Summary

Summary Chemistry 144 Notes

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Stellenbosch University (SUN)

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.

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Uploaded on August 2, 2023
Number of pages 10
Written in 2022/2023
Type Summary

organic chemistry

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Acids + Bases
Arrhenius Acid: Arrhenius Base: Bronsted Bronsted Base:
Lowry Acid:
Lowry
-
-

-> 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

Kara kw.ka=
influence

↳
-
Ka> kp ⑮ ub

acidic
=> =basic =neutral

HF 10 PH [H+] NMs
-

=

CH,N
strong
Acid.Base properties of salts
HNO2
CoH,LOON -> strong HONH- ->
conj.
conj
-

HS-
CH, COOH
acid (t) Hot-=
bases(-) ions reactw ith water ->
hydrolysis
·

HCLO COS

HCN
CLO-
·
is salt acidic/basic?
CoHs OH
↳ Inspectcation,
anion
separately & cation
has no

cation:acidneutral I
14.00 determine
pka+ pky combine to
=

effect on
overall solution pH?
weak
·

con;
acid of strong base -

very
acids the neutral
easier remove :does not reactwith water:
polyprotic
A always to
-

first proton than to remove the second
konjbase of acid is save a
strong

, Chemical equilibrium
Equilibrium constant
partial pressures: Reaction Quotient (a)
aA bB
(Pe
+
c dD+

kp =

I
gives butfor a
->
same ratio as
system

Ko=
Ibar 10 Pa
= notat
equilibrium
if Q = K :
system at equilibrium

solutions -> K determine which
only gases, aqueous compare & and
->
known to

direction proceed to reach
only temp affected reaction will
eq.
->

if Q k reaction shifts
right
< to

if k > [reaCt] reactant)
1 [prod] - cuse up -> Fwd

spontaneous

& k
=

·reaction atag
k 1
=

Sprod] [react] =
-

a > K reaction shifts to left

k< 1 (prod] [react]
* - <use up product) reverse
-

spontaneous

under non-standard conditions: ob=-RTW

Kraverse -Reward
Le ChateliersPrinciple
Knew (Kold]"
=

(co-efficients in balance can changel
disturbed
by change
-> in
system
Kret =

K, x
K2 (adding reactions) ·temp
·pressure comme
concentration
Table:
ICE system will shift to counteractt he
change
if (RJo > 100 x Kc ->
approx

initial reactantconc
change intemp:(K changes)
absorb heat
inc
temp:shifts
-> to

Harber Reaction: :encothermic favoured (04>0)

Ne 3H2+

-
INMs -> dec temp:shifts to release heat

:exothermic favoured (04(0)

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