Chem_215_Lecture_13_color - Titrations Three Possibilities:...

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1 Titrations 1. Strong acid + strong base - pH determined by excess acid or base. - No equlibrium constants needed for calculations 2. Weak acid with strong base: - Text: Acetic acid with NaOH - Lecture: Lactic acid with NaOH 3. Weak base with strong acid: - PS 5: NH 3 with HCl Three Possibilities:
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2 Titrate 100.0 ml of 0.100M HNO 3 with 0.200M Ba(OH) 2 Calculate pH after addition of the following: 1. No Ba(OH) 2 : 2. 10.00 ml Ba(OH) 2 : 3. 24.00 ml Ba(OH) 2 : 4. 25.00 ml Ba (OH) 2 : 5. 25.05 ml Ba (OH) 2 : 6. 35.00 ml Ba(OH) 2 : pH = 1.00 pH = 1.26 pH = 2.49 pH = 7.00 pH = 10.20 pH = 12.47
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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: 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:
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4 Shapes of Titration Curves depend upon Ka Titration of 50.0 mL of 0.10 M Acid
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5 Titrations of Polyprotic Acids, e.g., H 3 PO 4 Ka 1 = 7.5 x 10 -3 , Ka 2 = 6.2 x 10 -8 ; Ka 3 = 4.8 x 10 -13
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Chem_215_Lecture_13_color - Titrations Three Possibilities:...

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