2(s) is expected to increase.

It IS possible to have a system with Ksp > 1.8 x 10^-2 -- if you increase the temperature, then solubility and Ksp are both increased. It is also possible to have a system with Qsp > Ksp (as is true in this case). However, if Qsp > Ksp, the system will shift so that reequilibrium is reestablished. Over time, Qsp will be come equal to Ksp.

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