1. ACIDS, BASES, & SALTS

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

3. Electrolyte
Substance when dissolved in H2O produces soln that conducts electric current
Separate into ions in aq soln
Acids, bases, & salts are electrolytes
MgCl2(s)  Mg+2(aq) + 2Cl-1(aq)

4. Can metals react with acids?
See Table J
All metals above H2 react with acids
SR reactions
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 salt
Bases turn litmus blue

7. Formulas of Acids Format: HX where X = nonmetal (F, Cl, Br, I) or
X = negative polyatomic ion
Exception: H2O2
Some acids have 2 or 3 H’s
Ex: HF, H2S, H3PO4

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

9. Identify the Electrolytes
CCl4
HNO3
C5H12
K3PO4
CH3OCH3
LiOH HI
(NH4)2SO4
C12H22O11
NaCl
C2H5OH
H2SO4
NaOH
C6H12O6
CaI2 HF
Mg(OH)2
C3H7OH
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 - B NO NO

10. Acid, Base, or Neutral? all H2O contains some H+1 & 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) + H2O(l)  H+1(aq) + Cl-1(aq)
HNO3 + H2O(l)  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) + H2O(l)  Na+1(aq) + Cl-1(aq)
CaBr2(s) + H2O(l)  Ca+2(aq) + 2Br-1(aq)
Al(NO3)3(s) + H2O(l)  Al+3(aq) + 3NO3-1(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 (base) 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
H2O HSO4-1  H3O+1 + SO4-2

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

21. Bronsted-Lowry Acids & Bases

22. Amphoteric
Substance that acts as both acid & base

23. Water is amphoteric!

24. HX(g) + H2O(l)  H3O+1 + X-1
(base)
NH3 + H2O  NH4+1 + OH-1
(acid)

25. Naming
Acids & Bases

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

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

28. 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

29. 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