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Titration - Titrant usually a solution of known composition...

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1 Titrant: usually a solution of known composition or concentration Analyate: usually a solution of unknown composition or concentration 2 4 6 8 10 12 0 10 20 30 Volume of Base Titrant Added (mL) pH Titration Curve pH Run 2 pH Run 1 pK a Half-Titration Stoichiometric Point A C B X Y pH Buffering Region pKa ± 1 Typical titration of Acetic acid (weak acid) analyate with NaOH (strong base) titrant
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2 Titration: Mechanics of Calculations Titrate 100. mL of 0.181 M HOAc with 0.150 M KOH Examine pH at FOUR points: 1. Initial pH; 2. Any Intermediate point; 3. Half-Way point (“Half-Titration”); and 4. Stoichiometric point
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3 Titration: Initial pH No base added yet; pH calculation as usual! HOAc (aq) + H 2 O (l) H 3 O + ( aq ) + OAc ( aq ) I 0.181 M 0 0 x + x + x Eq. 0..181– x x x K a = x ( ) x ( ) 0.181 ( ) = 1.8 ! 10 " 5 x = 1.80 ! 10 " 3 M pH = 2.74 Titration: Intermediate points Determine pH after 5.00 mL of KOH has been added: Since a reaction has occurred we must now calculate the following: a) How much acid (HOAc) was used up; b) How much conjugate base (OAc - ) has been made; and c)
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