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Acid-Base Equilibria andSolubility Equilibria
Chapter 17
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
산 - 염기 평형과 용해도 평형
1. 균일 대 불균일 용액 평형2. 완충용액3. 산 - 염기 적정 - 당량점4. 산 - 염기 지시약 - 종말점5. 용해도 평형6. 공통이온 효과와 용해도7. 착이온 평형과 용해도8. 정성분석에 대한 용해도곱 원리의 응용
The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
The presence of a common ion suppresses the ionization of a weak acid or a weak base.
Consider mixture of CH3COONa (strong electrolyte) and CH3COOH (weak acid).
CH3COONa (s) Na+ (aq) + CH3COO- (aq)
CH3COOH (aq) H+ (aq) + CH3COO- (aq)
common ion
Consider mixture of salt NaA and weak acid HA.
HA (aq) H+ (aq) + A- (aq)
NaA (s) Na+ (aq) + A- (aq)Ka =
[H+][A-][HA]
[H+] =Ka [HA]
[A-]
-log [H+] = -log Ka - log[HA]
[A-]
-log [H+] = -log Ka + log [A-][HA]
pH = pKa + log [A-][HA]
pKa = -log Ka
Henderson-Hasselbalch equation
pH = pKa + log[conjugate base]
[acid]
What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK?
Common ion effect
0.30 – x 0.30
0.52 + x 0.52
pH = pKa + log [HCOO-][HCOOH]
HCOOH pKa = 3.77
pH = 3.77 + log[0.52][0.30]
= 4.01
HCOOH (aq) H+ (aq) + HCOO- (aq)
Initial (M)
Change (M)
Equilibrium (M)
0.30 0.00
-x +x
0.30 - x
0.52
+x
x 0.52 + x
Mixture of weak acid and conjugate base!
A buffer solution ( 완충용액 ) is a solution of:
1. A weak acid or a weak base and
2. The salt of the weak acid or weak base
Both must be present!
A buffer solution has the ability to resist changes in pH upon the addition of small amounts of either acid or base.
Add strong acid
H+ (aq) + CH3COO- (aq) CH3COOH (aq)
Add strong base
OH- (aq) + CH3COOH (aq) CH3COO- (aq) + H2O (l)
Consider an equal molar mixture of CH3COOH and CH3COONa
Pure water
0.005/0.005 AcH/Ac buffer
20 mL acetic acid/acetate(5/5 mM) buffer and water,With 0.1M HCl or 0.1 M NaOH
With 0.1M HCl 0.1 M NaOH
Which of the following are buffer systems? (a) KF/HF (b) KBr/HBr, (c) Na2CO3/NaHCO3
(a) KF is a weak acid and F- is its conjugate base buffer solution
(b) HBr is a strong acidnot a buffer solution
(c) CO32- is a weak base and HCO3
- is it conjugate acidbuffer solution
Calculate the pH of the 0.30 M NH3/0.36 M NH4Cl buffer system. What is the pH after the addition of 20.0 mL of 0.050 M NaOH to 80.0 mL of the buffer solution?
NH4+ (aq) H+ (aq) + NH3 (aq)
= 9.20
pH = pKa + log[NH3][NH4
+]pKa = 9.25 pH = 9.25 + log
[0.30][0.36]
= 9.17
NH4+ (aq) + OH- (aq) H2O (l) + NH3 (aq)
start (moles)
end (moles)
0.029 0.001 0.024
0.028 0.0 0.025
pH = 9.25 + log[0.25][0.28]
[NH4+] =
0.0280.10
final volume = 80.0 mL + 20.0 mL = 100 mL
[NH3] = 0.0250.10
Chemistry In Action: Maintaining the pH of Blood
Titrations( 적정 , 滴定 )
Equivalence point( 당량점 ) – the point at which the reaction is complete
Indicator – substance that changes color at (or near) the equivalence point
Slowly add known titrant to unknown solution(titrand)UNTIL
the indicator changes color
물방울목적 : 당량점을 찾아내는 것
방법 : 종말점을 이용한다
End point( 종말점 ) – the point at which the indicator changes color
Strong Acid-Strong Base Titrations
NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)
OH- (aq) + H+ (aq) H2O (l)equivalence point
•
phenolphthalein
phenolphthalein
methyl orange
methyl orange
Weak Acid-Strong Base Titrations
CH3COOH (aq) + NaOH (aq) CH3COONa (aq) + H2O (l)
CH3COOH (aq) + OH- (aq) CH3COO- (aq) + H2O (l)
CH3COO- (aq) + H2O (l) OH- (aq) + CH3COOH (aq)
At equivalence point (pH > 7):
18.919 6.00019.297 6.19519.545 6.39019.707 6.58519.812 6.78019.880 6.97519.923 7.17019.951 7.36519.969 7.56019.980 7.75519.988 7.95019.992 8.14519.996 8.34019.998 8.53520.000 8.73020.002 8.92520.004 9.12020.008 9.31420.013 9.50920.020 9.70420.032 9.89920.050 10.09420.079 10.28920.123 10.48420.193 10.67920.304 10.87420.478 11.06920.754 11.264 equivalence point
•
phenolphthaleinphenolphthalein
methyl orange
methyl orange
Strong Acid-Weak Base Titrations
HCl (aq) + NH3 (aq) NH4Cl (aq)
NH4+ (aq) + H2O (l) NH3 (aq) + H+ (aq)
At equivalence point (pH < 7):
H+ (aq) + NH3 (aq) NH4+ (aq)
equivalence point
•
phenolphthalein
phenolphthalein
methyl orangemethyl orange
Exactly 100 mL of 0.10 M HNO2 are titrated with a 0.10 M NaOH solution. What is the pH at the equivalence point ?
