7.0 Ionic Equilibria (Students)
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1. Acids and bases
2. Acids-Base titration
3. Solubility equilibria
a) Define acid and base
b) Define and identify conjugate acids andconjugate base according to Bronsted-Lowryteory
c) Define
d) Define pH ! pOH
e) "elate #$ and #%$ to &w at 2'(
f) alculate #$ *alue of strong acid and base
g) "elate strengt of a wea+ acid and wea+ baseto te Ka and Kb (pKa,pKb,pKw,pH,pOH)
) ,erfor calculation #$! &a! &b! / 0! α)
i) # salt ydrolysis and write its equation
j) Define buffer solution
+) Describe ow buffer solution controls #$
l) Deri*e $enderson-$asselbalc equation
a) Describe titration #rocess
b) Distinguis between te end #oint andequi*alence #oint
c) S+etc and inter#ret te *ariation of #$ againtstitre *alue for titration between
i) strong acid-strong base
ii) strong acid-weak base
iii) weak acid-strong base
a) dentify suitable indicator for acid-base titration
a) Define
i) solubility
ii) molar solubility
iii) solubility product ,Ksp
b) alculate &s#
c) ,redict te #ossibility of #reci#itation of sligtlysoluble ionic co#ounds by co#aring te *alue of ion-#roduct! Q to Ksp
d) Define and e#lain te coon ion effect
e) ,erfor calculation related to coon ion effect
Arrhenius theory
Bronsted-owry theory
ewis theory
strong acid and strong base strong acid and weak base
weak acid and strong base
strong acid and base
weak acid and base
4.( %5 67LB"A%8"89
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Learning outcoes: (1 hour)
At the end of this lesson , students should be able to:
Define acid and base according to Arrhenius, Bronsted-
Lowry and Lewis theories.
Define and identify conjugate acid and conjugate base
according to Bronsted- Lowry theory. Define strong acid and base, weak acid and base.
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;e #$ of te gastric juice is about 1.'! wiccorres#onds to $l (.(3 !
a concentration strong enoug to dissol*e <inc etal=
9at is te #$ of te gastric juice in your stoac>
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%5 67LB"7?
4.1 ;eory of Acids and Bases
9e generally classify acidsand bases as eiter strong or wea+! according to te etent of
teir dissociation into ions inwater.;e concentration of
/$@0 or /%$-0
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5"AL ,"%,";S % ADS and BASS
ADS BASS
$a*e a sour taste $a*e a bitter taste
"eact wit acti*e etals suc as Al and Cn to#roduce $2 gas
ange color of litusfro blue to red
ange color of litusfro red to blue
Aqueous acid solutions
conduct electricity
Aqueous base solutions
conduct electricity
"eact wit carbonates and bicarbonates suc
as 5a2%3! a%3 and
5a$%3 to #roduce %2 gas
eel sli##ery
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Acidbase definition:
Arrenius
BrEnstedLowry
Lewis teories
S*ante August Arrenius 1F'G-1G24). Swedis ceist.
Hoannes 5icolaus BrEnsted 1F4G-1GI4). Danis ceist.;oas ?artin Lowry 1F4I-1G3J)! nglis ceist.
ilbert 5ewton Lewis 1F4'-1GIJ). Aerican ceist.
9$A; S AD > 9$A; S BAS >
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Acid: Substance tat as $ in its forula and
dissociates in water to yield $3%@
KA?,L:
Base: Substance tat as %$ in its forula
and dissociates in water to yield %$
KA?,L:
A""$57S ADBAS D5;%5
$5%3a" ) @ $2%l ) $3%@a" ) @ 5%3
a" )
$3%%$a" ) @ $2%l ) $3%% a" ) @ $3%@a" )
5a%$a" ) 5a@a" ) @ %$ a" )
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Base: Any s#ecies tat acce#ts $@ #roton acce#tor )
B"5S;DL%9"M ADBASD5;%5
;e definition focus on #roducts and reactants
acidbase reaction)
5$3a" ) @ $2%l ) 5$I@a" ) @ %$ a" )
acid conjugatebase
base conjugateacid
Acid: Any s#ecies tat donates $@
#roton donor )
$3%%$a" ) @ $2%l ) $3%% a" ) @ $3%@a" )
KA?,L:
acid conjugate
base
base conjugate
acid
KA?,L:
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*ery acid as a conjugate base
*ery base as a conjugate acid
BAS-%5H7A; AD ,A"
$3%%$a" ) @ 5 a" ) $3%% a" ) @ $5a" )
acid base conjugatebase
conjugateacid
Acid: #roton donor
Base: #roton acce#tor
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Acid: Any s#ecies tat acce#ts an electron #air
KA?,L: B3 ! All3 ! S%2 ! %2 ! 5a@
KA?,L: 5$3! $3l! $3%$3! $2%! %2
Base: Any s#ecies tat donates an electron #air
A @ :B
L9S ADBAS D5;%5
ANB
acid base
new co*alent bond
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ontains a central ato tat is electron deficient inco#lete octet
KA?,L:●●
B
●●
●●
●●
●●
●●
●●
●●
●●
5 $
$
$●●
B
●●●
●●●
●●●●
●●
●●●●
●●
5 $
$
$
acid base
L9S ADS 9;$L;"%5 D5; A;%?S
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;able J.1 : a#les of Lewis acids and bases
Lewis acid Lewis base
(a) ositi!e ions
e.g : "# , $e%# , Al&#
(a) 'egati!e ions
e.g : "- , '- , l-
(b) *olecules with an inco+leteoctet of electrons.
e.g : B$& , Bel% , Bl&
(b) *olecules with lone air ofelectrons.
