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)

B. Taste sour Ex: citric acid in

oranges Lactic acid in milk

B. Taste bitter, feel soapy and slippery

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

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

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)

B. Bronsted-Lowry: An acid is a proton

donor Example: NH3 + H2O →

NH4+

Base 1 + acid 2

B. Bronsted-Lowry A base is a proton

acceptor

NH4+ + OH-

Acid 1 + base 2

C. Lewis: Electron Pair

Acceptor

C. Lewis: Electron Pair Donor

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-

Naming acids Binary acids: H nonmetalHydro stem of nonmetal

ic acidEx: HCl: hydrochloric Ternary acidsH – polyatomic ionTable 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