0.01
HNO2 (aq) + OH- (aq) NO2- (aq) + H2O (l)
start (moles)
end (moles)
0.01
0.0 0.0 0.01
NO2- (aq) + H2O (l) OH- (aq) + HNO2 (aq)
Initial (M)
Change (M)
Equilibrium (M)
0.05 0.00
-x +x
0.05 - x
0.00
+x
x x
[NO2-] =
0.010.200 = 0.05 MFinal volume = 200 mL
Kb =[OH-][HNO2]
[NO2-]
=x2
0.05-x= 2.2 x 10-11
0.05 – x 0.05 x 1.05 x 10-6 = [OH-]
pOH = 5.98
pH = 14 – pOH = 8.02
Exactly 100 mL of 0.10 M HNO2 are titrated with a 0.10 M NaOH solution. What is the pH at the equivalence point ?
NO2- (aq) + H2O (l) OH- (aq) + HNO2
(aq)
Initial (M)
Change (M)
Eq (M)
0.05 0.00
-x +x+y
0.05 - x
0.00
+x
x+y x
Kb =[OH-][HNO2]
[NO2-]
=x(x+y)0.05-x
= 2.2 x 10-11
0.05 – x 0.05 x 1.05 x 10-6 = [OH-]
pOH = 5.98
pH = 14 – pOH = 8.02
H2O (l) OH- (aq) + H+(aq)
0.00
y
Kw = [OH-][H+] = y(x+y) = 1.0x 10-14
Acid-Base Indicators
HIn (aq) H+ (aq) + In- (aq)
10[HIn]
[In-]Color of acid (HIn) predominates
10[HIn]
[In-]Color of conjugate base (In-) predominates
Red cabbage juice and pH
pH
Phenolphthalein
HIn In-
Indicator Low pH colorTransition pH range
High pH color
Thymol blue (first transition) red 1.2–2.8 yellow
Thymol blue (second transition) yellow 8.0–9.6 blue
Methyl yellow red 2.9–4.0 yellow
Bromophenol blue yellow 3.0–4.6 purple
Congo red blue-violet 3.0–5.0 red
Methyl orange red 3.1–4.4 orange
Bromocresol green yellow 3.8–5.4 blue-green
Methyl red red 4.4–6.2 yellow
Bromocresol purple yellow 5.2–6.8 purple
Bromothymol blue yellow 6.0–7.6 blue
Phenol red yellow 6.8–8.4 red
Naphtholphthalein colorless to reddish 7.3–8.7 greenish to blue
Cresol Red yellow 7.2–8.8 reddish-purple
Phenolphthalein colorless 8.3–10.0 fuchsia
Thymolphthalein colorless 9.3–10.5 blue
Alizarine Yellow R yellow 10.2–12.0 red
Litmus red 4.5-8.3 blue
Which indicator(s) would you use for a titration of HNO2 with KOH ?
Weak acid titrated with strong base.
At equivalence point, will have conjugate base of weak acid.
