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Summary Applications of aqueous equilibria
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Summary of 8th chapter from Chemical Principles: Zumdahl and Decoste. Notes containing key concepts from the chapter and thorough explanations of the terminology. Also includes formulas and relevant course-related information.

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  • Chapter 8
  • July 19, 2019
  • 9
  • 2018/2019
  • Summary

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Applications of Aqueous
equilibria
8.1 Solutions of Acids or Bases containing a common ion.

 The common ion is one that is being produced by a salt and an acid/base at the
same time within a solution.
 Common ion effect consists of creating stress in a reaction and changing the
equilibrium position thru the production of an ion that is product in 2 different
reactions. Such that the product from first reaction causes the second reaction to
tend backward (which has the same product), Lé Châtelier’s principle.
 Common ion effect also affects polyprotic dissociation.

8.2 Buffered Solutions

 A buffered solution is one that resists a change in pH even when either hydroxide
ions or protons are added.
 Blood is an example of a buffered solution.
 A buffered solution contains a weak acid and its salt or a weak base and its salt.




 Ka = [H+] [A-]/[HA]
 -log[H+] = -log (Ka) – log ([HA]/[A-])  Henderson Hasselbalch equation
 In buffer solutions, the pH depends upon the ratio of [HA]/[A -].
 When H+ is added to buffered solutions, it reacts essentially with weak base present.
 When OH- is added to a buffered solution, it reacts essentially with the weak acid
present.

8.3 Exact treatment of buffered solutions

, 8.4 Buffer capacity

 Buffer capacity of a buffer solution is defined as the number of protons or hydroxide
it can absorb without significant change in pH.
 The capacity of a buffer solution is determined by the magnitudes of [A -] and [HA]
 The closer the ratio of [A-] and [HA], the higher the buffering capacity of a solution.
 The pKa for the weak acid selected must be as close to the desired pH.

8.5 Titration and pH curves

 Progress of an acid-base titration is monitored by plotting pH of the solution being
analyzed as a function of amount of titrant added; such function is called a pH curve.
 Millimole is the unit used for titration calculations, equivalent to 1mol/1000
 Molarity = millimole of solute/ mL of solution
 For titration of strong acids with strong bases:
- Identify the amount of base that has reacted with H+ to produce H2O
- The remaining H+ will determine the pH.
- In case there is no more H+ and there exists an excess of OH- find the pH from
pOH or [H+] [OH-]




 In performing reactions between weak acids and strong bases, it is important to
remember that even though the acid is weak, it reacts essentially to completion with
hydroxide ion, a very strong base.




 For titration of weak acids with strong bases:
- Identify the amount of acid that has reacted with OH- to produce H2O, through
stoichiometry.
- The remaining acid will dissociate and produce H+, which will be used to find pH.

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