1. Strength of Acids & Bases
Acid and base strength is measured on the pH scale:
pH ranges from 0-14 (typically)
pH less than 7 is acidic
pH greater than 7 is basic
pH equal to 7 is neutral
Stronger acid
Stronger base
See page 3 of data booklet.

2. Each decrease of 1 on the pH scale is 10x more acidic
e.g.
pH 4 is times more acidic than pH 5 10
pH 3 is times more acidic than pH 6
1000
pH 2 is times more acidic than pH 7
100000
Using your data booklet, how much more acidic are…
lemons than tomatoes?
Stomach acid than bananas?
100 x
10000 x

3. Note: Square brackets [ ] = concentration
As pH goes up, [H+] goes down
As pH goes up, [OH-] goes up
As [H+] goes up, [OH-] goes down
Refer to diagram in data booklet.

4. Naming Acids Some common acid names are in your data booklet (p. 5)
How do you name the rest?

5. Hydro, -IC or -OUS? If the anion name ends in ide:
the acid name starts with hydro and ends with ic acid.
eg: HCl:
Cl- is chloride. So HCl is hydrochloric acid.
If the anion name ends in ate:
the acid name ends with ic acid; no hydro prefix.
eg: HNO3:
NO3- is nitrate. So HNO3 is nitric acid.
If the anion name ends in ite:
the acid name ends with ous acid; no hydro prefix.
eg: HNO2:
NO2- is nitrite. So HNO2 is nitrous acid.

6. Assignment
Homework:
Workbook Pages 85 & 86