e.g : "% , '"& , "
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dentify te conjugate acidbase #airs:a) $%%$a" ) @ $2%l ) $%% a" ) @ $3%
@a" )
b) $2%l ) @ a" ) %$ a" ) @ $a" )
c) $2,%I a" ) @ %3
2 a" ) $%3 a" ) @ $,%I
2 a" )
d) $2%l ) @ S%32 a" ) %$ a" ) @ $S%3
a" )
EXAMPLE
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Ans: EXAMPLE
a) $%%$a" ) @ $2%l ) $%% a" ) @ $3%@a" )
b) $2%l ) @ a" ) %$ a" ) @ $a" )
A O acid
cA O conjugate acid
B O base
cB O conjugate base
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Ans: EXAMPLE
c) $2,%I a" ) @ %32 a" ) $%3 a" ) @ $,%I2 a" )
d) $2%l ) @ S%32 a" ) %$ a" ) @ $S%3
a" )
A O acid
cA O conjugate acid
B O base
cB O conjugate base
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Dissociate co#letely 1(( P! α O 1.() into ions
in water
$Al ) @ $2%l ) $3%@a" ) @ A a" )
Ka etreely large
S;"%5 AD
$ydroalic acids: $l! $Br and $
%oacids: $5%3! $2S%I and $l%I
$5%3a" ) @ $2%l ) $3%@a" ) @ 5%3
a" )
KA?,L:
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Dissociate *ery sligtly α Q 1.() into ions in water
K a *ery sall
$Aa" ) @ $2%l ) $3%@a" ) @ A a" )
$5a" ) @ $2%l ) $3%@a" ) @ 5 a" )
KA?,L:
9A& AD
%oacids: $l%! $5%2 and $3,%I
%rganic acids: $3%%$ and J$'%%$
$ydroalic acids: $
%ter: $5 and $2S
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Dissociate co#letely 1(( P) into ions in water
K b etreely large
S;"%5 BAS
?2% or ?%$:
?% or ?%$)2:
Soluble co#ounds containing %2 or %$
?: rou# 1) etal Li! 5a! &! "b! s)
?: rou# 2) etal a! Sr ! Ba)
KA?,L:
5a%$a" ) 5a@a" ) @ %$ a" )
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Dissociate *ery sligtly into ions in water
K b *ery sall
5$3g ) @ $2%l ) 5$I@a" ) @ %$ a" )
KA?,L:
9A& BAS
?olecules wit an 5 ato tat as a lone#air electrons:
5$3 ..
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lassify eac of te following co#ounds asa strong acid! wea+ acid! strong base! or wea+ base! or s#ecies wit negligible acidity.
a) $3
)2
$%%$
b) &%$c) $3)2$5$2
d) $5%2
e) $2S%I
f) $,%I2
g) $I
) $35$3
@
EXAMPLE
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Ans: EXAMPLE
a) $3)2$%%$
b) &%$
c) $3)2$5$2
d) $5%2
e) $2S%I
f) $,%I2
g) $I
) $35$3@
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Define #$ and #%$
"elate #$ and #%$ to te ionic #roduct ofwater! K w at 2'(
alculate te #$ *alues of a strong acidand base.
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4.1.I: #$ and #%$
#%$ is defined as te negati*e logarit log) ofte ydroide ion.
#$ is defined as te negati*e logarit log) of
te ydroniu!$3%@
concentration. /$3%
@0 in a solution is easured using
#$ scale etod.
#$ O - log /$@0
∴
f /$@0↑
! #$↓
.
concentration of %$- is easured using #%$.
#%$ O - log /%$-0
∴
f /%$-
0↑
! #$ ↑
! #%$ ↓
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#$ O log /$3%
@
0#%$ O log /%$ 0
#$ SAL
;e iger /$3%@0! te lower #$
;e iger te /%$ 0! te lower #%$
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Acidbase indicator
#$ #a#er R color cart)
#$ eter
#$ ?AS7"?5;
#$ of a neutral solution O 4.(
#$ of an acidic solution Q 4.(
#$ of an basic solution 4.(
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9ater dissociates into ions *ery sligtly
/ $3%@
0 / %$
0K 9 O
O 1.( 1( 1I at 2'o)
n #ure water at 2'oT
K 9 : ion #roduct constant for water
A7;%%5CA;%5 % 9A;"
$2%l ) @ $2%l ) $3%@a" ) @ %$ a" )
/$3%@0 O /%$ 0 O 1.( 1( 4 ?
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"elationsi# between K w! #$ and #%$ at 2'o!
/$@0 /%$-0 O K w
-log bot side! -log /$@0 /%$-0) O -log K
w-log /$@0 @ log /%$-0) O - log 1.( 1(-1I)
#$ @ #%$ O #K w
#$ @ #%$ O 1I
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A cange in /$3%0@
causes an in*erse cangein /%$ 0
$iger /$3%@0 lower /%$ 0
$iger /%$ 0 lower /$3%@0
Bot ions are #resent in all aqueous systes
n acidic solution! /$3%@0 /%$ 0
n basic solution! /$3%@0 Q /%$ 0
n neutral solution! /$3%@0 O /%$ 0
/$3%@0 and /%$ 0
/$@0 /%$-0 O K w
AL7LA;5 /$ %@0 A5D /%$ 0
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K 9 O / $3%@ 0 / %$ 0 O 1.( 1( 1I at 2'o)
/ $3%@ 0 O
K 9
/ %$
0
/ %$ 0 OK 9
/$3%@
0
AL7LA;5 /$3%@0 A5D /%$ 0
5 A67%7S S%L7;%5
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#$ U #%$ S;"%5 ADS A5D BASS
Strong acids and bases are considered to be 1((P dissociated in an aqueous solution
KA?,L: Strong acid
$la" ) @ $2%l ) $3%@a" ) @ l a" )
before: (.(2( ! ( (
after: (( #$$% dissociated )
(.(2( ! (.(2( !
#$ O log /$3%@0
O 1.4(
O log /(.(2(0
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KA?,L: Strong base
Ba%$)2a" ) Ba2@a" ) @ 2%$ a" )
before: (.(((3' ! ( (
after: (( #$$% dissociated ) (.(((3' ! (.(((4( !
#$ O log /$3%@0
O 1(.F'O log 1.I3 1( 11)
/ $3%@ 0 O K 9
/%$ 0
O1.( 1( 1I
(.(((4(O 1.I3 1( 11 !
#$ U #%$ S;"%5 ADS A5D BASS
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EXAMPLE
a) 9at is te #$ of a (.(I( ! solution of $l%I >
b) An aqueous solution of $5%3 as a #$ of
2.3I. 9at is te concentration of te acid >
c) 9at is te #$ of A (.((11 ! solution of a%$)2>
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Ans: EXAMPLE
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Ans: EXAMPLE Ans: EXAMPLE
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Ans: EXAMPLE
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Ans: EXAMPLE
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"elate te strengt of a wea+ acid and wea+ base tote res#ecti*e dissociation constant! K a and K b.
