CHEM 1120 1nd Edition Lecture 17 Outline of Last Lecture I. Titrationsa. Variables that determine features of a titration curveb. Weak acid-strong base titration curvec. Diprotic Acidsd. Acid-base indicatorsOutline of Current Lecture I. Titrationsa. Acid-Base indicatorsII. Solubility Equilibriaa. KspIII. Factors affecting solubilitya. Common ion effectb. pHc. Complex ion formationd. Amphoterism IV. Precipitation and Separation of IonsCurrent LectureI. Titrationsa. Acid-Base Indicators: a weak acid or weak base whose color differs in acidic and basic solutionsi. Still satisfies Henderson-Hasselbalch equationii. Choosing an indicator: pH < pKa – 1 acid color observed1. pH > pKa +1 – base color is observed2. A titration’s endpoint occurs when the indicator changes colorII. Solubility Equilibriaa. Ksp = solubility productb. Solubility: grams of solute dissolved in one liter of saturated solutioni. [C]^c x [D]^dc. Molar solubility: moles of solute dissolved in one liter of saturated solutionIII. Factors Affecting Solubilitya. Common ion effecti. Add common ion, lowers solubilityThese 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. pHi. If a substance has a basic anion, it will be more soluble in an acidic solutionii. Use Le Chatliers principleiii. Acidic salt increase pH to increase solubilityiv.c. Complex Ion Formationi. 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 reactioniv. Multiply Ks and Kf because you added reactionsd. Amphoterism i. Amphoteric: referring to a substance that will react with both acids and bases ii. Metal oxides and hydroxidesIV. Precipitation and Separation of Ionsa. Do example in slide showV. Start Chapter 22: Chemistry of the
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