1. Acids
and Salts
Bases
Brainpop~Acids and Bases

2. A substance that releases H+ ions in an aqueous solution
Acid:
A substance that releases H+ ions in an aqueous solution
“aqueous” means: water

3. H Characteristics of Acids: Acids have a sour taste
Acids react with metals
Acids contain Hydrogen
Many are poisonous and corrosive to skin H

4. Strong Acids
(break down completely to give off many H+ ions)

5. Weak Acids (only partially breaks down, gives less H+)
Mark Bishop Acid animation

6. Common Acids: All others considered Weak (examples) Sulphuric acid
Strong Acids
The Formula
Sulphuric acid
Hydrochloric acid
Hybrobromic acid
Hydroiodic acid
Nitric acid
Perchloric acid
H2SO4
HCl
HBr HI
HNO3
HClO4
All others considered Weak (examples)
Weak Acid The Formula
Acetic acid (vinegar) HC2H3O2
Carbonic acid HCO3

7. Base:
A substance that releases OH- ions in an aqueous solution

8. OH- Characteristics of Bases: Bases usually taste bitter
Bases feel slippery
Bases contain hydroxide ions
STRONG bases are also poisonous and corrosive to skin
OH-

9. (Hydroxides of Group 1 and Group 2 Metals are STRONG)
Common Bases:
Strong Bases
The Formulae
Lithium hydroxide
Sodium hydroxide
Potassium hydroxide
Rubidium hydroxide
Caesium hydroxide
Barium hydroxide
Calcium hydroxide
Strontium hydroxide
LiOH
NaOH
KOH
RbOH
CsOH
Ba(OH)2
Ca(OH)2
Sr(OH)2
(Hydroxides of Group 1 and Group 2 Metals are STRONG)
All others are WEAK

10. Some bases (VERY FEW)
don’t have OH-
Most commonly:
ammonia NH3

11. Reactions between acids and bases
When and acid and a base react with each other, the characteristic properties of both are destroyed. This is called neutralization.

12. Reactions between acids and bases
General formula for acid base reaction:
Acid +
Base →
Salt
H2O +
NOT JUST
NaCl !!
“Salt” means any ionic compound formed from an acid/base reaction
Neutralization Reaction Animation

13. Neutralization
HCl + NaOH → H2O + NaCl
acid base water salt

14. Neutralization HNO3 + KOH → H2O + KNO3 H NO3 K OH Another Example
acid base water salt

15. Indicators
An indicator is a compound that will change color in the presence of an acid or base
Red Litmus-Turns blue in base
Blue Litmus-Turns red in acid
Universal indicator (pH paper) Used for the full pH range
Phenolphthalein-Turns pink in base

16. pH
pH stands for “potential hydrogen” and is a measure of how many H+ ions there are in solution.
The MORE H+ there are, the LOWER the pH will be.

17. Shows the range of H+ concentrations
pH Scale
Shows the range of H+ concentrations
High H+ concentration
Low H+ concentration