CHEM 1120 1nd Edition Lecture 17 Outline of Last Lecture I Titrations a Variables that determine features of a titration curve b Weak acid strong base titration curve c Diprotic Acids d Acid base indicators Outline of Current Lecture I Titrations a Acid Base indicators II Solubility Equilibria a Ksp III Factors affecting solubility a Common ion effect b pH c Complex ion formation d Amphoterism IV Precipitation and Separation of Ions Current Lecture I II III Titrations a Acid Base Indicators a weak acid or weak base whose color differs in acidic and basic solutions i Still satisfies Henderson Hasselbalch equation ii Choosing an indicator pH pKa 1 acid color observed 1 pH pKa 1 base color is observed 2 A titration s endpoint occurs when the indicator changes color Solubility Equilibria a Ksp solubility product b Solubility grams of solute dissolved in one liter of saturated solution i C c x D d c Molar solubility moles of solute dissolved in one liter of saturated solution Factors Affecting Solubility a Common ion effect i Add common ion lowers solubility These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute b pH IV V i If a substance has a basic anion it will be more soluble in an acidic solution ii Use Le Chatliers principle iii Acidic salt increase pH to increase solubility iv c Complex Ion Formation i Complex ion a species containing a central metal ion Lewis acid bonded to one or more molecules or ions Lewis base ii Kf formation constant products reactants iii Combine 2 reactions do ICE table on combined reaction iv Multiply Ks and Kf because you added reactions d Amphoterism i Amphoteric referring to a substance that will react with both acids and bases ii Metal oxides and hydroxides Precipitation and Separation of Ions a Do example in slide show Start Chapter 22 Chemistry of the Nonmetals
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