At equivalence point, pH > 7
Use cresol red or phenolphthalein
Solubility Equilibria
AgCl (s) Ag+ (aq) + Cl- (aq)
Ksp = [Ag+][Cl-] Ksp is the solubility product constant
MgF2 (s) Mg2+ (aq) + 2F- (aq) Ksp = [Mg2+][F-]2
Ag2CO3 (s) 2Ag+ (aq) + CO32- (aq) Ksp = [Ag+]2[CO3
2-]
Ca3(PO4)2 (s) 3Ca2+ (aq) + 2PO43- (aq) Ksp = [Ca2+]3[PO3
3-]2
Dissolution of an ionic solid in aqueous solution:
Q = Ksp Saturated solution
Q < Ksp Unsaturated solution No precipitate
Q > Ksp Supersaturated solution Precipitate will form
4.2
Na+ K+ NH4+ Al3+ H+ Mg2+ Ca2+ Sr2+ Ba2+ Cr3+ Fe3+ Fe2+ Co2+ Ni2+ Cu2+ Zn2+ Cd2+ Hg2+ Hg2
2+ Ag+ Pb2+ As3+ Sb3+ Bi3+
CH3CO2- S S S S S S S S S S U S S S S S S S I I S U U I
Br- S S S S S S S S S S S S S S S S S I Ia Ib I D D D
Cl- S S S S S S S S S S S S S S S S S S Ib Ib I D S D
I- S S S S S S S S S I U S S S U S S Ia Ia I Ia S D I
ClO3- S S S S S S S S S U U U S I S S S S S S S U U U
NO3- S S S S S S S S S S S S S S S S S S D S S U U D
CrO42- S S S U S S S Ia Ia U S I I U S Ia I Ia Ia Ia Ia U U U
SO42- S S S S S S Ia I Ib S S S S S S S S D I I I U D D
SO32- S S S U S S I I I I U I I I U I I U U I I U U U
C2O42- S S I I S I I I I S S I I I I I I I I I I U I D
PO43- S S S Ia S Ia Ia Ia Ia I Ia Ia I I Ia Ia I U U Ia Ia U U I
CO32- S S S U S Ia I Ia I U U I I I I Ia I I Ia Ia Ia U U U
SiO32- S S U I I Ia Ia Ia S U U I I U U Ia I U U U Ia U U I
O2- D D U Ib H2O Ia I I S I Ia Ia I I Ia I I I Ia I I I I I
OH- S S U Ia H2O Ia Ia I S I Ia Ia I I Ia Ia I U U U Ia U U D
S2- S S S D S D Ia I D I I Ia I I Ia Ia I I I Ia Ia I D I
Ia Soluble in AcidsIb Slightly Soluble in Acids
H2O Produces water
S Soluble I InsolubleD=Decomposes in
waterU=Compound does not exist or is
unstable
Solubility of Ionic Compounds in Water
Salt Ksp Salt Ksp Salt Ksp
Bromides Carbonates Oxalates
PbBr2 6.6 x 10-6 MgCO3 6.8 x 10-6 MgC2O4 4.8 x 10-6
CuBr 6.3 x 10-9 NiCO3 1.3 x 10-7 FeC2O4 2 x 10-7
AgBr 5.4 x 10-13 CaCO3 5.0 x 10-9 NiC2O4 1 x 10-7
Hg2Br2 6.4 x 10-23 SrCO3 5.6 x 10-10 SrC2O4 5 x 10-8
Chlorides MnCO3 2.2 x 10-11 CuC2O4 3 x 10-8
PbCl2 1.2 x 10-5 CuCO3 2.5 x 10-10 BaC2O4 1.6 x 10-7
CuCl 1.7 x 10-7 CoCO3 1.0 x 10-10 CdC2O4 1.4 x 10-8
AgCl 1.8 x 10-10 FeCO3 2.1 x 10-11 ZnC2O4 1.4 x 10-9
Hg2Cl2 1.4 x 10-18 ZnCO3 1.2 x 10-10 CaC2O4 2.3 x 10-9
Fluorides Ag2CO3 8.1 x 10-12 Ag2C2O4 3.5 x 10-11
BaF2 1.8 x 10-7 CdCO3 6.2 x 10-12 PbC2O4 4.8 x 10-12
MgF2 7.4 x 10-11 PbCO3 7.4 x 10-14 Hg2C2O4 1.8 x 10-13
SrF2 2.5 x 10-9 Hydroxides MnC2O4 1 x 10-15
CaF2 1.5 x 10-10 Ba(OH)2 5.0 x 10-3 Phosphates
Iodides Sr(OH)2 6.4 x 10-3 Ag3PO4 8.9 x 10-17
PbI2 8.5 x 10-9 Ca(OH)2 4.7 x 10-6 AlPO4 9.8 x 10-21
CuI 1.1 x 10-12 Mg(OH)2 5.6 x 10-12 Mn3(PO4)2 1 x 10-22
AgI 8.5 x 10-17 Mn(OH)2 2.1 x 10-13 Ba3(PO4)2 3 x 10-23
Hg2I2 4.5 x 10-29 Cd(OH)2 5.3 x 10-15 BiPO4 1.3 x 10-23
Sulfates Pb(OH)2 1.2 x 10-15 Sr3(PO4)2 4 x 10-28
CaSO4 7.1 x 10-5 Fe(OH)2 4.9 x 10-17 Pb3(PO4)2 7.9 x 10-43
Ag2SO4 1.2 x 10-5 Ni(OH)2 5.5 x 10-16 Chromates
Hg2SO4 6.8 x 10-7 Co(OH)2 1.1 x 10-15 CaCrO4 7.1 x 10-4
SrSO4 3.5 x 10-7 Zn(OH)2 4.1 x 10-17 SrCrO4 2.2 x 10-5
PbSO4 1.8 x 10-8 Cu(OH)2 1.6 x 10-19 Hg2CrO4 2.0 x 10-9
BaSO4 1.1 x 10-10 Hg(OH)2 3.1 x 10-26 BaCrO4 1.2 x 10-10
Acetates Sn(OH)2 5.4 x 10-27 Ag2CrO4 2.0 x 10-12
Ag(CH3COO) 4.4 x 10-3 Cr(OH)3 6.7 x 10-31 PbCrO4 2.8 x 10-13
Hg2(CH3COO)2 4 x 10-10 Al(OH)3 1.9 x 10-33
Fe(OH)3 2.6 x 10-39
So
lub
ilit
y P
rod
uct
Co
nst
ant
(Ksp
) V
alu
es a
t 25
oC
Molar solubility (mol/L) is the number of moles of solute dissolved in 1 L of a saturated solution.
