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Lecture Comments (1)

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Post by Deborah Walters on July 20, 2009

what if the problem is this:

The equation for the reaction between Al(s) and Pb+2(aq) is:_____

2Al(s) + 3Pb+2(aq) 2 Al+3(aq) + 3Pb(s) .

Therefore, for each 2 moles of Al(s) that are used, how many moles of Pb(s) are formed?

From the moles of Al(s) consumed, 0.011 moles, calculate the number of moles of Pb(s) that should have been formed:_____moles.

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Solubility Product Constant, Precipitation

  • Apply equilibrium law to solutions of slightly soluble salts; Ksp solubility product constant

  • Do calculations of solubility from Ksp and vice-versa

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Solubility Product Constant, Precipitation

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Equilibrium in Saturated Salt Solution 1:12
    • Example: Silver Chloride
    • Ksp (Solubility Product Constant)
  • Solubility Product Constant 6:19
    • Example : Lead Iodide
  • Limitations of the Solubility Product 9:06
    • Low Solubility
    • Complexes that are Soluble
  • Ksp Values and Ion Concentrations 13:28
    • Example: Silver Chloride
    • Example: Lead Chloride
  • Precipitation of Salts 23:56
    • Example: Silver Bromide and Copper Bromide
  • Common Ion Effect 31:52
    • Example: Lead Sulfate
    • Le Chatelier's Principle
  • Common Ion Solubility 42:37
    • Example: Lead Chloride in Sodium Chloride Solution
  • Acids, Bases, and Solubility Equilibria 48:32
    • Example: Lead Carbonate
    • Lle Chatelier's Principle
  • Group Separation and Qualitative Analysis of Metal Ions 55:09
    • Examples
  • Additional Example 1