1 / 21

Solubility and Complexation Equilibria

Solubility and Complexation Equilibria. Chapter 18. Is AgCl soluble or insoluble?. Dissolution Reactions and K sp Expressions AgCl (s) Mg(OH) 2 (s) Ca 3 (PO 4 ) 2 (s). Standard Reaction Types:. Determining K sp Experimentally

zytka
Download Presentation

Solubility and Complexation Equilibria

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Solubility and Complexation Equilibria Chapter 18

  2. Is AgCl soluble or insoluble?

  3. Dissolution Reactions and Ksp Expressions AgCl(s) Mg(OH)2(s) Ca3(PO4)2(s)

  4. Standard Reaction Types:

  5. Determining Ksp Experimentally The solubility of PbF2 is found to be 0.525 g/L. What is Ksp?

  6. Predicting Solubility

  7. Can you eyeball rank solubilities? AgCl AgBr AgCl CaF2

  8. Standard Types

  9. Determining if a precipitation will occur:

  10. Determining if a precipitation will occur: If 5.0 mL of 1.0 x 10-3M NaCl is added to 1.0 mL of 1.0 x 10-3M Pb(NO3)2, will solid PbCl2 (Ksp = 1.7 x 10-5) precipitate? If a precipitate will not form, what chloride ion concentration will cause a precipitate of lead chloride to form?

  11. Determining if a precipitation will occur: If 5.0 mL of 1.0 x 10-3M NaCl is added to 1.0 mL of 1.0 x 10-3M Pb(NO3)2, will solid PbCl2 (Ksp = 1.7 x 10-5) precipitate? If a precipitate will not form, what chloride ion concentration will cause a precipitate of lead chloride to form?

  12. Common Ion Effect: The presence of an ion common to a solubility equilibrium will decrease solubility of the salt. Will PbCl2 be more soluble in pure water or in a 0.200 M NaCl solution?

  13. Common Ion Effect: The presence of an ion common to a solubility equilibrium will decrease solubility of the salt. What is the solubility of PbCl2 in pure water and in a 0.200 M NaCl solution? (Ksp = 1.7 x 10-5)

  14. Common Ion Effect: The presence of an ion common to a solubility equilibrium will decrease solubility of the salt. What is the solubility of PbCl2 in pure water and in a 0.200 M NaCl solution?

More Related