1. ACIDS, BASES, & SALTS

2. Properties of Acids Sour taste Electrolytes:
- aqueous solns conduct an electric current
React with bases to form water and a salt (Neutralization Reaction)
React with most metals to produce H2(g)
Acids turn litmus red

3. Electrolyte
Substance that dissolves in H2O to produce a solution that conducts an electric current
Acids, bases, & salts are electrolytes – form ions in H2O
NaCl(s)  Na+1(aq) + Cl-1(aq)

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

5. 2HCl + Mg  MgCl2 + H2
Mg above H2 so reaction proceeds
Single replacement reaction

6. Properties of Bases Bitter taste Slippery or soapy feeling
Electrolytes
React with acids to produce water and a salt
Bases turn litmus blue

7. Formulas of Acids 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

8. Formulas of Bases Format: MOH where M is a metal
Ex: NaOH, Ca(OH)2
Exception: NH3 and NH4+1
CH3OH is NOT a base. WHY?

9. 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 - S NO NO
Yes - A
Yes - A NO
Yes - B
Yes - S NO NO
Yes - S
Yes - B
Yes - A
Yes - A
Yes - B
Yes - S NO NO

10. 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

11. Water & self-ionization
H2O(l) + H2O(l)  H3O+1(aq) + OH-1(aq)
H3O+1 = hydronium ion
OH-1 = hydroxide ion
H2O(l)  H+1(aq) + OH-1(aq)
H+1 and H3O+1 used interchangeably
H+1 called proton or hydrogen ion

12. Self-ionization of water

13. Arrhenius Acid
Substance that contains hydrogen & ionizes to produce H+1 ions in aqueous solution
HCl(g)  H+1(aq) + Cl-1(aq)
HNO3  H+1(aq) + NO3-1(aq)

14. Arrhenius Base
substance that contains hydroxide group & ionizes to produce OH-1 ions in aqueous solution
NaOH(s)  Na+1(aq) + OH-1(aq)

15. Arrhenius Salt
Electrolytes where H+1 not only positive ion and OH-1 not only negative ion formed in aqueous solution
Ex: NaCl, CaBr2,KNO3, NH4I

16. Salts in Water (ionic compounds)
NaCl(s)  Na+1(aq) + Cl-1(aq)
CaBr2(s)  Ca+2(aq) + 2Br-1(aq)
KNO3(s)  K+1(aq) + NO3-1(aq)
NH4I(s)  NH4+1(aq) + I-1(aq)

17. Arrhenius Model has limitations
Don’t always use H2O as solvent
Arrhenius model only applies when H2O is solvent
Doesn’t explain all cases:
NH3 doesn’t contain OH-1 but it produces OH-1

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

19. 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

20. Bronsted-Lowry Base Base = proton acceptor OH-1 is a base
H+1 + OH-1  H2O
Not restricted to aqueous solution
NH3 + H2O  NH4+1 + OH-1
NH3 is a base!

21. Bronsted-Lowry Acids & Bases

22. Amphoteric Substance that acts as both acid & base H2O is amphoteric
HX(g) + H2O(l)  H3O+1 + X-1
(base)
NH3 + H2O  NH4+1 + OH-1
(acid)

23. Water is amphoteric!

24. Naming
Acids & Bases

25. Hydro + stem of nonmetal + ic
Naming Binary Acids
Hydro + stem of nonmetal + ic
HF = ?
HCl = ?
H2S = ?
Hydrofluoric acid
Hydrochloric acid
Hydrosulfic acid

26. Naming Ternary Acids Name derived from polyatomic anion (see Table E)
Replace –ite with –ous , add acid
HNO2 is nitrous acid
Replace –ate with –ic, add acid
HNO3 is nitric acid

27. Ternary Acids polyatomics with S and P, make stem long again
H3PO4 = phosphoric acid, not phosphic acid
H2SO4 = sulfuric acid, not sulfic acid
H2SO3 = sulfurous acid, not sulfous acid
SEE TABLE K

28. Name the metal + hydroxide NaOH = ? Ca(OH)2 = ? Mg(OH)2 = ?
Naming Bases
Name the metal + hydroxide
NaOH = ?
Ca(OH)2 = ?
Mg(OH)2 = ?
Sodium hydroxide
Calcium hydroxide
Magnesium hydroxide