Identify each as soluble (S) or insoluble (I). PbI2

Question

Identify each as soluble (S) or insoluble (I). PbI2

BlackTom AI · Accepted Answer

We are asked to classify PbI2 as soluble (S) or insoluble (I) in water.
First, recall the general solubility rules: most salts of alkali metals (Li+, Na+, K+, etc.) and ammonium (NH4+) are soluble, as are most nitrates, acetates, and chlorides, with notable exceptions.
Second, for halides, most are soluble, but there is an important exception: iodides (I−) become insoluble when paired with heavy metal cations such as Pb2+, Ag+, Hg22+, and Hg2+. Since Pb2+ is in PbI2, this rule predicts decreased solubility.
Third, consider the lattice energy and ionic interactions: lead(II) iodide forms a relatively strong ionic lattice, and water molecules are often not sufficient to overcome the lattice energy to dissolve a significant amount of PbI2 at room temperature.
Fourth, empirical solubility data confirms that PbI2 has very low solubility in water, often described as insoluble or only sparingly soluble, with a solubility product (Ksp) that is very small in comparison to highly soluble salts.
Fifth, even though some iodide salts can be soluble in certain conditions, the Pb2+–I− combination is a classic insoluble pair under standard laboratory conditions, reinforcing the classification as insoluble.
In summary, applying the halide solubility exception for Pb2+ with iodide and the general tendency of PbI2 to resist dissolution due to lattice energy, PbI2 is insoluble in water.

Identify each as soluble (S) or insoluble (I). PbI2Short answer

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