1. Acids, Bases
& Salts

2. Naming Acids Binary acids Ternary acids
Hydro(first syllable of element)ic acid
Ternary acids
Replace PAI suffix –ate with –ic
Replace PAI suffix –ite with –ous

3. Name that Acid HF HBr HNO3 H2SO4 H3PO4 CH3COOH
We will work mainly with the
–ic acids, but you should know that the others exist.

4. Definitions of Acids Brønsted-Lowry Acids Arrhenius Acids
Ionize to form H+ in water
Brønsted-Lowry Acids
Proton donor
HCl + H2O  H3O+ (aq) + Cl- (aq)

5. ?
water
hydrogen ion
“proton”
hydronium ion

6. Ionization of Acids H3PO4 + H2O 3 3H3O+(aq) + PO4-3(aq)
CH3COOH + H2O
H3O+(aq) + CH3COO-(aq)
H3PO4 + H2O
H3O+(aq) + PO4-3(aq)
1 H+ = Monoprotic
2 H+ = Diprotic
3 H+ = Triprotic

7. H2CO3 KH CH3OH KI Acid? Yes or No An Acid must ionize
with H+ as the only
positive ion in soln
H2CO3 KH
CH3OH KI

8. Acids are electrolytes
…because they ionize in water
The more ions, the stronger the electrolyte
Strong acids completely ionize
Form lots of ions
Weaker acids do not

9. Acid dissociation constantKa
Acid dissociation constant
Stronger acids
larger Ka

10. . . . Other Acid Characteristics
Acids change the colors of indicators
blue litmus changes to red
pH < 7 can be neutralized by bases
Dilute acids taste sour

11. Characteristics of Bases
Arrhenius Base
Defined as a substance that provides OH- ions to solution
BrØnsted-Lowry Base
proton acceptor
Ex: NH3 + H2O  NH4+ + OH-

12. all bases end in hydroxide
Naming Bases
Name the ca+ion
all bases end in hydroxide
KOH
Mg(OH)2
NH4OH
Exception?

13. NaOH  Na+ + OH - NH4OH  NH4+ + OH - Base ionization Metal ion
Group 1 hydroxides are your strongest bases.
Polyatomic Ion
NH4OH  NH4+ + OH -

14. Change the colors of indicators
Bases never contain carbon
Feel Slippery
ex. soap
Taste bitter
Change the colors of indicators
Phenolphthalein
Red litmus turns blue
pH > 7 can be neutralized by acids

15. THE END