Ionic eq-invert.pdf,notes.chemistry from pw

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1. FormulasheetofIONICEQUILIBRIUM
BY
:SUHANSHUSIR
#Acid-Base
Theory
①Arrhenius
H
A
H20120
⑦
Theory[
-Hot
->H502-H70z
"¥
⑦
Acid=gives
Hoinwater3
Man
+1
On
-
Base=
gives
On
inwater
"¥
O
-1
-
O 300
H503
↑
20-
neutral
"¥
Han-10
AllArrhenius
acids
②Bronsted-lowny
Theory
areBronsted
Acids
Acid=
gives
notinsolution
(Proton
doncs
Y
-
Base=
accept
10insolution(Protonaccepter)
Acid
-+
Conjugate
Base
/
Base+10-conjugate
Acid
C
.B)
(A)
C

2. ->All
strong
acidshaveweak
Conjugate
Base
Y
samefor
All
weakacids
have
strongconjugate
Base
Bases
.
=>20-Amphoteric
innature
↑20
+120-
↑30
+ok
Auto-protolysis
or
self
Ionisation
n 3of
water
.
C-B
Acid
Bas
-
#Lewis
theory
Lewis
Bases=eOdmor
-
L
wisAcids
=eOacceptor
"¥must
havecomplete
"¥
musthavein complete
Octet
Octetwithlonepair
.
and
vacant
orbitals.
->AllBranstedBasesOreLewis
Bases.
=>Base-Bitterintaste
Acids
--
=
sour
intaste
"¥
changes
BluelitmustoRed
"¥
Changes
RedlitmustoRed

3. #
wald
dilutionlaw-validfor
weak
electrolytes
.
"¥
degreeof
dissociation
C
concentration
x)
-ABA+BE
it<25%or0
.05
,Keg
=222T
C O O
C
-CL CX CX
c=
↑
V
M
Ke
=
2YI
N
=
-
=>Temp
.
4&4 ConcentrationI
[=>for
strongelectrolytes<=100%%orI
degree
of
dissociation↑
=>
S
traction
=Y
=>itdielectricconstant
of
solventincreases
,
&4

4. #pHCalculation
-
P=
-logX
I
cutx=aIQ
oa
pt
=
10gTH
+
]
po
=
-log[OO]
pka
=
-
1099
Case
-I-
strong
acids
Monoproticacid(A)
->TH
=TACIA)
Kb
P
=
=
10gKb Diproticacid
[2A)
-
THE
=2TACIDY
pkw-
-
log
Kw
·
Triproticacid
(HA)
-TH
+
]=
3 TACID]
In
general
pt=
-
logTHt)
-
T
case-
I
-
p4
+
po=14->
Strong
Bases->findpothenpl
.
MonoacidicBase
(BOH)
-TOMO)=
<BAS]
Diacidic
Base(B20H)-[OHO)=
2 TBase]
po=
-log(OH)-
then
ph
=14-pot

5. Case II
Water(120) Kw=[H]TOO]
"¥
Molarityofpure
water
=55
.
55M "¥ejonic
product
of
wate
-
--
Pre/neutral
wate=>TH]
=[0O]
P
kw
=
pH
+pOt
Acidicwater=>[H]TONG)
Basic
water
=>[H
+
]</OO]
aroomtempkw=10Y
-
- pkw=14
forPurewater
,(H)
=TOMO]
10+Y=Th
+
]TOMO]
KW
=THETOMOJ 2
14=
pH
+pot
[
+
]=[00]
=Vkw For
neutralwater
-
atroomtemp
pscale
=0to14
(n
+
]=TO]
=
W
=107
--
acidic
-
-Basic p
=
pOH=7
O H
14
(neutral)
Pscale
=0topkw
=0to14

6. =>asTempincreases
,
Kw↑
at98c
kw=1042
,
pkw
=12
PKW (H
+
]=100]=10-6M
P"
of
neutralwaterI Ph
of
neutralwater=6
pHscale
range
↓ prscale
range
=0to12↓
-
acidia
-
->Basic
Case-IV
effectof
dilution
onpH
!
1
--
8
L
&
12
Dilution/concentration
:M,
V
,
=
M2V2 (neutral)
-
M4V ↓
,
Y
ondilutionincreas
,pH
increases
.
Y
Conc4PHX,
M LV4
ondilutiondecrease
,pl
decream
Case
itHEorTONG]fromacid/Base>10
%
m
,
we
neglectno/onO⑨
fromH20.
⑬it[H]
orTON)fromauid/Basearein
blu10-M
to10-5M
,then
weconsider[H
+
/TOMO]
fromH20
.

