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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)
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B. Taste sour Ex: citric acid in
oranges Lactic acid in milk
B. Taste bitter, feel soapy and slippery
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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
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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
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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)
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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
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C. Lewis: Electron Pair
Acceptor
C. Lewis: Electron Pair Donor
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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-
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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