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Chapter 17

Chapter 17. Solubility Equilibrium. Solubility Equilibrium AgCl (s) ↔ Ag + (aq) + Cl - (aq) Ksp = [Ag + ][Cl - ] PbCl 2(s) ↔ Pb 2+ (aq) + 2 Cl - (aq) Ksp = [Pb 2+ ][Cl - ] 2. Watch this solubility animation . Also look through the notes and problems underneath the animation.

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Chapter 17

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  1. Chapter 17 Solubility Equilibrium

  2. Solubility Equilibrium AgCl(s) ↔ Ag+(aq) + Cl-(aq) Ksp = [Ag+][Cl-] PbCl2(s) ↔ Pb2+(aq) + 2 Cl-(aq) Ksp = [Pb2+][Cl-]2

  3. Watch this solubility animation. Also look through the notes and problems underneath the animation. http://www.kentchemistry.com/links/Kinetics/Ksp.htm

  4. Uses of Ksp: 1. Calculation of concentration of one ion, knowing the concentration of the other. Ex What is [Pb2+] in a solution in equilibrium with PbCl2 (Ksp = 1.7 x 10-5) if [Cl-] = 0.020 M?

  5. 2. Determination of whether a precipitate will form If P < Ksp, no ppt. If P > Ksp, ppt. forms until P = Ksp (P is the same as Q was for Kp and Kc equilibrium) ex Suppose enough Ag+ is added to a solution 0.001 M in CrO42- to make an Ag+ concentration of 0.001 M. Will silver chromate precipitate?

  6. 3. Determination of Solubility a. In pure water: Ex What is the solubility of PbCl2 in pure water?

  7. b. In solubility containing a common ion. Ex What is the solubility of PbCl2 in 0.100 M HCl?

  8. Take quiz here https://docs.google.com/spreadsheet/embeddedform?formkey=dDlHOWdIc2xPTGF2NUxlT3BESlZSNkE6MQ

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