1. Acids and Bases 1) Properties and examples 2) Theories 3) pH scale
4) Indicators
5) Neutralization
6) Molarity

2. Acids Properties and Examples
1) Have a sour taste
2) React with metals
3) Contain Hydrogen
4) Formed from non metals

3. Acids Properties and Examples
5) Form hydronium ions in water (H3O+)
6) Poisonous and corrosive to the skin
7) Conducts electricity in water (electrolytes)

4. Acids (cont.)
8) Forms ionic bonds
9) Turns blue litmus paper red

5. EXAMPLES acetic acid - vinegar (from grapes and apples)
lactic acid - milk, butter milk, sour cream

6. EXAMPLES citric acid - citrus fruits
hydrochloric acid- muratic, cleaning, stomach acid

7. Acids (cont.)
nitric acid - a dehydrator, turns skin yellow

8. Acids (cont.) sulfuric acid - battery acid, dehydrator
The number one chemical produced in the US. More sulfuric acid is produced than any other compound.

9. Bases Properties and Examples
1) Taste bitter
2) Feel slippery
3) Poisonous and corrosive to the skin

10. Bases Properties and Examples
4) Contains a metal, hydrogen and oxygen (except for ammonia NH3 )
5) Forms the OH- ion (hydroxide) in water
6) conducts electricity (electrolyte) in water

11. Bases (cont.) 7) Dissolves oils and fats 8) forms ionic bonds
9) Turns red litmus paper blue

12. EXAMPLES
sodium hydroxide - lye, drain cleaner, used to make soap, hair treatment
calcium hydroxide - tums antacid
aluminum hydroxide -antiperspirant, Rolaids antacid

13. Acid-Base Theories Arrhenius acid = releases H+ ions in water
base = releases OH- ions in water
Bronsted / Lowery
acid = proton donor H+
base = proton acceptor
Lewis (organic acids and bases)
acid = electron pair acceptor
base = electron pair donor

14. Conjugate Acids and bases
HCl + NaOH <=> NaCl H+ (OH-)
acid base con. base con. acid
conjugate acids = product side, contains the proton from the acid and the (-) part of the base.
conjugate base = product side, contains the (+) part of the base and the (-) part of the acid.

15. Neutralization
When an acid reacts with a base a salt and water is formed. The salt is the CB and the water is the CA.
HCl + KOH <=> H(OH) + KCl
A B water salt
salts are not always NaCl

16. Anhydrides
Basic anhydrides = are formed when water is removed from a base
Acidic anhydrides = are formed when water is removed from an acid
The problem of acid rain is a result of acidic anhydrides being formed when high sulfur coal is burned. The anhydrides combine to form sulfuric acid.

17. Indicators
Are weak acids that will turn different colors in acid and base solutions.
Examples
Litmus: red turns blue in a base
blue turns red in an acid
Phenolpthalein: clear in an acid / red in a base
Methyl Orange: turns red to yellow in a pH range of 3.1 to 4.4
Red Cabbage: variety of colors from acids to bases

18. pH scale pH is the measurement of the number of H3O+
ions in a solution.
Distilled water has 1 x H3O+ ions.
Using the -log the pH = 7
pH range
1………....…...…6.9…....7…...7.1……………
acid neutral base

19. Common Substances Stomach acid = 1.6 vinegar = 2.8 apples =3.0
orange juice = 3.5
carrots = 5.0
urine = 6.0
milk = 6.5
blood = 7.35
sea water = 8.4
milk of magnesia antacid = 10.5

20. Titration
In the reaction of an acid with a base an indicator is used to detect the pH change.
By carefully measuring the amount of acid or base used to cause the color change we can tell the number of moles used.
Then a mass:mass problem can be used to determine the amount of the unknown compound.

21. Molarity solute = what gets dissolved
solvent = what does the dissolving
moles of solute / 1 liter of solvent
grams / 1000 ml

22. ACID BASE STRENGTH STRONG ACIDS H2(SO4) H(ClO4) H(NO3) HBr HI HCl
WEAK ACIDS
H3(PO4) H2(CO3)
CH3COOH H2S
STRONG BASES
Ca(OH)2 Sr(OH)2
Ba(OH)2 Na(OH)
K(OH) Rb(OH)
Cs(OH) Mg(OH)2
WEAK BASES
NH3