2.  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.  B. Taste sour  Ex: citric acid in oranges  Lactic acid in milk  B. Taste bitter, feel soapy and slippery

4.  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

6.  E. Metal + acid →salt + hydrogen  Use table J (only metals above hydrogen can replace it)  Ex: Mg + 2HCl→MgCl2 + H2  E. Emulsify (breaks down) fats and oils

7.  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.  B. Bronsted-Lowry:  An acid is a proton donor  Example:  NH 3 + H 2 O → NH 4 +  Base 1 + acid 2  B. Bronsted-Lowry  A base is a proton acceptor NH 4 + + OH - Acid 1 + base 2

9.  C. Lewis:  Electron Pair Acceptor  C. Lewis:  Electron Pair Donor

10.  Additional information:  Monoprotic (1H: HCl)  Diprotic (2H: H 2 SO 4 )  Polyprotic (more than 2H: H 3 PO 4 )  Additional information:  Amphiprotic or amphoteric: acts as either an acid or a base.  Example: H 2 O and HSO 4 -

11.  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: H 2 SO 4 : 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