,erfor calculations in*ol*ing #$! dissociationconstant! initial concentration and te degree ofdissociation! V
WWWW alculations are liited to #robles wit quadraticequation: a2@b@cO(. A##ly a##roiationetod if &a or &b X1(-'
AD DSS%A;%5 %5S;A5; K )
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Dissociation of wea+ acid in water :
/ $3%@
0 / A
0/ $A 0
K a O
ADDSS%A;%5 %5S;A5; K a)
$Aa" ) @ $2%l ) $3%@a" ) @ A a" )
KA?,L:
$5a" ) @ $2%l ) $3%@a" ) @ 5 a" )
/ $3%@ 0 / 5 0
/ $5 0
K a O
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$@a" ) O $3%@a" )
KA?,L:
$5a" ) @ $2%l ) $3%@a" ) @ 5 a" )
/ $3%@ 0 / 5 0
/ $5 0K a O
or
$5a" ) $@a" ) @ 5 a" )
K a O / $@ 0 / 5 0
/ $5
0
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stronger acid
iger /$3%@0
larger K a
saller K a
lower P $A dissociated
wea+er acid
or strong acids and bases dissociate 1((P):K a or K b *alues a*e not been easured
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EXAMPLE
Nitrous acid, HNO2, is a weak acid that or!ed in thesto!ach when nitrite ood "reser#ati#es encounter
sto!ach acid$ %here has &een so!e concern that
this acid !a' or carcinoenic "roducts &' reaction
with "roteins$9rite te ceical equation for te equilibriuioni<ation of $5%2 in water and te a##ro#riate
K a
e#ression.
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Ans: EXAMPLE
BAS DSS%A;%5 %5S;A5; K )
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Dissociation of wea+ base in water :Ba" ) @ $2%l ) B$@a" ) @ %$ a" )
/ B$@ 0 / %$ 0/ B0
K b O
BASDSS%A;%5 %5S;A5; K b)
KA?,L:
5$3a" ) @ $2%l ) 5$I@a" ) @ %$ a" )
/ 5$I@ 0 / %$ 0
/ 5$3 0K b O
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9en a #roton $@) is acce#ted by a wea+base contains a 5 ato! te $@ binds to a lone#air of electrons on a 5 ato of te base
KA?,L: for te reaction wit water)
5$3a" ) @ $2%l ) 5$I@a" ) @ %$ a" )
52$Ia" ) @ $2%l ) 52$'@a" ) @ %$ a" )
$3)25$a" ) @ $2%l ) $3)25$2@
a" ) @ %$
a" )
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EXAMPLE
H'dra*ine is a weak &ase$ +t is a "oisonous su&stancethats so!eti!es or!ed when ch-orine &-each is
added to an a.ueous so-ution o a!!onia$
9rite te equation for te reaction of ydra<ine
52$I) wit water and write te e#ression for its K b.
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Ans: EXAMPLE
#$ alculation for 9ea+ Acid
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#$ alculation for 9ea+ Acid
/onsider a general wea+ acid! $A$
%he ionisation equation in water is i#en &':
HA(a.) 0 H2O(-) H
O0(a.) 0 A(a.)
i*en! c O initial concentration
O concentration of $3%@ ion dissociated
HA(aq)
H3O+
(aq)A-
(aq)
Initial Conc. (M)
Change (M)
Equilibrium Conc.(M)
At equilibriu, ][
][][ 3
HA
AO H −+
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&a
O ) )
c- )
&a for a wea+ acid in water $
Assu!in, that on-' a sall aount of aciddissociates, i$e$ &
a QQQ 1, thereore:
$A] O c ~ c ∴ K a !"
c2 O &
a.c
O √ &a
. )
O $3O+]
#$ alculation for 9ea+ Acid
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f te degree of dissociation! α is gi*en!
$Aaq) @ $2
%l) A-aq) @ $3%@aq)
i*en! c O initial concentration α O Degree of dissociation
HA(aq)
A-(aq)
H3O+
(aq)
Initial Conc. (M) c # #
Change (M) -cα
+cα
+cα
Equilibrium conc.(M) c - cα
c( $-α
)
cα
cα
At equilibriu, &a O A-
] $3%+]
$A ]
#$ alculation for 9ea+ Acid
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][
][][ 3
HA
AO H −+
&a 4
)1(
)()(
α
α α
−c
cc4
)1(
2
α
α
−
c4
5or a wea+ electrolyte, α is #er' s!a--$
%hus, on-' a s!a-- a!ount o acid dissociates,
Hence, &a QQQ 1, thereore: 1 - α ≈ 1
α = (&a & c) $&"
[H+] = c α = c (&a & c) $&"
= (&a. c) $&"
∴
&a c
α
2
#$ alculation for 9ea+ Base
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/onsider a general wea+ base! B$
%he ionisation equation in water is i#en &':
Baq) @ $2%l) $B@aq) @ %$-aq)
i*en! c O initial concentration
O concentration of %$- ion dissociated
'(aq)
H'+(aq)
OH-(aq)
Initial Conc. (M) c # #
Change (M) -! +! +!Equilibrium conc.(M) c- ! ! !
At equilibriu, &b O B$+
] %$
]
B]
#$ alculation for 9ea+ Base
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Assu!in, that on-' a sall aount of basedissociates, i$e$ &
b QQQ 1, thereore:
B]
O c
~ c
∴ K b
!"
c
2 O &b.c
O √ &b . c
O OH-]
&b for a wea+ base in water $
At equilibriu, &b O $B+]
%$
]
B ]
O ) ) c- )
#$ alculation for 9ea+ Base
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Baq) @ $2%l) $B@
aq) @ %$-
aq)
f te degree of dissociation! α is gi*en!
i*en! c O initial concentration α O Degree of dissociation
'(aq) H'+(aq) OH-(aq)
Initial Concentration (M) c # #
Change (M) -cα +cα +cα
Equilibriumconcentration(M)
c( $-α
) cα
cα
At equilibriu, &b O $B+
] %$
]
B]
#
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)1(
)()(
α
α α
−c
ccO
)1(
2
α
α
−
cO
5or a wea+ electrolyte,α
is #er' s!a--$%hus, on-' a sall a!ount o acid dissociates,
$ence! &b QQQ 1, thereore: 1 -
α
≈
1
α = (&
b & c) $&"
[H+] = c α = c (&b & c) $&"
= (&b. c) $&"
At e.ui-i&riu!, &b O $B+
]
%$
]
B ]
∴
&b c
α
2
S%L85 ,"%BL?S 58%L85
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;wo general ty#es of #robles:
i*en equilibriu concentration! find K a or K b)
i*en K a or K b) and soe concentration
inforation! find te oter equilibriu concentrations
S% % S % 9A& AD U 9A& BAS 67LB"A
7se &' table =
Assu#tions:
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Assu#tions:
/$3%@0 fro autoioni<ation of $2% is
negligible
A wea+ acid as a sall K a! So:
/$A0initial /$A0dissoc Z /$A0initial
/$A0initial O /$A0initial *ery sall)
A##ly ' P test to cec+ teassu#tion is justified
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Approximationmethod or quadratic
method??