7. it
I/TONG)
fromGuid/Base
<10-9M
,
then
pH/PO
=-
⑧
it 0n0
>IM
,
thenowillbe
negative
Laveto
waters
"¥
/po
scale
willnotbevalidfor
concentrane
solution.
Case -
:·
①
Mixture
oftwo
strong
acids
Th]mix
=
NMVzI then
P mix
=
-109THH)
mie
②Mixtureoftwo
strong
bases
10 mix=
Uz]
thenpormixE-log[OnSmi
e
p"mix=14
-
poix
-

8. ③
mixture
ofstrong
audand
strong
Bases.
it
(g)avia
=
(e)
Base
,
thenph
=7(neutral)
it
(neg)acid<(C)Bar
,
thenTh]
mix
=AVA-VB
VA+
VB
↑mix=
-logTmix
it(e)
Acid
<
(neg)
Base
,
then[00mix
= -NAVA
VA+
VB
por
mix=
-log[0mix
↑
=14
-
Po

9. #WeakAcid(HA) WeakBase(BOH)
HA
=
10+AO BOM
-BO+ON
t
=0C
O
O t
=0C O O
-
t
=
em
C
-LxCd(X t=
equ
C
-2X CL
Ca
a
=
d
kb
=
applying
Ostwalddilution
law
,
applying
ostward
dilution
law
,
ka
=
22
kb
=C2
Kax=v
v
=
X
=K
=
[H
+
]=C=
X
[00]
= =Vx[
ph=
z(p(
-
log2)
pol=
z(pkb
-
logC)

10. WeakAcids WeakBases
--
Cacidicstrength&ThL
oraBasic
strength
<
100
Cavidicstrength)
,
Basicstrength),
--
(acidicstrength)=strengths
it 2
,it
Lacidicstrength,
=
=
(Basicstrength)
I
=a
=
--
--
Lavidic
strength)
2
92Basic
strength/a
&
2 Kb2
weak
aids
aremixed,t
weakbasesaremixed
,
Int]mix
=
,X+192x2
+
-
...
-[0]mix
=
4+1 b2x(+-. .
pmix
=
-log/
+
]mix Po=
-10g
08T
mix

11. aud-C
.B
(a)
avid(b)
c
.
B
=Kw
oddion
effect
-
"¥
or
degreeof
pla+pl=pkw dissociation
increase
.
acid
C-B
Base-c
.A
(a)
.
x(b)
Base
=KwCommon
inn
effect
"¥
/degreeof
dissociation
Da
A
+
pl
.B
=pkw
decreases
Wiw
.B
only
-
d=
ca&E
Ka
e
conc"
of
conc
no/onE
tom
Weakaid
B
in
presence
of
S
.
A/S
.B=Commonin
effect
.
Strong
acid

12. #
Buffersolution:
-resistthe
change
in
ph
.
-
"¥
pt
ofBuffersolutiondoesnotdepend
onthewome
of
"¥
solution
.
F Mixed
Buffen-Acidic
BufferWaitsCoB
Simple
Buffer I
W.
A+its
saltwith
says
(W
.
A+w
-
B) L
S
:B
↓
phplalogaWats
mo
Jona
Buffer
=capacity Basi
Buffer (xy)
↓
W
.
B+itsC
.A
PO
=P
Maximum
bufferCapacity
~
B+its
saltwithSoA
3
"¥
log
[sautsres
for
W
.B+S.A
LasAcidic
=>p=pla
Ima(2
>y)
Buffer
&mol
(b)Basic
Buffer
Po
=pkb

13. =>
Higher
the
BufferCapacity,
more
resistantisthesolution
AcidicBuffer BasicBuffer
to
plcharge
.
pk=pl+
logsall
po=p1+
10g[alCA
itamoves
of
S
.
Aisadded itamolesof5.Ais
added
pl
=
p(+
log(
.
B
-x] On
=pkb
+
10g(A
+
]
TACID+U
[Base-]
it
y
moves
of
S
-
1isadded it
f
molesof
S
.Bisadded,
pH
=pl
+
10gB
e
por
=po+
10g-
Max
.
Buffer
Capacity
,p
=pa
Max.
BufferCapacity
,po
=pKb
-[
"¥
&
whensall whensalss
=1

14. BufferRange
-
·
BufferAcidicE
N
phpka ↑
n
=p(+1
-
p
=
pk
-1 "¥
-
(max
.buffercapacity ↓
When
Isalt)
#1
[Acid]
10 over
a
as
10
Buffer
A
↑
po
=#b Pop
-1
#[
↓
ohn
sales
=
t
max
.buffercapacity
when 10
(Base]

