Ksp → equilibrium constant related to slightly soluble ionic compounds.
PbBr2 dissociates in solution:
PbBr2(s) ⇌ Pb2+(aq) + 2 Br–(aq)
KBr dissociates completely in solution: KBr → K+ + Br-
Using an ICE table:
The Ksp of PbBr2 is 6.60 x 10-6
What is the molar solubility(M) of PbBr2 in 0.500M KBr solution?
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