Apply theapproximation
method if Ka orKb ≤ 10-5
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HOW?? xam le if Ka or Kb i!
1"# x 10
-5
$ then u!e
a roximation method if
%"# x 10
-&
$ u!e quadratic
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HOW?? r your can check the !alue, if
less than / than you can
choose aro0i+ation +ethod. 1hefor+ula is :
2 3a or 3b 0 455
c6
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B.7eak Base
80a+le 4 :
1he base-dissociation constant for a++onia, '"&(a9) is 4. 0 45-/ *.alculate the concentration of "- ion, " and dissociation at
e9uilibriu+ if the initial concentration of '"& is 5.4/ *.
Kb
; <initial
use approximationmethod because
Ka is 1.8 x 10-5
"83=
2 3a or 3b 0 455
c
2 1.8 x 10-5 x 100
5.4/2 4.5> less than /
(use aro0i+ation +ethod )
6
6
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80ercise :
4. alculate the ercentage of "$ +olecules ioni?ed in
(a) a 5.45 * "$ solution the K a of "$ is @. 0 45 -A (.> )
use quadratic
because Ka of HF is
6.8 x 10 -4 greaterthan 10-5
"83=
2 3a or 3b 0 455c
2 6.8 x 10 -4 x 100
5.45
2 .%A +ore than /
(use 9uadratic)
66
EXAMPLE 1
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EXAMPLE 1
9at is te #$ of a (.'
! $ solution at 2'
o
)>K a of $ O 4.1 1( I
Ans: EXAMPLE 1
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Ans: EXAMPLE 1
Ans: EXAMPLE 1
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Ans: EXAMPLE 1
EXAMPLE 2
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EXAMPLE 2
alculate:a) ;e basedissociation constant! K b!
for te fluoride ion ) K a of $ O J.F 1( I
b) ;e aciddissociation constant! K a!
for te aoniu ion 5$I@)
K b of 5$3 O 1.F 1( '
Ans: EXAMPLE 2
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Ans: EXAMPLE 2
Ans: EXAMPLE 2
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Ans: EXAMPLE 2
"LA;%5S$, B;95 &a and &b
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Dissociation of 5$3 in water:
5$3a" ) @ $2%l ) 5$I@a" ) @ %$ a" )
K b O/ 5$I
@ 0/ %$ 0
/ 5$30
% S a a d b
K a O/ 5$3
0 / $3%@ 0
/ 5$I@0
base onjugate acid
Dissociation of 5$I@ in water:
5$I@
a" ) @ $2%l ) 5$3a" ) @ $3%@
a" )
K a ! K b ! K w ! #K a ! #K b A5D #K 9
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K a K b O K w
/ 5$I
@ 0 /%$-0
/ 5$30
2$2%l ) $3%@a" ) @ %$ a" )
/ 5$3 0 /$3%
@ 0
/ 5$I@0
#K a @ #K b O #K w
a ! b ! w ! # a ! # b # 9
5$3
a" ) @ $2
%l ) 5$I
@a" ) @ %$ a" )
5$I@a" ) @ $2%l ) 5$3a" ) @ $3%
@a" )
K b K a O
base onjugate acid
acid onjugate base
O / $3%@ 0/%$ 0
K a A5D #K a
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#K a O N log K a
a # a
$ig K a low #K a
iger acidity
K b A5D #K b
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#K b O N log K b
b # b
K b #K b
I.4I
F.44
G.I2
1I.F2
iger basicity
$ig K b low #K b
∴
Acid-dissociation constant K a) andb di i ti t t Kb)
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;e *alue of K a or K b can be used to distinguis terelati*e acidity strengt of wea+ acid and wea+ base.
6 &a ↑ #K a ↓ ) O /$@0 ↑ ! tus #$ ↓ ore acidic)
6 &b ↑
#K b↓
) O /%$-0↑
! tus #$↑
ore basic)
∴base-dissociation constant K b)
80a+le :
Acid #K a
$3%%$ I.4I$%%$ 3.4J
Base #K b
J$'5$2 G.345$3 I.4I
"elati*e acidity!$%%$ $3%%$
"elati*e basicity!5$3 J$'5$2
EXE7/+8E 1
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EXE7/+8E 1
A5S:a) 4.1 1( 11
b) 2.3 1( 11
a) Lactic acid, H/H9O2, is res"onsi&-e or the taste o sour !i-k$ At 2'o it K a O 1.I 1( I.
9at is te K b of its conjugate base! te
lactate ion! 3$'%2
>
b) Meth'-a!ine, /HNH2, rese!&-es a!!onia in
odor and &asicit'$ ts K b O I.I 1( I.
alculate te K a of its conjugate acid
EXE7/+8E 2; 4.1
EXE7/+8E 2
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Pro"anoic acid (/2H9/OOH)(!ono"rotic)is an oranic acid whose sa-ts are used to
retard !o-d rowth in oods$
9at is te /$3%@0 of (.1( ! 2$'%%$ >
5ote: K a O 1.3 1(-'.
A5S:/$
3
%@0 O 1.1 1(-3 !
EXE7/+8E 2; 4.1EXE7/+8E 2
EXAMPLE 2 4.1
EXE7/+8E
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EXAMPLE 2
;e a*erage #$ of noral arterial blood is 4.I(.At noral body te#erature 34o)!K w O 2.I 1( 1I. alculate /$@0 and /%$ 0 for blood
at tis te#erature.
