A review of the fundamentals

1. ACIDS AND BASES
A REVIEW OF THE FUNDAMENTALS

2. LEARNING OBJECTIVES
• REVIEW THE BASIC CHARACTERISTICS OF ACIDS
AND BASES.
• PRACTICE HOW TO NAME ACIDS AND BASES.
• MEMORIZE STRONG ACIDS AND BASES.
• DETERMINE WHICH OXIDES WILL PRODUCE ACIDS
AND WHICH WILL PRODUCE BASES.
• REVIEW TITRATION VOCABULARY.

3. COMMON ACIDS AND BASES
• ACIDS
• FRUITS (LEMONS, ORANGES, ETC…) CONTAIN CITRIC ACID
• VINEGAR CONTAINS ACETIC ACID
• RAIN WATER CONTAINS SULFURIC ACID
• SOFT DRINKS CONTAIN CARBONIC AND PHOSPHORIC ACIDS
• BASES
• CLEANERS CONTAIN AMMONIA.
• MILK OF MAGNESIA CONTAINS MAGNESIUM HYDROXIDE
• DRAIN CLEANER CONTAINS SODIUM HYDROXIDE

4. CHARACTERISTICS OF ACIDS AND BASES
ACIDS
• TASTE SOUR
• TURN BLUE LITMUS
PAPER RED
• HAVE A PH < 7.0
• ARE CORROSIVE
BASES
• TASTE BITTER
• TURN RED LITMUS
PAPER BLUE
• HAVE A PH > 7.0
• ARE CAUSTIC

5. ACIDS
• ARE MOLECULAR COMPOUNDS THAT FORM IONS
IN AQUEOUS SOLUTION.
• INCREASE [H+] IN SOLUTION.
• MEMORIZE 6 STRONG ACIDS:

6. 6 STRONG ACIDS
HI
HCl
HBr
HNO3
HClO4
H2SO4

7. NAMING ACIDS
RULES:
IF THE ANION ENDS IN:
-IDE, HYDRO____IC ACID
-ATE, ____IC ACID
-ITE, _____OUS ACID
SULFUR ADD “UR”
PHOSPHOROUS ADD “OR”
EXAMPLES:
• CHLORIDE  HYDROCHLORIC
ACID
• ACETATE  ACETIC ACID
• HYPOIODITE  HYPOIODOUS
ACID
• SUFATE  SULFURIC ACID
• PHOSPHATE  PHOSPHORIC ACID

8. BASES
• INCREASE [OH-] IN SOLUTION.
• AMMONIA (aq) FORMS A WEAK BASIC SOLUTION
NH3 + H2O  NH4
+ + OH-
• MEMORIZE SOLUBLE HYDROXIDE (EXCEPT NH4OH)
THAT ARE STRONG BASES.

9. STRONG BASES + NH4OH
• LiOH
• NaOH
• KOH
• RbOH
• CsOH
•Ca(OH)2
•Sr(OH)2
•Ba(OH)2
***NH4OH – weak base

10. NAMING BASES
BASES ARE IONIC HYDROXIDES AND SO ARE NAMED
WITH THE SAME RULES AS IONIC COMPOUNDS.

11. OXIDES
METAL OXIDES
• FORM BASES
• CaO + H2O  Ca(OH)2
• Li2O + H2O  2LiOH
NON-METAL OXIDES
• FORM ACIDS
• CO2 + H2O  H2CO3
• SO2 + H2O  H2SO3

12. NEUTRALIZATIO
N
EXAMPLES:
HNO3 (aq) + Al(OH)3(s)
3HNO3 (aq) + Al(OH)3(s) → Al(NO3)3 (aq) + 3H2O
(l)
3H+ + 3NO3
-(aq) + Al(OH)3(s) → Al+3 +3NO3
- +
3H2O (l)
3H+(aq) + Al(OH)3(s) → Al+3(aq) + 3H2O (l)
ACIDS REACT
WITH BASES TO
FORM WATER
AND A SALT.

13. NEUTRALIZATIO
N
EXAMPLES:
Solid silver hydroxide and hydrobromic acid
ACIDS REACT
WITH BASES TO
FORM WATER
AND A SALT.
AgOH(s) + HBr(aq) → AgBr(s) + H2O (l)
AgOH(s) + H+(aq) +Br-(aq) → AgBr(s) +
H2O (l)
AgOH(s) + H+(aq) +Br-(aq) → AgBr(s) +
H2O (l)

14. TITRATIONS – VOLUMETRIC ANALYSIS
Buret - lab apparatus consisting of a graduated glass tube with a
spigot at one end used for titrations.
Titrant – solution of known concentration
Analyte – substance being analyzed
Equivalence point (Stoichiometric point) – The point in the titration
when exactly enough titrant has been added to react exactly with
the analyte.
Indicator – substance added to the analyte that changes color at
(or very near) the equivalence point.
Endpoint – The point where the indicator actually changes color.
(Ideally corresponds with equivalence point)
Phenolphthalein – indicator often used for acid/base titrations. It

15. TITRATIONS – VOLUMETRIC ANALYSIS
• Titrations can be done with acids and bases and with
redox reactions (more next week).
• Titrations are used to standardize (determine the
concentration) of a solution.