1. Properties of Acids and Bases
2. Hydrogen Ions from Water
3. The pH Concept
4. Calculating pH Values
5. Arrhenius Acids and Bases
6. Bronstead-Lowry Acids and Bases
7. Lewis Acids and Bases
8. The Strengths of Acids and Bases [Practice ]
9. Calculating Dissociation Constants

Chapter 17

17-1 Properties of Acids and Bases

- Acids are sour; bases are bitter.

17-2 Hydrogen Ions from Water

- Hydroxide ion = OH^(-)

- Hydronium ion = H3O^(+). This is, for most purposes, the same as a H^(+) ion.

- Self-ionization of water: H2O <===> H^(+) + OH^(-)

- K(w) = 10^(-14)

17-3 The pH concept

- pH = -log[ H^(+) ]

17-4 Calculating pH Values

- Note: if x = log y then 10^x = y

17-5 Arrhenius Acids and Bases

- Arrhenius: acids yield H^(+) when dissolved, bases yield OH^(-) when dissolved.

17-6 Bronsted-Lowry Acids and Bases

- Bronsted-Lowry: acids give a H^(+), bases receive a H^(+).

17-7 Lewis Acids and Bases

- Lewis: acids accept electron-pairs, bases provide an electron-pair.

17-8 The Strengths of Acids and Bases [Practice]

- Strong acids ionize completely in water.

- Acid dissociation constant (K(a)):

 K(a) = [ H^(+) ] x [anion]
                      [acid]

- Bases ionize completely in water.

- Base dissociation constant (K(b)):

 K(a) = [cation] x [ OH^(-) ]
                       [base]

17-9 Calculating Dissociation Constants

- Can be done for weak acids.

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