1. Chapter 17
Acid-Base Titrations

2. Strong Acid- Strong Base
H+ + OH-  H2O K = 1/Kw = 1 x 1014
Note:
pH = 7 at equivalence point
pH changes rapidly near equivalence point

3. Adding acid to base:

4. Weak Acid-Strong Base
HA + OH- → A- + H2O K = 1/Kb
Running alkali into the acid
Note:
pH > 7 at equivalence point
pH changes more slowly near the eq. pt.
flat buffer region leading up to eq. pt.

5. Strong Acid- Weak Base
H+ + A-  HA K = 1/Ka
Running acid into the alkali
Note:
pH < 7 at eq. pt.
pH changes slowly near eq. pt.
buffer region leading up to eq. pt

6. Go to this link and scroll down to “explore these ideas below”
Go to this link and scroll down to “explore these ideas below”. Look at the differences between the different titration curves by turning them on and off.

7. Choice of Indicator
HIn ↔ H+ + In-
HIn and In- have different colors, the color of solution depends upon the ratio of concentrations
Ka = =
end point occurs when [H+] = Ka or when pH = pKa (of the indicator!)

8. Choose your indicator to have a pKa near the pH of the equivalence point of your acid-base reaction.

9. Take the notes quiz here.