22. Lead(II) iodide, PbI 2 , is a slightly solublesalt with a K SP value of9.8 x...
Question:
22. Lead(II) iodide, PbI2, is a slightly solublesalt with a KSP value of9.8 x 10-9. The equation for itsdissociation in water is
PbI2(s) <----------> Pb2+(aq) + 2I-(aq)
What is the molar solubility of PbI2 in distilledwater?
23. In the previous problem, you calculated the molarsolubility of PbI2 in distilled water. Nowconsider the molar solubility of PbI2 in a1.50 M NaI solution. Sodium iodide is a freely solublesalt, and completely dissociates into its ions when dissolved inwater:
NaI(s) ==========> Na+(aq) + I-(aq)
Therefore, a 1.50 M NaI solution is 1.50 M inNa+ and 1.50 M in I-. Whenthe PbI2 is dissolved in this solution, itestablishes its usual equilibrium:
PbI2(s) <----------> Pb2+(aq) + 2I-(aq) KSP = 9.8 x 10-9
But in the 1.50 M NaI solution, theI- concentration will be 1.50 Meven before thePbI2 dissociates. TheI- formed in the dissociation ofPbI2 will be in addition to thatalready present.
What is the molar solubility of PbI2 in the1.50 M NaI solution?