Chemical Equation: Dissociating PbBr2 - Ksp of 6.3E-6

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The discussion centers on the dissociation of lead (II) bromide (PbBr2) in water, with a solubility product constant (Ksp) of 6.3E-6. PbBr2 dissociates into lead ions (Pb²⁺) and bromide ions (Br⁻) when it dissolves. Participants emphasize that PbBr2 is an ionic compound and slightly soluble, which is crucial for understanding its dissociation. The equilibrium is reached when the concentration of the ions in solution stabilizes. The conversation highlights the importance of recognizing the ionic nature of PbBr2 to solve the problem effectively.
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the Ksp of lead (II) bromide is 6.3E-6. A large amount of PbBr2 sits at the bottom of a beaker with water above it. Equilibrium is reached. Write the chemical equation fo rthe dissociation of lead II bromide as it dissolves for which the Ksp applies.


-How would i go about solving this problem?
 
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What are the ions in PbBr2?
 
there are none. it just shows PbBr2
 
kokenwa, rethink eli64's question. PbBr2 is an ionic compound, so you should be able to answer his question. Also, PbBr2 is slightly soluble, therefore you should think through to your original question.
 

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