Is lead iodide a strong electrolyte?

So, lead iodide is insoluble. I see conflicting answers online. Some say it's a weak electrolyte because it is insoluble, others say it is a strong electrolyte because it is an ionic compound and any small amount that dissolves does so in the form of ions.


Which one is the correct answer?




[Lead(II) iodide](https://en.wikipedia.org/wiki/Lead(II)_iodide) is sparingly soluble in water at room temperature $(\pu{0.76 g/L}$ at $\pu{20 °C})$ and a bit more soluble in hot water $(\pu{4.1 g/L}$ at $\pu{100 °C}).$ In solution, all of the lead iodide is dissociated into ions. At high concentrations of iodide, the lead ions form two complexes, $\ce{PbI3-}$ and $\ce{PbI4^2-}$ [[1](https://doi.org/10.1021/ja01848a010)]:



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> The increase of solubility of lead iodide caused by the presence of iodide ion in concentration greater than 0.1 molal may be explained by the formation of the complex ions $\ce{PbI3-}$ and $\ce{PbI4^=}.$
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In any case, all of the dissolved lead iodide is present as ions (there is no neutral $\ce{PbI2(aq)}$ species), so it is a strong electrolyte. This is different from weak electrolytes such as, say, acetic acid, where there is a neutral species $\ce{CH3COOH(aq)}$ in solution which dissociates into the charged $\ce{CH3COO-(aq)}$ and $\ce{H+(aq)}$.


As an aside, the difference in color (colorless in solution, yellow as a solid) and the temperature-dependence of the solubility leads to a beautiful effect that has been called toxic golden rain, see e.g. video [YouTube — Golden Rain - Growing crystals of lead iodide. Chemical reaction](https://youtu.be/TRq9hnOGvaE?t=74).


### Reference


1. Lanford, O. E.; Kiehl, S. J. The Solubility of Lead Iodide in Solutions of Potassium Iodide-Complex Lead Iodide Ions. *J. Am. Chem. Soc.* **1941**, 63 (3), 667–669. DOI: [10.1021/ja01848a010](https://doi.org/10.1021/ja01848a010).


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