A5S:a) /$@0 O I.( 1( F !
b) /%$
0 O J.( 1( 4
!
EXE7/+8E
EXE7/+8E ;
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1. A (.2( ? solution of wea+ acid $K is G.IP dissociated.7sing tis inforation! calculate $3%
@ ! K- and $K
concentrations at equilibriu. Deterine also #$ and&a for $K acid.
1.FF 1(-2 ?! (.1F12 ?! 1.43! 1.4J 1(-3)
2. alculate te forate ion concentration and #$ of asolution tat is (.('( ? in foric acid.$$%2 : &a O 1.F 1(-I).
$%2- O G.( 1(-' ! #$ O 1.(( )
EXE7/+8E ;
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#lain salt ydrolysis and write ydrolysis equationfor te salt fored fro te reaction between:
i. Strong acid and strong base
ii. Strong acid and wea+ base iii. 9ea+ acid and strong base
Define buffer solution
SAL; $MD"%LMSS
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Salt ydrolysis: reaction of an anion or cation of asalt or bot) wit water.
eneral equation of neutrali<ation :
$K @ ?%$ ?K @ $2%
acid) base) salt) water)
?K salt dissociation equation:
?K ?@
@ K-
ation $ydrolysis : ?@aq) @ $2%l) ?%$aq) @ $@
aq)
Anion $ydrolysis : K-aq) @ $2%l) $Kaq) @ %$-aq)
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$3%%5as) 5a@
a" ) @ $3%%
a" )
$2%
9at is te effect to te acidity of te solution>
KA?,L:
S#ecies eist:
5a@ and $3%%
$3%@ and %$ fro autoioni<ation of $2%
negligible)
Salt ydrolysis:
5a@ @ $2% 9at a##en >
$3%% @ $2% 9at a##en>
SAL; $MD"%LMSS : "%? S;"%5 AD A5DS;"%5 BAS
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S;"%5 BAS
Anion fro strong acid l ! 5%3 ! Br ! l%I
)
5als) 5a@a" ) @ l a" )$2%
KA?,L: 5al solution
Salt consisting:
ation fro strong base 5a@! &@! Li@! a2@ )
5eiter 5a@ nor l ioni<e in water
?ay ro 5a%$ solution
?ay ro $l solution
SAL; $MD"%LMSS : "%? 9A& AD A5DS;"%5 BAS
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S;"%5 BAS
Anion fro wea+ acid e.g: $3%% ! ! 5%2 )
KA?,L: $3%%5a solution
Salt consisting:
ation fro strong base 5a@! &@! Li@! a2@ )
$3%%5as) 5a@a" ) @ $3%% a" )$2%
$3%% a" ) @ $2%l ) $3%%$a" ) @ %$ a" )
5a@ does not ioni<e in water
?ay ro 5a%$solution
ro $3%%$
solution
;erefore! te ydrolysis salt equation:
SAL; $MD"%LMSS : "%? S;"%5 AD A5D9A& BAS
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9A& BAS
Anion fro strong acid l ! 5%3 ! Br ! l%I
)
KA?,L: 5$Il solution
Salt consisting:
ation fro wea+ base e.g: 5$I@! $35$3
@ )
5$Ils) 5$I@a" ) @ l a" )
$2%
l does not ioni<e in water
ro 5$3 solution
ro $l solution
;erefore! te ydrolysis salt equation:
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5als) 5a@a" ) @ l a" )$2%
Dissolution and dissociation of salts in water can be
written as:
or 5ala" ) 5a@a" ) @ l a" )
EXAMPLE
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9rite te ydrolysis salt equation:
a) 5$I
b) al2
c) &5
d) Lil%I
e) $35$3@ 5%3
f) 5a%l
g) &l) 5$I5%3
i) 5a5%2
EXAMPLE
Ans: EXAMPLE
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Ans: EXAMPLE
EXAMPLE 9 4.1
Ans: EXAMPLE
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EXAMPLE 9 Ans: EXAMPLE
EXAMPLE 9 4.1
Ans: EXAMPLE
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EXAMPLE 9 Ans: EXAMPLE
B7" S%L7;%5
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$ow does blood aintain a constant#$ in contact wit countless cellular
acidbase reaction >
;e noral of #$ of blood is 4.I
Se*ere illness or deat can resultsfro sustained *ariation just a fewtents of a #$ unitfro tis
noral *alue
;ere ust be as syste in our body to aintain te #$ of blood or anyaqueous solution =
B7" S%L7;%5
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is a solution wic as te ability to maintain its pH
wen a small amount of strong acid or strong baseis added to te solution.
t ust contains:
Acidic co#onent can react wit added /%$ 0
Basic co#onent
can react wit added /$3%@
0 ?ost coon buffer co#onents:
base - onjugate acid #air of wea+ base) %" acid - onjugate base #air of wea+ acid)
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Buffer solution contains only eiter
wea+ acid or base.
f te syste contains strong acid or base!te syste A55%; act as a buffer solution.
B7""D 8s 75B7"D S%L7;%5
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Solution of dilute $l
Solution of iture of1 ! $3%%$ and
1 ! $3%%5a
Addition of 1 ! $l Addition of 1 ! 5a%$
Addition of 1 ! $l Addition of 1 ! 5a%$
;e syste is not buffer solution due
to te large different of #$ *alue.
;e syste is buffer solution due tote sall different of #$ *alue.
EXAMPLE
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9ic of te following are buffer systes>
a) & U $b) &Br U $Br c) 5a2%3 U 5a$%3
Ans: EXAMPLE
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Deri*e te $enderson-$asselbalc equation. alculate te #$ of buffer solutions.
