1. Acid-Base Titrations
progressive addition of one reactant to another in measured volumes until an endpoint is reached.
equivalence point (mL) is when the mole ratio is exactly satisfied, volume used for stoichiometry
is shown by an indicator which changes color at the endpoint (pH)

2. Buffering: area where the pH is constant/little change even thought the titrant is being added.

3. Titration of Sample with Titrant
pH Titration Curves
Titration of Sample with Titrant

4. A. Strong Base with a Strong Acid
Titration of NaOH with HCl
-sudden pH change, steep curve
-endpoint is at pH = 7
-H30+(aq) + OH-(aq)  H20(l)

5. B. Weak acid with a Strong Base Titration of HCN with NaOH
-less steep curve
-endpoint is pH>7,
-Ex) HCN(aq) + OH-(aq)  CN-(aq) + H20(l), CN- is a weak base so pH>7
then CN-(aq) + H20(l ) HCN(aq) + OH-(aq) , OH- increases pH

6. Titration of NH3 with HCl
C) Weak Base with a Strong Acid
Titration of NH3 with HCl
-less steep curve
-endpoint is pH<7
-Ex) NH3(aq) + H30+(aq)  NH4+(aq) + H20(l), NH4+ is a weak acid so pH<7
then NH4+(aq) + H20(l ) NH3(aq) + H30+(aq) , H30+ decreases pH

7. D. Weak Base with Weak Acid Titration of F- with HCN
-difficult to see endpoint without curve
-pH stays near 7, either acidic or basic depending on Ka/Kb
- F-(aq) + HCN (aq) HF(aq) + CN-(aq)