Final answer:
The statement that PbCl2 does not react with HCl immediately because of low HCl concentration is false; the reaction is influenced by the common ion effect which shifts the equilibrium and promotes precipitation.
Step-by-step explanation:
The question asks whether PbCl2 does not react with HCl immediately because the HCl concentration is low. This statement is false. The lack of immediate reaction is instead due to the common ion effect, where the added HCl increases the chloride ion concentration in the solution. This causes the reaction quotient for PbCl₂ to be greater than the equilibrium constant, leading to a shift of the reaction towards the left, promoting the precipitation of PbCl₂ and thus decreasing its solubility in the reaction.