This document defines acids and bases and their key characteristics. Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases fully dissociate in water, while weak ones only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. When acids and bases react, they undergo a neutralization reaction where water and a salt are formed. Indicators are used to test whether a solution is acidic or basic. The pH scale measures the concentration of H+ ions, with lower pH indicating more H+ ions and higher pH less H+ ions.

1. Brainpop~Acids and Bases

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

3. 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)
Strong Acids The Formula
Sulphuric acid
Hydrochloric acid
Hybrobromic acid
Hydroiodic acid
Nitric acid
Perchloric acid
H2
SO4
HCl
HBr
HI
HNO3
HClO4
Acetic acid (vinegar) HC2H3O2
Carbonic acid HCO3
Weak Acid The Formula

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

8. 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. 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
Common Bases:
(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 → H2O + Salt
“Salt” means any ionic
compound formed from
an acid/base reaction
NOT JUST
NaCl !!
Neutralization Reaction Animation

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

14. Neutralization
Another Example
HNO3 + KOH → H2O + KNO3
H OHKNO3
acid base water salt

15. Indicators
An indicator is a compound
that will change color in the
presence of an acid or base
Universal indicator (pH paper)
Used for the full pH range
Red Litmus-Turns blue in base
Blue Litmus-Turns red in acid
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. pH Scale
Shows the range of H+
concentrations
High H+ concentration Low H+ concentration