1. ACIDS, BASES, & SALTS

2. Acids verses Bases Properties of ACIDS: Properties of BASES:
bitter taste
classified as electrolyte
react with acids (neutralization rxn)
slippery or soapy feeling
bases turn litmus paper blue
sour taste
classified as electrolyte
react with bases (neutralization reaction)
react with most metals to produce H2(g) (SR rxn)
acids turn litmus paper red

3. Chemical Formulas Formula of Acid: Formula of Base: format: HX
where X = non-metal/poly ion
format: XCOOH
exceptions: H2O2
H2O
format: MOH
where M is metal
ex: NaOH, Ca(OH)2
exceptions: NH3
NH4+1
OH -1
Why is CH3OH NOT a base?

4. Which metals react with acids?
see Table J: all metals above H2 react with acids
undergo SR rxns (metal replaces H in acid)
Cu, Ag, and Au do NOT react with acids

5. Electrolyte
substance that dissolves in H2O to produce aqueous soln that conducts electric current
3 substances fit this description:
acids, bases and salts

6. All 3 subs dissociate (ionize) in H2O
Electrolytes
All 3 subs dissociate (ionize) in H2O
ACID: HCl(s)  H+1(aq) + Cl-1(aq)
BASE: NaOH(s)  Na+1(aq) + OH-1(aq)
SALT: NaCl(s)  Na+1(aq) + Cl-1(aq)
H2O(l)
H2O(l)
H2O(l)

7. Identify the Electrolytes
NaCl
C2H5OH
H2SO4
NaOH
C6H12O6
CaI2 HF
Mg(OH)2
C3H7OH
CCl4
HNO3
C5H12
K3PO4
CH3OCH3
LiOH HI
(NH4)2SO4
C12H22O11
Yes - salt NO NO
Yes - acid
Yes - acid NO
Yes – base & salt
Yes - salt NO NO
Yes - salt
Yes – salt & base
Yes - acid
Yes - acid
Yes – base & salt
Yes - base NO NO

8. Acid-Base Theories: Arrhenius Theory acids/bases ionize in water
based on type ions produced when acid/base mixed with water
limitations
Bronstead-Lowry Theory
aka: alternative theory
based on acid/base being proton donor/receiver
NO limitations

9. Arrhenius Acid
substance that contains hydrogen & ionizes to produce H+1 ions in (aq) soln
HCl  H+1(aq) + Cl-1(aq)
CH3COOH  H+1(aq) + CH3COO-1(aq)
H2O(l)
H2O(l)

10. Arrhenius Base
substance that contains hydroxide group & ionizes to produce OH-1 ions in (aq) soln
NaOH(s)  Na+1(aq) + OH-1(aq)
H2O(l)

11. Arrhenius Salt
electrolyte where H+1 not only (+) ion and OH-1 not only (-) ion formed in aqueous solution
ex:
CaBr2(s)  Ca+2(aq) + 2Br-1(aq)
KNO3(s)  K+1(aq) + NO3-1(aq)
H2O(l)
H2O(l)

12. Arrhenius Model has limitations
Arrhenius model ONLY applies when H2O is solvent
don’t always use H2O as solvent
doesn’t explain why NH3 (and its ion:NH4+1) are bases:
doesn’t contain OH-1
but will produce OH-1 ions in (aq) soln
NH3(g)  NH4+1(aq) + OH-1(aq)
H2O(l)

13. Alternate Theory: Bronsted-Lowry
Acid is a proton donor
all Arrhenius acids = Bronsted-Lowry Acids
H+1
HX(g) + H2O(l)  H3O+1(aq) + X-1(aq)
H+1 forms molecule-ion bond with water molecule
to form H3O+1 (hydronium ion)

14. Bronsted-Lowry Acids HCl + H2O  H3O+1 + Cl-1
H2SO4 + H2O  H3O+1 + HSO4-1
HSO4-1 + H2O  H3O+1 + SO4-2
H+1
H+1

15. Bronsted-Lowry Base bases are proton acceptors
NH3 + H2O  NH4+1 + OH-1
explains why NH3 is a base!

16. Amphoteric
substance that acts as
BOTH
an acid & a base

17. Water is amphoteric! HX(g) + H2O(l)  H3O+1 + X-1 (base)
NH3 + H2O  NH4+1 + OH-1
(acid)