WebLecture: Common Ions
Kotz and Triechel, Chemistry and Chemical Reactivity Chapter 17: Sections 5-7.
- 17.5 We can now define a new "special value" for Q. The value of Q at the point at which a reaction reaches saturation is the solubility equilibrium constant Ksp. If Q < Ksp, the solution is not yet saturated. If Q > Ksp, the solution is supersaturated and will precipitate. We can use the relationship between Q (the quotient at an time) and Ksp to predict the outcome of a reaction.
- 17.6 When complex ions are involved in a solution equation, the formation of the ion can be identified by yet another "special Q", Kf, the equilibrium constant for the formation of the ligand bonds with the metal ion.
- 17.7 The relationship of solubility and formation constants determine whether a solid will dissociate in a given solvent. The small solubility value of a solute in water indicates that it does not dissolve, but if one of the solute components will form a complex ion with another molecule, the solute will dissolve in a solvent containing that moleucule.
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Videos for Chapter 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibri
Review the Videos at Thinkwell Video Lessons.
- Under "EQUILIBRIUM IN AQUEOUS SOLUTIONS"
Homework problems: See your Moodle assignment!
AP #14 GUIDED INQUIRY — Creating an effective buffer solution — Phase III
Complete your data analysis and file your formal report.
- APGIE Investigation 16 Buffer Design: The Preparation and Testing of an Effective Buffer: How Do Components influence a Buffer’s pH and Capacity?
- IGHCE Lab 13.2 Quantify the common ion effect
- There is no alternate form for this lab
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