For a sparingly soluble salt AB_2, the equilibrium concentrations of A^2+ ions and B^-ions are 1.2 10^-4M and 0.24 10^-3M, respectively. The solubility product of AB_2 is :

Question

Accepted Answer

Correct answer: A. (a) AB_2 ( s ) ⇌A_ ( aq )^+2+2 B_ ( aq )^-K_ sp= (A^+2 ) (B^- )^2 =1.2 10^-4 (2.4 10^-4)^2 =6.91 10^-12M^3

$For a sparingly soluble salt AB_{2}, the equilibrium concentrations of A^{2 +} ions and B^{-} ions are 1.2 \times 10^{- 4} M and 0.24 \times 10^{- 3} M, respectively. The solubility product of AB_{2} is :$

Solution

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