1. Describing Acids and Bases
Properties of Acids and Bases
Acids
Produce H+ ions when dissolved in water
Sour taste
Solutions are electrolytes (some strong, some weak)
React with metals to produce H2
React with a base to form water and salt
Turn litmus paper red

2. Describing Acids and Bases
Produce OH- ions when dissolved in water
Bitter taste
Feel slippery
Solutions are electrolytes (strong and weak)
React with acids to form water and a salt
Turn litmus paper blue

3. What are acids and bases?
Arrhenius Acids
Hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solutions
Arrhenius Bases
Compounds that ionize to yield hydroxide ions (OH-) in aqueous solutions

4. What are acids and bases?
Bronsted-Lowry Acid
A hydrogen-ion donor
Bronsted-Lowry Base
A hydrogen-ion acceptor

5. Describing Acids and Bases
Names and formulas of acids and bases
Acids
Acids have a hydrogen ion
The general formula for an acid is HX, where the X is a monatomic or polyatomic ion
Bases
Bases usually have an OH- ion
Ionic compounds that are bases are named like any other ionic compound
There are exceptions like ammonia which is NH3

6. Hydrogen Ions and Acidity
The pH concept
Expressing concentration in molarity is inefficient, so we use a pH scale
The scale ranges from 0 to 14
0 is very acidic, 7 is neutral, and 14 is very basic
The pH of a solution is the negative logarithm of the hydrogen-ion concentration
pH = -log [H+], [H+] = 2nd log (-) pH
The pOH of a solution equals the negative logarithm of the hydroxide-ion concentration
pOH = -log[OH-], [OH-] = 2nd log (-) pOH
pH + pOH = 14