Problem: A precipitation reaction.Which ions remain in solution after PbI2 precipitation is complete?

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FREE Expert Solution

We are asked to identify which ions remain after PbI2 precipitates in the given reaction:

2 KI(aq) + Pb(NO3)(aq) → 2 KNO3(aq) + PbI2(s)


We will refer to the solubility rules shown below:

Solubility Rules:

•Soluble Ionic Compounds:

▪ Group 1A ions (Li+, Na+, K+, etc.) and Ammonium ion (NH4+) are soluble
▪ Nitrates (NO3-), Acetates (CH3COO- or C2H3O2-), and most Perchlorates (ClO4-) are soluble
▪ Cl-, Br-, and I- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+
▪ Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+

•Insoluble Ionic Compounds:

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Problem Details


A series of photographs shows the overall reaction of the reactants 2 KI (aqueous) plus Pb(NO3) 2 (aqueous) going to the products 2 KNO3 (aqueous) plus PbI2 (solid). In the first photograph, K+ and I- ions in solution are added to a beaker containing Pb2+ and NO3- ions in solution. In the second photograph, Pb2+ (aqueous) and I- (aqueous) combine to form a yellow solid precipitate. In the third photograph, the solid precipitate has settled on the bottom of the beaker. Because PbI2 is ionic, it forms a 3-dimensional structure.

A precipitation reaction.


Which ions remain in solution after PbI2 precipitation is complete?

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