1. Acids and Bases

2. Arrhenius Acids and Bases
Arrhenius acid: Break apart (dissociate) to yield hydrogen ions (H+) in water (aqueous) solutions
HCl → H+ + Cl-
Arrhenius base: Break apart (dissociate) to yield hydroxide ions (OH-) in water (aqueous) solutions
NaOH → Na+ + OH-

3. Naming Acids and Bases Acids: Remember this chart???
Anion Ending
Acid Name
-ide
hydro-(stem)-ic acid
-ite
(stem)-ous acid
-ate
(stem)-ic acid
Bases: cation name + hydroxide

4. The pH Scale

5. The pH scale Acidic solution: pH < 7.0 Neutral solution: pH = 7.0
Basic solution: pH > 7.0
Neutral
ACIDIC
BASIC
pH =
Increasing acidity
Increasing basicity

6. [H+] = the hydrogen ion concentration IN MOLARITYpH
pH (“potential hydrogen”): a way of expressing the hydrogen ion concentration
pH = - log [H+]
[H+] = the hydrogen ion concentration IN MOLARITY
[H+] = 10-pH

7. The pH Scale - As pH increases, [H+] decreases
- As pH decreases, [H+] increases

8. Calculating pH pH [H+] Acidic Solution pH < 7.0 Neutral Solution
Basic Solution
pH > 7.0
[H+] > 1 x 10-7
[H+] = 1 x 10-7
[H+] < 1 x 10-7

9. [OH-] = the hydroxide ion concentration IN MOLARITY
pOH
Just like pH…
pOH (“potential hydroxide”): a way of expressing the hydroxide ion concentration
pOH = - log [OH-]
[OH-] = the hydroxide ion concentration IN MOLARITY
Just like [H+]:
[OH-] = 10-pOH
pH + pOH = 14

10. Bronsted-Lowry Acids and Bases
Bronsted-Lowry acid: donates a proton (H+) in solutions
Bronsted-Lowry base: accepts a proton (H+) in solutions
HNO2 + H2O ↔ NO2- + H3O+
B-L acid
B-L base

11. Conjugate Acids and Bases
Used in Bronsted-Lowry definition ONLY
Conjugate acid: the acid formed when a proton (H+) is added to the base
Conjugate base: the base formed when a proton (H+) is removed from the acid
HNO2 + H2O ↔ NO2- + H3O+
B-L acid
B-L base
Conjugate base
Conjugate acid