If true enter 1, else enter 0.
There is precipitation of soluble AB if its ionic product is greater than $K_{s p}$ value,i.e., $[A] [B] > K_{s p}$ .

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Solution

The precipitation of AB will occur only if the ionic product exceeds solubility product. $[A^{+}] [B^{-}] > K_{s p}$
For example, $A g C l$ is precipitated if $[A g^{+}] [{C l}^{-}] > K_{s p}$
Also, ${P b I}_{2}$ is precipitate of $[{P b}^{2 +}] [I^{-}]^{2} > K_{s p}$ , hence true.
But, if the ionic product is less than solubility product, then precipitation will not occur.

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