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Ch. 10: Acid-Base Titrations

Ch. 10: Acid-Base TitrationsOutline: 10-1 Titration of Strong Base with Strong acid 10-2 Titration of Weak acid with Strong Base 10-3 Titration of Weak Base with Strong acid 10-4 Titrations in Diprotic Systems 10-5 Finding the End Point with a pH Electrode 10-6 Finding the End Point with Indicators 10-7 Practical Notes 10-9 The Levelling EffectUpdated Oct. 31, 2011: minor edits: 2, 5; new slides 22-27 Strong acid -Strong Base TitrationsEach type of titration:1. Write the involved chemical Measure pH values with a pH electrode (or sometimes an indicator).3. Construct a pH , Titration of mL of M KOH with M HBr. The equilibrium is:H++OH- H2O, Kw=1014meaning any amount of H+ which is added will be consumed by OH- stoichiometrically, until all of the OH- is consumed (after which H+ is in excess).What volume of HBr, (Ve) is needed to reach the equivalence point?Ve = mL, which means that after mL of HBr solution has been added, the titration is Prior to : OH- in At the : H+ and OH- react completely, pH dependent upon water After the : H+ in XSEquivalence point vs.

Titration: Weak Acid with Strong Base We will consider the titration of 50.00 mL of 0.02000 M MES with 0.1000 M NaOH. MES is an abbreviation for 2-(N-morpholino)ethanesulfonic acid, which is a weak acid with pKa = 6.27. This the reverse of the Kb reaction for the base A−.Therefore, the equilibrium constant for is K = 1/Kb = 1/(Kw/Ka (for HA)) = 5.4 × 107.

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