1. ACIDS, BASES, & SALTS

2. Properties of Acids 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. Formula of Acid format: HX where X = nonmetal (F, Cl, Br, I) or
X = negative polyatomic ion
some acids have 2 or 3 H’s
ex: HF, H2S, H3PO4
exceptions: H2O2 and H2O

4. Properties of Bases bitter taste slippery or soapy feeling
classified as electrolyte
react with acids (neutralization rxn)
bases turn litmus paper blue

5. Formula of Base format: MOH where M is metal CH3OH is NOT a base WHY?
ex: NaOH, Ca(OH)2
exceptions: NH3 and NH4+1
CH3OH is NOT a base
WHY?

6. Electrolyte
substance that dissolves in H2O to produce aqueous soln that conducts electric current

7. 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)

8. 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
Yes - salt NO NO
Yes - salt
Yes - base
Yes - acid
Yes - acid
Yes - base
Yes - base NO NO

9. Which metals react with acids?
See Table J
All metals above H2 react with acids
Cu, Ag, and Au do NOT react with acids

10. 2HCl + Mg
 MgCl2 + H2
Mg above H2 so reaction proceeds
single replacement reaction occurs

11. Arrhenius Acid
substance that contains hydrogen & ionizes to produce H+1 ions in (aq) soln
HCl + H2O(l)  H+1(aq) + Cl-1(aq)
HNO3 + H2O(l)  H+1(aq) + NO3-1(aq)

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

13. 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)

14. Arrhenius Model has limitations
don’t always use H2O as solvent
Arrhenius model only applies when H2O is solvent
doesn’t explain why NH3 is base:
doesn’t contain OH-1
but produces OH-1 ions in soln
NH3(g)  NH4+1(aq) + OH-1(aq)

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

16. Bronsted-Lowry Acids HCl + H2O  H3O+1 + Cl-1
HNO3 + H2O  H3O+1 + NO3-1
H2SO4 + H2O  H3O+1 + HSO4-1
HSO4-1 + H2O  H3O+1 + SO4-2
H+1
H+1
H+1

17. Bronsted-Lowry Base bases are proton acceptors OH-1 is base
H+1 + OH-1  H2O
not restricted to aqueous solution
NH3 + H2O  NH4+1 + OH-1
NH3 is a base!

18. Bronsted-Lowry Acids & Bases

19. water: self-ionization
H2O(l) + H2O(l)  H3O+1(aq) + OH-1(aq)
H3O+1 = hydronium ion
OH-1 = hydroxide ion OR
H2O(l)  H+1(aq) + OH-1(aq)
H+1 :hydrogen ion = proton
H+1 & H3O+1 used interchangeably

20. self-ionization of water
H2O (l) + H2O (l)  H3O+1 (aq) +OH-1(aq)

21. Acid, Base, or Neutral? all H2O contains some H+1 and some OH-1 ions
pure H2O: concentrations very low
neutral solution: [H+1] = [OH-1]
acidic solution: H+1 > OH-1
basic solution: OH-1 > H+1

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

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