Decribe qualitati*ely ow a buffer solutioncontrols its #$
; t f b ff l ti
B7" S%L7;%5
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;wo ty#es of buffer solutions :
i. Acidic buffer solution #$Q4)
ii. Basic buffer solution #$4)
A wea+ acid and its conjugate base
KA?,L:
?iture of $3%%$ U $3%%5a
?iture of 5$3 U 5$Il
Acidic co#onent $3%%$
Basic co#onent $3%%
A wea+ base and its conjugate acid
Acidic co#onent 5$I@
Basic co#onent 5$3
$%9 A B7" %5;"%L its #$:a#le: $3%%$ U $3%%5a
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$3%%$$3%%-
$3%%-
$3%%-$3%%$
acid $@) base %$-)
A buffer syste contains etanoic acid!$3%%$
and etanoat ion! $3%%-
fro $3%%5a
$3%%$ aq) $3%%- aq) @ $@ aq)
$3
%%5a aq) $3
%%- aq) @ 5a@ aq)
$@
added) @ $3%%-
%$-added) @ $3%%$
$3%%$ $3%%- @ $2%
3 3
Addition of $3%@ :
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Aount of $3%@ added O Aount of $3%% consued
O Aount of $3%%$ #roduced
$3%@a" ) @ $3%% a" ) $3%%$a" ) @ $2%l )
/$3%%-0 decrease and /$3%%$0 increase
As a result! tere will be only a sall cange in #$
$3%%-
$3%%-
$3%%$$3%%$
$@)
$3%%- aq) @ $@ $3%%$ aq)
Addition of %$ :
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Aount of %$ added O Aount of $3%%$ consued
O Aount of $3%% #roduced
%$ a" ) @ $3%%$a" ) $3%% a" ) @ $2%l )
/$3%%-0 increase and /$3%%$0 decrease
As a result! tere will be only a sall cange in #$
$3%%-
$3%%-
$3%%$$3%%$
$%-)
$3%%$ aq) @ $%- $3%%- aq)
EXE7/+8E < 4.1
EXAMPLE 1
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Sow ow 5$3 5$Il solution is abuffer solution.$int: dentify a co#onent in te solution tat neutrali<es acids and a co#onent
tat neutrali<es bases)
Ans: EXAMPLE 1
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$5D"S%5$ASSLBAL$ 67A;%5
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$Aa" ) @ $2%l ) A a" ) @ $3%@a" )
/ $3%@
0 O
or wea+ acid:
/A 0 / $3%@0
/$A0K a O
rearrange
* log K a N log /$3%@0 O
/A 0
/ $A0 * log
#$ O #K a @ log/wea+ acid0
/ onjugate base0
/A 0
/ $A0K a
$5D"S%5$ASSLBAL$ 67A;%5
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5$3a" ) @ $2%l ) 5$I@a" ) @ %$-a" )
or wea+ base:
/5$I@0/%$-0
/5$30K b O
rearrange
* log K b N log /%$-0 O/5$I@0
/5$30 * log
#%$ O #K b @ log/wea+ base0
/ onjugate acid0
/5$I@0
/ 5$30K b/%$-0 O
EXAMPLE ;1 4.1
EXAMPLE 2
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a) alculate te #$ of a solution containing(.2( ! $3%%$ and (.3( ! $3%%5a.
b) 9at would te #$ of a (.2( ! of
$3%%$ solution be if no salt were#resent>
K a of $3%%$ O 1.F 1( '.
EXAMPLE ;1 4.1
Ans: EXAMPLE 2
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EXAMPLE ;1 4.1
Ans: EXAMPLE 2
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EXAMPLE ;1 4.1
Ans: EXAMPLE 2
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EXAMPLE ;= 4.1
EXAMPLE
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%o stud' the in-uence o an a-ka-ine !ediu!o a reaction, a buffer solution was #re#ared bydissol*ing (.12 ol of 5$3 and (.(G' ol of
5$Il in water. 9at is te #$ of te buffer>
K b of 5$3 O 1.F 1( '
EXAMPLE ;= 4.1
Ans: EXAMPLE
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EXAMPLE ;= 4.1
Ans: EXAMPLE
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80a+le :
EXE7/+8E 1
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A buffer solution is #re#ared by iing I(( L of 1.'( ?
5$Il solution wit J(( L of (.1( ? 5$3.
i. alculate te #$ of a te buffer solution.ii. alculate te #$ of te buffer solution after te
addition ofa) (.1' ? 5a%$b) (.(11 ? $
Assue tat te *olue of te solution does not
cange wen $l and 5a%$ is added)K b for 5$3 O 1.F 1(-' ?
Ans: EXE7/+8E 1
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Ans: EXE7/+8E 1
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Ans: EXE7/+8E 1
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Ans: EXE7/+8E 1
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7.2 :
ACID-BASE
TITRATION
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Describe the titration process and distinguish the
end point and equivalence point.
Sk tch and int rpr t th variation pH against titr valu for
titration b tw n :
i. strong acid- strong bas
ii. strong acid-w ak bas
iii. w ak acid-strong bas
Id ntify suitabl indicators for acid-bas titrations.
&M9%"DS
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titration
end #oint
equi*alence #oint
indicators
titration cur*e
ADBAS ;;"A;%5
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A solution of accurately +nown concentration
is added gradually to anoter solution of un+nown concentration until te ceical
reaction neutrali<ation) between te two solutionis co#lete.
ADBAS ;;"A;%5
Burette: t ti f l ti i id
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onical flas+:oncentration of solution inside:un+nown KA?,L: $3%%$a" ))
ndicator:KA?,L:#enol#talein)
Before titrationbegin
After titrationat te end #oint)
oncentration of solution inside:+nown KA?,L: 5a%$a" ))
5DA;%"
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ndicator is a substance tat is generally added to tesolution in te recei*ing *essel an wic undergoessoe sort of colour cange wen reaction is o*er.
A wea+ organic acid tat as different colortan it conjugate base
olor canges occurring o*er a s#ecific andrelati*ely narrow #$ range
#$ "A5
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"ange o*er wic te indicator canges fro
te acid color to te base color
KA?,L:
,enol#talein#$ rangeF.3 [ 1(.(
?etyl orange3.1 [ I.I
?etyl red I.2 [ J.3
Soe oon AcidBase ndicators
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olors and A##roiation #$ "ange ofSoe oon AcidBase ndicators
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?ost indicators a*e a range of about 2 #$ units
acidic basicin
between
678AL5; and 5D,%5;
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;e equi*alent #oint is te #oint at wic teaount of acid and base #resent eactlyneutrali<es one anoter. nuber of oles of %$-
ions and nuber of oles of $@ ions are equal)
;e end #oint of titration is te #oint wen teindicator canges colour.