15. #SaltHydrolysis
Acid
+Base
-
Salt
+
120
-
=>weakerpartof ↓
AnAidCation
Salt
undergoesHydrolysis
fromBase
W-A+SoB
salts
of-noweaker
part
salts
of-
"¥
no
Hydrolysis
"¥
AntoniaPart
Weake
"¥
pt==
"¥
an"¥
no Loo
·
nicHydrolysis
effect
onlitmus
H
>7
Salt
of
B-Cationicpart
weeken
10+
H20-
HA+on
"¥
Cationic
Hydrolysis
Salts
ofE
L
"¥
W.A+
W
.B
pt<7
"¥
bothcations
&anions
tomsbluelitmustoRed undergoHydrolysis
B+
H-
BOM+H
+B+
H20*
HA+BOH

16. h=degreeofhydrolysis
,Ku=
Hydrolysis
constant
Salt
of
(SA
+
WoB) Salt
of
W
.A+SoB
B
⑦
+
H20
-
>BOH
+1 A
+Hyp
-
#A
+010
&
O
C O
D
C
O
c
-ch
Ch Ch c
-ch
Ch
ch
2
kn
=
-
kn
=
n
=
Kw
Ka
=
1
-n K
b
Applying
Ostwalddilution
law
,
Applying
Ostwalddilutionlaw
kn
=
Ch2
kn
=Ch
n=
va=ICh=
+=
=
r
-
- ION0]
=Ch=VEXC=
(n
+
1=Ch=xnx
=
T pon==
-
1
(pk4
+
10gC)
pt
==
-
z
(pkb+
10g)) ph
=
z+
z(p
**
+
109C)

17. #
Saltf
(
.A+w
.
B)
->
nodependence
on
concentration
-
0+B+
H20
-HA+BOH
C
C
&
D OTrick
to
identity
c
-chc
-ch
Ch Ch
o25
Kale
or
/pla
atvalueot
part
kn
=
h
=
Xb
Weak
Applying
Ostwolddilutionlaw
,
kn
="¥2
P
"
=7+
zz(pk
-p(b)
-
n
=
+I
T
+
]=

18. #
Solubility
Product
(SP)
-
defined
forraingly
solublesalt
↓
product
of
molar
concentration
of
ions
(solubility
<0
.01
M)
raisedtotheirstoichiometric
officients
at
equilibrium
.
-
-
AB(s)
-
A+Bo
AuBy
=A
+
7
+
y
B
>p
=S2
S S
S
S
ksp
=(xs)(ys)y
=>solubilityalways
in
moles/litres
.
Ionic
Product(I.P)
⑮
-
definedonly
at
equin
ledefined
at
any
momentof
reaction
"¥
valueconstantduring
"¥
value "¥
theXM
"¥ changesduring
theExt.
depends
only
ontemp.
dependsonconch
,Temp,
Pressure,
volume

19. I
.P=
Sp
=atequilibrium/saturated
solution
I
.
PS
=
>Unsaturatedsolution
&P>
=>Precipitate
willbeformed
.
For
numericals=>Precipitation
willstartfrom1oP
is
justgreate
than
"¥So
,
IP=P
P
.
I
=>when
equal
vot.
of
differentsaltsaremided
,
[cation]mix=
initial[Anion mi
=#initial
2
2
=>
Common
for
effect
inSolubility
Product
=
>solubility
dureaus
in
presenceofStrongSalt
.
anc"
of
communion
fromstrongexectorate

20. #
SimultaneousEquilibrium
Bothweekelectrolytes
attainequilibrium
insamevessel
andhaveonecommonion.
AB(-
A+Bo
3(SP)Ar
=(
+
su)
s
S2
+S
,
Si
Ac
-A
+c
Y
(SP)
Ac
=(51
+
S2)
Su
s
,
+
52)
S2
C
->it
kspof
bothareof
nearvalues
,
thenS
,
and52
areconsidered
and
solved
.
-it
kpof
oneis
veryhigh,
then
solubilityof
othersalisneglected
andsolved.

21. #
Indicators
-is
a
dya/substance
which
changes
colourover
ashort
range
"¥is
Phenophthalain
:weakad(PhH)
"¥s
colourlessinavidsolutionandpink
inbasicsolution
.
phH
-
>ph8+HE
colorlessPink
inBase
ph
=
pin
+
loge
(ii)M
Orange
:WeakBase(MEOH)
"¥
pinkin
strong
acidicsolution
and
yellow
inBasicsolution
E
MeOl-Me
+On
T
yellowin
Pink/Red
in
Base acid