APFIVE Calculating Ksp From Molar Solubility
The salt $$AB_2$$ dissolves in water according to the equation: $$AB_2(s) \rightleftharpoons A^{2+}(aq) + 2*B^-(aq)$$. If the molar solubility of the salt is $$2.0 \times 10^{-3}\,M$$, what is the value of its solubility product constant, $$K_{sp}$$?
A
$$8.0 \times 10^{-9}$$
B
$$1.6 \times 10^{-8}$$
C
$$6.4 \times 10^{-8}$$
D
$$3.2 \times 10^{-8}$$
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