1. Modern Chemistry Chapter 15 Acid-Base Titration & pH

2. Section 1
self-ionization of water occurs when two water molecules produce a hydronium (H3O+) and a hydroxide (OH-) ion
2 H2O  H3O+ + OH-
The ionization constant (Kw) of water is: Kw = [H3O+] [OH-] = 1.0 x M

3. Acidic, Basic, & Neutral IF [H3O+] > [OH-] then solution is acidic.
IF [H3O+] < [OH-] then solution is basic.
IF [H3O+] = [OH-] then solution is neutral.

4. Calculating [H3O+] & [OH-]
Since the product of the hydronium and hydroxide ion concentrations is a constant, we can use the following formula to determine these concentrations.
[H3O+] [OH-] = 1.0 x M
Use this formula to answer problems #1-4 on page 502 of the textbook.

5. The pH Scale
The pH of a solution is defined as the negative of the common logarithm of the hydronium ion concentration, [H3O+].
pH = -log [H3O+]
The pOH of a solution is defined as the negative of the common logarithm of the hydroxide ion concentration, [OH-].
pOH = -log [OH-]

6. pH & pOH pH + pOH = 14 so 14 – pH = pOH and 14 – pOH = pH
See figure 3 on page on page 503.
See table 3 on page 504.
See table 4 on page 504.
Do problem #1 on page 505.
Do problems #1-4 on page 506.
Do problems #1-4 on page 508.

7. Cross-Disciplinary Connection
Read the Cross-Disciplinary Connection titled “Liming Streams” on page 510.
Answer both questions at the end of the article.

8. Section 2 Determining pH and Titrations
acid-base indicators are compounds whose colors are sensitive to pH
transition interval is the pH range over which an indicator changes color
a pH meter determines the pH of a solution by measuring the voltage between two electrodes placed in a solution.

9. Titration
titration is the controlled addition and measurement of the amount of a solution of a known concentration required to react completely with a measured amount of solution of an unknown concentration
equivalence point is the point at which the two solutions used in a titration are present in chemically equivalent amounts
endpoint is the point in a titration at which the indicator changes color
standard solution is the solution that contains a precisely known concentration of solute

10. Titration see figure 10 on pages 518-519 for the steps of a titration
A general equation for the solution of titration problems would be
VaMaeqa = VbMbeqb
Va = volume of acid Vb = volume of base
Ma = molarity of acid Mb = molarity of base
eqa = #H in formula of acid eqb = #OH in formula of base

11. Titration Do practice problems #1-2 on page 521.
Do section review problems #1-2 on page 521.
Do chapter review problems #6, 8, 9, 12, 13, 24, 25, & 26 on pages

12. Modern Chemistry Chapter 15 Test Review
25 multiple choice
definition of self-ionization
[H3O+] [OH-] = 1 x 10-14
definition and formula for calculating pH = -log[H3O+]
pH >7 is a base; pH <7 is an acid; pH = 7 is neutral
pH range is normally 0 to 14
calculate pH from [H3O+]
calculate [H3O+] from pH
definitions of indicators, transition interval, titration, neutralization, endpoint, standard solution
acid-base titration monitors pH
titration problems using VaMaeqa = VbMbeqb