1 / 14

Catalyst

Catalyst. It is found that 1.1 x 10 -2 g of SrF 2 dissolves per 100 mL of solution. Calculate the solubility product of SrF 2. End. Acetate. Lecture 8.2 – Application of K sp. Today’s Learning Targets.

matia
Télécharger la présentation

Catalyst

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. Catalyst • It is found that 1.1 x 10-2g of SrF2 dissolves per 100 mL of solution. Calculate the solubility product of SrF2. End

  2. Acetate

  3. Lecture 8.2 – Application of Ksp

  4. Today’s Learning Targets • LT 8.4 – I can hypothesize about which slightly soluble compound will precipirate first through utilization of the Ksp

  5. Predicting Precipitation • Recall, the reaction quotient (Q) can be used to determine the direction an equilibrium needs to shift in order to achieve equilibrium: Q > Ksp: Shift left and precipitate more Q < Ksp: Shift right and dissolve more Q = Ksp: Solution is at equilibrium • Therefore, we can predict whether more or less solid will precipitate based on this answer

  6. Class Example • Does a precipitate form when 0.10 L of 8.0 x 10-3 M Pb(NO3)2 is added to 0.40 L of 5.0 x 10-3 M Na2SO4? Note – the Ksp of PbSO4 is 6.3 x 10-7

  7. Table Talk • Doe a precipitate form when 0.050 L of 2.0 x 10-2 M NaF is mixed with 0.010 L of 1.0 x 10-2 M Ca(NO3)2. KSP (CaF2) = 3.9 x 10^-11

  8. Selective Precipitation • Oftentimes, we have solutions that contain multiple solubility equilibriums. • We can selectively precipirate some of the compounds, but not all, by utilizing Ksp • The smaller the Ksp of an ion, the more likely it will precipitate from solution first.

  9. Class Example • A solution contains 1.0 x 10-2 M Ag+ and 2.0 x 10-2 M Pb2+. When Cl- is added, both AgCl (Ksp = 1.8 x 10-10) and PbCl2 (Ksp = 1.7 x 10-5) can pre. What concentration of Cl- is necessary to begin precipitation of each salt? Which salt precipitates first?

  10. Table Talk • A solutions consists of 0.050 M Mg2+ and Cu2+. Which ion precipitates first when OH- is added? What concentration of [OH-] is needed to begin to precipitation of each cation? NOTE – Ksp of Mg(OH)2 is 1.8 x 10-11 and Ksp of Cu(OH)2 is 4.8 x 10-20.

  11. Drill Baby Drill • Drill – Calculating Molar Solubilities • Drill – Predicting Precipitation • Integrated Practice – Connecting Ksp to past Units

  12. Closing Time • Read 17.1, 17.4, 17.5, 17.6, and 17.7 • Homework: Drills and Integrated Practice • Exam Debrief – Thursday or Friday 3:30 – 4

More Related