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!
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Ment to write that PbCl2 in the conjugate base of HCL, not HCL is the conjugate base of PbCl2.... sorry about that!
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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