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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
Use Ksp to determine if salts precipitate at given conditions
Common ion effect: adding an ion present in salt will reduce its solubility greatly
Study effects of acids and bases on solubility equilibria
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
- Equilibrium in Saturated Salt Solution
- Solubility Product Constant
- Limitations of the Solubility Product
- Ksp Values and Ion Concentrations
- Precipitation of Salts
- Common Ion Effect
- Common Ion Solubility
- Acids, Bases, and Solubility Equilibria
- Group Separation and Qualitative Analysis of Metal Ions
- Additional Example 1































0 answers
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.