;;"A;%5 7"8
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Strong Acid Strong Base
9ea+ Acid Strong Base
Strong Acid 9ea+ Base
3 ty#es of acid-base titration :
;;"A;%5 7"8: Strong Acid and Strong Base ea#le: $l and 5a%$
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#$
8olue of 5a%$added L)
iter etyl red or #enol#talein is a suitable indicator because eac canges color on te
stee# #ortion of te cur*e
,enol#talein
#$ range
F.3 [ 1(.(
?etyl red I.2 [ J.3
9A& ADS;"%5 BAS 7"8S
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;ree different wit strong acidstrong base:
nitial #$ is iger
9ea+ acid dissociates sligtly
radual rising #ortion buffer region
?iture of acid and salt
$AUA buffer syste #roduced
#$ at equi*alence #oint 4.((
Salts of wea+ acid and strong base
a#le: $3%%
5a@
) is basic in water
;;"A;%5 7"8: 9ea+ Acid and Strong Base ea#le $3%%$ and 5a%$)
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,enol#talein is a suitable indicator because itcanges color on te stee# #ortion of te cur*e! butetyl red is not its color canges o*er a large
*olue range
,enol#talein
#$ range
F.3 [ 1(.(
?etyl red I.2 [ J.3#$
S;"%5 AD9A& BAS 7"8S
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KA?,L: 5$3a" ) in conical flas+
$la" ) in burette
nitial solution O wea+ base #$ 4.((
radual rising #ortion buffer region ?iture of base 5$3) and salt 5$I
@)
#$ at equi*alence #oint Q 4.((
Salt 5$I@l ) is acidic in water
#$ decrease slowly as ecess $3%@ is
added
;;"A;%5 7"8: Strong Acid and 9ea+ Base ea#le: $l and 5$3 )
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?etyl red is a suitable indicator because it cangescolor on te stee# #ortion of te cur*e! but#enol#atalein is not its color canges o*er a large
*olue range
,enol#talein
#$ range
F.3 [ 1(.(
?etyl red I.2 [ J.3
#$
EXAMPLE
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S+etc titration cur*es for te following
acidbase titrations:
a) $l *ersus 5a%$b) $l *ersus $35$2
c) $3%%$ *ersus 5a%$
n eac case! te base is added to te acidin a conical flas+. Mour gra# sould sow
#$ on te yais and *olue of base addedon te ais.
Ans: EXAMPLE
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#$
8olue of
5a%$ added
4.(( equi*alence#oint
a) ;itration cur*e: $l *ersus 5a%$
Ans: EXAMPLE
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#$
8olue of
5a%$ added
Q 4.((
buffer region
b) ;itration cur*e: $l *ersus $35$2
equi*alence#oint
Ans: EXAMPLE
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#$
8olue of
5a%$ added
4.(( equi*alence#oint
;itration cur*e: $3%%$ *ersus 5a%$
buffer region
EXE7/+8E 4.1
EXE7/+8E 1
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ndicator " range colour change
henolhthalein .% C 45.5
*ethyl orange &.% C .%
Bro+othy+olblue
@.5 C .@
henol red @. C .
1. 9at is te colour of te solution wen 3 dro#s of tebelow indicators are added se#arately to water #$ O 4) >
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Define solubility! olar solubility and solubility#roduct! K s#.
alculate K s# fro concentration of ion and *ice
*ersa ,redict te #ossibility of #reci#itation of sligtly
soluble ionic co#ounds te *alues of ion-#roduct!Q to K s#.
Define and e#lain te coon ion effect. ,erfor calculations related to coon ion effect.
&M9%"DS
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solubility
olar solubility
solubility #roduct K s#)
Q
#reci#itation
coon ion effect
Solubility and ?olar Solubility
Solubility: is te aiu aount of solute g or ole
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Solubility: is te aiu aount of solute g or oleor +g) tat can be dissol*ed in a gi*en quantity of
sol*ent to for a saturated solution at a gi*ente#erature. or ea#leT
Solubility gUL)
ras of solute dissol*ed in 1 L of a saturated
solution ?olar solubility olUL):
?oles of solute dissol*ed in 1 L of a saturatedsolution
8uar (so-ute)
+n !a> a!ount
A cu" ?itter tea
(so-#ent)
@er' sweet tea
(saturated so-ution)
@
S%L7BL;M % SL$;LMS%L7BL %5 %?,%75DS
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,bl2s)
Assu#tion: ;e sall aount of a sligtly
soluble ionic co#ound tat dissol*es in water also dissociates co#letely into ions
Sligtly soluble ,bl2a" )
1((P dissociates into ions
,b2@
a" ) 2l
a" )
,bl2s) ,b2@a" ) @ 2l a" )
KA?,L:
quilibriu eist between solid solute andaqueous ions:
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,bl2s) ,b2@a" ) @ 2l a" )
KA?,L:
Ag2Ss) 2Ag@a" ) @ S2a" )
KA?,L: Saturated solution of Agl in water
S%L7BL;M,"%D7; %5S;A5;! K s#
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KA?,L: Saturated solution of Agl in water
Agls) Ag@a" ) @ l a" )
K s# O /Ag@0 /l 0
An equilibriu constant related to te
equilibriu between solid salt and its ions in solution
ts #ro*ide a quantitati*e easure of te
solubility of a sligtly soluble salt
&s# : ;e #roduct of ion concentrations in saturated
solution! eac raised to te #ower of itsstoicioetric in te equilibriu equation.
S l bl i i d 1(( P l bl d di i t
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Soluble ionic co#ounds 1(( P soluble and dissociatein water) suc as 5al a*e no K s# *alue
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Ans: EXAMPLE
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Ans: EXAMPLE
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Ans: EXAMPLE
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7S5 K s# ;% %?,A" S%L7BL;S
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?g%3s) ?g2@a" ) @ %32a" )
K s# \ Solubility \
KA?,L:
K sp O 3.' 1( F
,bS%Is) ,b2@a" ) @ S%I2a" ) K sp O 1.J 1( F
?g%3
is ore soluble tan ,bS%I
Mou ust co#are K s# of co#ounds
wose forula a*e sae total nuber of ions
AL7LA;%5 58%L85 K s#
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Deterining K s# fro
solubility or olar solubility
Deterining solubility orolar solubility fro K s#
;wo ty#es:
EXAMPLE 1
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A5S:'.( 1( 13
8i-#er &ro!ide, A?r, is the -ihtsensiti#e
co!"ound used in near-' a-- "hotora"hic i-!$ ;e olar solubility of AgBr is 4.1 1( 4 ! .at 2'o. alculate K s# for AgBr at tis
te#erature.
