Chem_208_18_07_web - 1. Before addition of NaOH: 2. 10.0 ml...

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1 Today: Finishing 17.4 (Skip Polyprotic acids), Starting Ch. 18 Skip Sections 17.5, 17.6 Next week: Completing Ch. 18 PS7 due tomorrow: NOTE: PKa = 9.3 for phenolphthalein Prelim 2: Tues. Apr. 10, 7:30-9:00 PM, 15- Equilibrium 16- Acids/Bases 17- Buffers/Indicators/Titrations 18- Solubility and Complex-Ion Equil. Problem Sets 5 - 8
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2 Titration of a weak acid using NaOH pH > 7 at equivalence point (moles base = moles acid) Good indicator choice (Equiv. pt. = Endpoint) Poor indicator choice (Endpoint reached BEFORE equiv. pt) Titration of 25.0 ml of 0.100 M Acetic Acid
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3 Titrate 50.0 ml of 0.200M Lactic Acid (pKa = 3.86) with 0.200M NaOH Calculate pH after addition of the following:
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Unformatted text preview: 1. Before addition of NaOH: 2. 10.0 ml NaOH: 3. 25.0 ml NaOH: 4. 49.0 ml NaOH: 5. 50.0 ml NaOH: 6. 51.0 ml NaOH: pH = 2.27 pH = 3.26 pH = 3.86 (pH = pK a halfway to equiv. pt) pH = 5.55 pH = 8.43 (equiv. point) pH = 11.30 4 18. Solubility and Complex Ion Equilibria Solubility Product, K sp :-Equilibrium constant for ions in saturated aqueous solution. e.g., For Mg(OH) 2 (s) Mg 2+ (aq) + 2OH-(aq) K sp = [Mg 2+ ][OH-] 2 = 1.8 x 10-11 What is the solubility of Mg(OH) 2 in water, in mol/L and g/L? What is the molar solubility of Mg(OH) 2 in 0.010M NaOH? 1.7 x 10-4 M; 9.6 mg/L 1.8 x 10-7 M...
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This note was uploaded on 05/18/2008 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell University (Engineering School).

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Chem_208_18_07_web - 1. Before addition of NaOH: 2. 10.0 ml...

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