1Week 11 CHEM 1310 - Sections L and M 1Ch 8 - Applications of Equilibrium 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations and pH Curves 8.6 Acid-Base Indicators 8.8 Solubility Product Sections to Skip: 8.3, 8.7, 8.9, and 8.10Week 11 CHEM 1310 - Sections L and M 2Making a Buffer How would you prepare 1 L of buffer at pH5?Week 11 CHEM 1310 - Sections L and M 3Buffer Capacity Buffer capacity is the amount of protons orhydroxide ions that can be absorbed without asignificant change in pH.Buffering Regionlittle to no changein pH with large additions of basenbase = nacid2Week 11 CHEM 1310 - Sections L and M 4pH Titration Controlled addition of a “titrant” ofknown concentration to a solutionof unknown concentration Reaction characteristics Acid-Base Complete reactivity (no sidereactions) Color change given by an indicatorWeek 11 CHEM 1310 - Sections L and M 5pH Titration Controlled addition of a “titrant” ofknown concentration to a solutionof unknown concentration Reaction characteristics Acid-Base Complete reactivity (no sidereactions) Color change given by an indicatorWeek 11 CHEM 1310 - Sections L and M 6pH TitrationMeniscusRead a buret using the levelof the meniscusIndicatorPhenolphthaleinAt pH <7: ColorlessAt pH = 7: PINK(Endpoint)3Week 11 CHEM 1310 - Sections L and M 7pH Titrationsnbase = nacid Endpoint of a titration = equivalence pointWeek 11 CHEM 1310 - Sections L and M 8Titration Problem It takes 37.65 mL of an NaOH solution totitrate 0.6135 g of dissolved potassiumhydrogen phthalate (weak acid) to thephenolphthalein endpoint.What is the molar [NaOH]?Solve on boardWeek 11 CHEM 1310 - Sections L and M 9Review Acid-Base Equilibria Ka for acids or Kb for bases Complex Ion Solutions Buffers pH Titrations Dissolution-Precipitation Equilibria Ksp for “solubility product”
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