A salt, AB_3, expresses an aqueous solubility of 0.0750*mol*L^-1 with respect to the given solubility? What is K_"sp" for this solute?

1 Answer
anor277
Nov 22, 2016

K_(sp)=[A^(3+)][B^-]^3=27xx0.0750^4

Explanation:

We examine the following equilibrium:

AB_3(s) rightleftharpoons A^(3+)+3B^-

Since the solid cannot express a concentration, we write the following expression to represent the "solubility product:"

K_(sp)=[A^(3+)][B^-]^3

As is usual in these problems, we raise each concentration to the power of the stoichiometric coefficient in the solubility expression, and thus we have the product [A^(3+)]^1xx[B^-]^3.

But we are given that [AB_3(aq)]=0.0750*mol*L^-1, and thus we are in a position to evaluate K_"sp" directly.

And thus [A]=0.0750*mol*L^-1, and [B^-]=3xx0.0750*mol*L^-1.

K_(sp)=[0.0750][3xx0.0750]^3=27xx0.0750^4

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