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Good Acids and Bases
Strong and Weak Acids
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Strong acids
completely disassociate
in water.
Weak acids only
slightly ionize
in solution
Strong
acids and bases have more "
extreme
" pH values than
weak
acids and bases.
Examples of strong acids:
HCl
HNO3
(nitric acid)
H2SO4
(sulphuric acid)
Examples of strong bases:
NaOH
(
sodium hydroxide
)
KOH
(
potassium hydroxide
)
Ba(OH)2 (
barium hydroxide
)
monoprotic
acid -> produces
1
mol of
H+
per mole of acid (ex.
HCl
)
diprotic acid -> produces
2
mols of
H+
per mole of
acid
(ex.
H2SO4
)
Examples of weak acids:
ethanoic
acid (
CH3COOH
)
carbonic
acid (CO2 in water (H2CO3))
Examples of weak bases:
ammonia
(
NH3
)
aminoethane (C2H5NH2)
3 experimental ways to distinguish between strong and weak acids/bases in
equimolar
solutions:
Concentration
measurement:
Rate of reaction of strong acids is
greater
than that of weak ones.
pH
measurement:
Strong acids have a
lower
pH than weak ones
Strong bases have a
higher
pH than weak ones
Conductivity:
Strong acids/bases are
more
conductive because they contain
more
ions in the solution
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