1. ACIDS AND BASES

2. Acids Bases Operational Definitions (properties) A. Electrolytes
Strong acids: completely dissociate into ions (hydrochloric, nitric, sulfuric, hydrobromic, and hydroiodic)
Weak acids: do not completely dissociate into ions. (all other acids)
Operational Definitions (properties)
A. Electrolytes
Strong bases: completely dissociate into ions. (soluble hydroxides on table F)
Weak bases: do not completely dissociate into ions. (insoluble hydroxides on table F)

3. Acids Bases B. Taste sour Ex: citric acid in oranges
Lactic acid in milk
B. Taste bitter, feel soapy and slippery

4. C. Change the color of acid-base indicators. (table M)
Acids
pH: between 1 & 7
Litmus: red stays red, blue turns red
Bromothymol blue:
Yellow
Phenolphtalein:
Clear
Bases
Between 7 and 14
Red turns blue, blue stays blue
Blue
Pink

5. D. Undergo neutralization Acid + Base →Salt + Water ex: HCl + NaOH→NaCl + HOH

6. Acid Bases E. Metal + acid →salt + hydrogen
Use table J (only metals above hydrogen can replace it)
Ex: Mg + 2HCl→MgCl H2
E. Emulsify (breaks down) fats and oils

7. Acids Bases Conceptual definitions (explanations) A. Arrhenius:
Acids contain the hydrogen ion or hydronium ion as the only positive ion.
Table K
Ex: HCl, HBr, HF
Conceptual definitions (explanations)
A. Arrhenius:
Bases contain the hydroxide ion as the only negative ion.
Table L
Ex: NaOH (note: first element is a metal)

8. Acids Bases B. Bronsted-Lowry: An acid is a proton donor Example:
NH3 + H2O → NH4+
Base acid 2
B. Bronsted-Lowry
A base is a proton acceptor
NH OH-
Acid 1 + base 2

9. Acids Bases C. Lewis: Electron Pair Acceptor C. Lewis:
Electron Pair Donor

10. Acids Bases Additional information: Monoprotic (1H: HCl) Diprotic
(2H: H2SO4)
Polyprotic
(more than 2H: H3PO4)
Additional information:
Amphiprotic or amphoteric: acts as either an acid or a base.
Example: H2O and
HSO4-

11. Acids Bases Naming acids Binary acids: H nonmetal
Hydro stem of nonmetal ic acid
Ex: HCl: hydrochloric
Ternary acids
H – polyatomic ion
Table E ate becomes ic acid and ite becomes ous acid
Example: H2SO4 : sulfuric acid (no hydro)
Naming bases
Name the metal (use a roman numeral if a metal has more than one oxidation number) followed by hydroxide
Example: KOH: potassium hydroxide