Asked by Robin

Explain why the solubility of PbF2 is pH dependent, but the solubility of PbCl2 is not. I know the solubility of PbF2 is pH dependent because the solubility would increase as the solution becomes more acidic because the F^- ion is the conjugate weak base of the weak acid HF. So the solubility equilibrium of PbF2 is shifted to the right as the concentration of F^- ions is reduced by the protonation to form HF. I know the conjugate base of PbCl2 is HCL, making a strong acid that does not ionize. But am having problems wording and finding a direct answer on how to properly word why PbCl2 is not pH dependent. Please better explain! Thanks!
Answered by Robin
Ment to write that PbCl2 in the conjugate base of HCL, not HCL is the conjugate base of PbCl2.... sorry about that!
Answered by DrBob222
Robin,you've done a terrific job but you need a couple of changes. Is F^- a weak base; if so it would not attract H^+ to make HF. Then HCl is a strong acid that IONIZES COMPLETELY which makes Cl^- a weak conjugate base of HCl. Since HF is a weak base the added H^+ makes HF but added acid to PbCl2 does not make HCl since it is a strong acid.
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