Notes made from lecture slides and textbook that will help with understanding and memorisation of the content for chemistry 144. Covers acids and bases, chemical equilibrium, buffers, organic chemistry and organic reactions.
-> substance that in 2 -> substance inc (ON]
>needs renders
Proton ->
proton acceptor
[H+]when
it)
dissolve e when dissolved in water <needs pair of
non-bonding ef
of
*
in
will
any
acid-base reaction,
favour the reaction that
the equilibrium
moves the
short
·restricted
comings
aqueous
to
Arrhenius
solutions
concept:
proton
stronger
to the base
bases Acid-base titrations
only on-containing
· *
·Bronsted expands compounds
considered ->
equivalence point
Lowry
-
of neutralisation
point
->
↓
pH[H+]
How
expands base to include
apes that
-
accepts protons
P
M =
-10g
=
-log[4,O]
(at252)
-
includes ions and molecules
solutions
(HSO,) as acids/bases
well
pH pOH pkw=14.00
as
+
=
-
includes non-agenous
can act as both acid
-
considers amphoteric/amphiprotic species ->
base
and a
acids bases eg. 420 Autoionisation
strong
-
strong
HC
LiOH
In water:
HBr NaOH pure
HI (*) kon equilibrium X 100
K=(H10r] =1.0x0-
H2SO4
RbOH %Ionisation:SHAJinzial :(H+] (OH-]
=
=
1.0x10-2
HNOs C.OH
acid (Ht] equilibrium
greater
at
HCOs CaCOH)2 ->
higher -
stronger
->
Sr(OH), the solution *?
HC0p -> inc more
= dilute
Bu(OH),
weak acids weak bases of cation/anion
Effect in solution
HA(ag) A Laq) H+(aq)
-
+
affect
-weak
cons base anion -> not pl
Ray- -strong conj. base anion -
increase
pH
↓ cations of I and Ca"Sr" Bat- affectph
group
not
greater ha/kb acid/base
stronger
=
-other metalions - decrease in pH
-if both conj. acid + base are
strong, ion with larger Ka, Ky will have
greater
inference
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