Acid/Base Titration Curves

Table XXIV. Formulas for Calculating Titration Data, pH vs. mL of Reagent

1

Substance TitratedV0 ml. of Solution
M0 its Molarity

2

Initial [H+] or [OH-]

3

Intermediate Points 10, 50, 90, etc. Percent Neutralized,
V1 ml. of Reagent of
M1 Molarity Added

4

Equivalence Point

5

Excess of Reagent
V1 Volume Reagent
M1 its Molarity
VT Total Volume

(1) Strong Acid[H+]=M0
(2) Strong Base[OH-]=M0
(3) Weak Acid (Ka=10-5 to 10-8)

(Value in Column 4 to be added)
(4) Weak Base (Kb=10-5 to 10-8)

(Value in Column 4 to be added)
(5) Salt of Very Weak Acid (e.g. KCN)

(Correct for value in Column 4)
(6) Salt of Very Weak Base

(Add to [OH-] found in Column 4)


pH vs. mL of 0.1 N NaOH in the Titration of 25 mL. of 0.1 N of HCl.
the shaded blocks show the transition ranges of the indicators.

Strong Acid/Strong Base


Graphs showing the course of pH vs.mL of 0.1 N NaOH in the titration of 25 mL portions of various acids of the Ka values indicated (10-4, 10-5, 10-6, etc.).

Weak Acid/Strong Base


Graphs showing the course of pH vs. mL of 0.1 N HCl in the titration of 25 mL portions of bases of Kb 10-5, 10-7, 10-9.

Strong Acid/Weak Base


The course of pH during the titration of 30 mL of 0.1 Molar phosphoric acid with 0.1 N sodium hydroxide.

Polyprotic Acid/Strong Base