Ans: EXAMPLE 1
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EXAMPLE 2
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A5S:1.3 1( I
;e solubility of sil*er carbonate is
(.(32 ol L 1 at 2(o. alculate te K s# of sil*er carbonate.
Ans: EXAMPLE 2
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EXAMPLE
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;e solubility of calciu sulfate is founde#erientally to be (.J4 gUL.alculate te *alue of K s# for calciu sulfate.
?olar ass of aS%I O 13J.2 gUol)
A5S:
2 I 1( '
Ans: EXAMPLE
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Ans: EXAMPLE
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9en &s# is gi*en!
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EXAMPLE 1
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A5S:1.3 1( ' ol L 1
9at is te olar solubility of Agl in
#ure water at 2'o>K s# of Agl O 1.F 1( 1(
Ans: EXAMPLE 1
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alculate te olar solubility of ,bl
EXAMPLE 2
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alculate te olar solubility of ,bl2.
K s# O 1.J 1( '
A5S:
1 J 1( 2
!
Ans: EXAMPLE 2
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EXE7/+8E 4.1
EXE7/+8E 1
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1. ;e solubility of agnesiu ydroide! ?g%$)2 is
1.4 1(-I ol d-3. alculate te solubility #roduct oftis co#ound.
2. ;e solubility of calciu sulfate! aS%I is founde#erientally to be (.J4 g L-1. alculate te K s# *alue
for aS%I. ?olar ass of aS%I O 13J.2 g ol-1)
3. 1.(( liter of a saturated solution of sil*er croate!Ag2r%I at 2'o contains (.(I3' gra of dissol*ed
Ag2r%I. alculate its olar solubility and its solubility
roduct constant
6 O K s#
+rediction o precipitation, Q s# 8s. K s#
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s#
- te solution is saturated
- equilibriu eist between undisol*esolid salt and its dissol*ed ions
6 Q K s#
- te solution is unsaturated- no #reci#itation of ?A- ore salt sould be dissol*ed to increase
te ion concentrations until 6 O K s#
6 K s#
- te solution is su#ersaturated- ?As) will #reci#itate out until te #roduct
of te ionic concentrations is equal to Ks#
?ore solid candissol*e =
EXAMPLE 1
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A5S:,reci#itate will for until Q
s#
O K s#
9ill a #reci#itate of aS%I for in a solution
if te a2@ concentration is (.((2' ! and teS%I
2 concentration is (.(3( ! >
K s# of aS%I O 2.I 1( ')
Ans: EXAMPLE 1
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9 ibl i i i f b
EXAMPLE 2
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9at #ossible #reci#itate igt for by
iing '(.( L of 1.( 1( I ! 5al wit'(.( L of 1.( 1( J ! Ag5%3> 9ill it for>
K s# of Agl O 1.F 1( 1()
A5S:Q s# O 2.' 1( 11
Agl #reci#itate will not for
Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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%??%5 %5 ;
Sift of equilibriu caused by addition or te
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Sift of equilibriu caused by addition or te
te #resence of a co#ound a*ing an ion incoon wit te dissol*ed substance
,br%Is) ,b2@a" ) @ r%I2a" )
Add r%I2
KA?,L:
,resence of a coon ion decreases solubility
; % %??%5 %5%5 S%L7BL;M
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,resence of a coon ion decreases solubility
of sligtly soluble ionic co#oundKA?,L: Addition of 5a2r%I soluble salt) to
saturated solution of ,br%I
,br%Is) ,b2@a" ) @ r%I2a" )
K s# O /,b2@0/r%I20 O 2.3 1(-13
Add r%I2-
ffect of te addition of coon ion r%I2 :
/r%I20 \ Soe r%I
2 cobine wit
,b2@ to for solid ,br%I
Solubility of ,br%I ]
,b2@
,br%I
Add r%I2
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,b
r%I2
,br%I
,b2@
r%I2
,br%I
,br%I dissol*es in 5a2r%I solution
;e sae results if:
Soluble lead )salt suc as ,b5%3)2 is added
9at is te olar solubility of AgBr in
EXAMPLE 1
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9at is te olar solubility of AgBr in
a) #ure waterb) (.((1( ! 5aBr >.
K s# of AgBr O 4.4 1( 13
A5S:a) F.F 1( 4 !
b) 4.4 1( 1( !
Ans: EXAMPLE 1
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Ans: EXAMPLE 1
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l l t t l bilit f il l id
EXAMPLE 2
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A5S:a) 1.F 1( 3 gULb) 3.J 1( J gUL
alculate te solubility of sil*er cloride
in gUL) in
a) #ure water b) a J.' 1( 3 ! sil*er nitrate solution
K s# of Agl O 1.J 1( 1(
Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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Ans: EXAMPLE 2
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1 t f d i t ll t t t l bilit f
EXAMPLE
EXE7/+8E 4.1
EXE7/+8E 1
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1. t was found e#erientally tat te solubility of
calciu sul#ate is (.J4 g L-1. alculate te K s# forcalciu sul#ate. 2.I 1(-I )
2. ;e solubility of sil*er sul#ate is 1.' 1(-2 ol L-1.alculate te solubility #roduct of te salt. 1.I 1(-' )
3. 9ill #reci#itate for if 2(( L of (.((I( ? Bal2 areadded to J(( L of (.((F( ? &2S%I > K s# BaS%I O 1.1
1(-1() 6 K s# terefore BaS%I will #reci#itate)
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&idney Stone
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Are #ains sooting troug your body tat are so se*ere tat tey cause you to curl u# in #ain>
Does your lower bac+ feel li+e being stabbed o*er and o*er again wit
a ot +nife>
Are your #ains so se*ere tat a+e you feel nauseous or e*en cause
you to *oit>
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a2@a" ) @ 2%I2a" ) a2%Is)
;e noral #ysiological concentration of calciu ions in blood #lasa is about ' !
%alate ion 2%I2)! deri*ed fro oalic acid #resent
in any *egetables suc as rubarb and s#inac! reac wit calciu ions to for insoluble calciu oalate! wic can gradually build u# in te +idneys
8/16/2019 7.0 Ionic Equilibria (Students)
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