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AP Chemistry Unit 11 – Additional Equilibrium Topics

AP Chemistry Unit 11 – Additional Equilibrium Topics. Lesson 6 – Precipitation Book Section: 17.6. Mixing Solutions and K sp. Concentrations of ions after solutions are mixed will allow us to determine whether or not a compound will precipitate.

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AP Chemistry Unit 11 – Additional Equilibrium Topics

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  1. AP ChemistryUnit 11 – Additional Equilibrium Topics Lesson 6 – Precipitation Book Section: 17.6

  2. Mixing Solutions and Ksp • Concentrations of ions after solutions are mixed will allow us to determine whether or not a compound will precipitate. • Remember the concept of Q (reaction quotient) – equilibrium constant at non-equilibrium conditions • If Q > Ksp, precipitation occurs until Q = Ksp • Q = Ksp, saturated solution • Q < Ksp, solid dissolves until Q = Ksp

  3. Sample Problem • Will a precipitate form when 0.10 L of 8.0 x 10-3M Pb(NO3)2 is added to 0.40 L of 5.0 x 10-3 M Na2SO4? • Ksp = 6.3 x 10-7 for PbSO4

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

  5. Homework: 17.64, 66, 68 • Wednesday: Begin Unit 12: Electrochemistry – Balancing Redox Reactions in Acids & Bases (20.1-20.2) • Thursday: Voltaic Cells (20.3) • Friday: Additional Equilibrium Topics Exam • Determining an Equilibrium Constant With a Spectrophotometer

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