Solubility (g/L) is the number of grams of solute dissolved in 1 L of a saturated solution.
What is the solubility of silver chloride in g/L ?Ksp = 1.6x10-10, M(AgCl) = 143.35
0.00AgCl (s) Ag+ (aq) + Cl- (aq)
Ksp = [Ag+][Cl-]Initial (M)
Change (M)
Equilibrium (M)
+s
0.00
+s
s s
Ksp = s2
s = Ksps = 1.3 x 10-5
[Ag+] = 1.3 x 10-5 M [Cl-] = 1.3 x 10-5 M
Solubility of AgCl = 1.3 x 10-5 mol AgCl
1 L soln143.35 g AgCl
1 mol AgClx = 1.9 x 10-3 g/L
Ksp = 1.6 x 10-10
If 2.00 mL of 0.200 M NaOH are added to 1.00 L of 0.100 M CaCl2, will a precipitate form? Ksp = 8.0x10-6
The ions present in solution are Na+, OH-, Ca2+, Cl-.
Only possible precipitate is Ca(OH)2 (solubility rules).
Is Q > Ksp for Ca(OH)2?
[Ca2+]0 = 0.100 M [OH-]0 = 4.0 x 10-4 M
Ksp = [Ca2+][OH-]2 = 8.0 x 10-6
Q = [Ca2+]0[OH-]02 = 0.10 x (4.0 x 10-4)2 = 1.6 x 10-8
Q < Ksp No precipitate will form
What concentration of Ag is required to precipitate ONLY AgBr in a solution that contains both Br- and Cl- at a concentration of 0.02 M? Ksp = 7.7x10-13
AgCl (s) Ag+ (aq) + Cl- (aq)
Ksp = [Ag+][Cl-]
Ksp = 1.6 x 10-10
AgBr (s) Ag+ (aq) + Br- (aq) Ksp = 7.7 x 10-13
Ksp = [Ag+][Br-]
[Ag+] = Ksp
[Br-]7.7 x 10-13
0.020= = 3.9 x 10-11 M
[Ag+] = Ksp
[Br-]1.6 x 10-10
0.020= = 8.0 x 10-9 M
3.9 x 10-11 M < [Ag+] < 8.0 x 10-9 M
The Common Ion Effect and Solubility
The presence of a common ion decreases the solubility of the salt.
What is the molar solubility of AgBr in (a) pure water and (b) 0.0010 M NaBr? Ksp = 7.7x10-13
AgBr (s) Ag+ (aq) + Br- (aq)
Ksp = 7.7 x 10-13
s2 = Ksp
s = 8.8 x 10-7
NaBr (s) Na+ (aq) + Br- (aq)
[Br-] = 0.0010 M
AgBr (s) Ag+ (aq) + Br- (aq)
[Ag+] = s
[Br-] = 0.0010 + s 0.0010
Ksp = 0.0010 x s
s = 7.7 x 10-10
16.8
pH and Solubility
• The presence of a common ion decreases the solubility.• Insoluble bases dissolve in acidic solutions• Insoluble acids dissolve in basic solutions
Mg(OH)2 (s) Mg2+ (aq) + 2OH- (aq)
Ksp = [Mg2+][OH-]2 = 1.2 x 10-11
Ksp = (s)(2s)2 = 4s3
4s3 = 1.2 x 10-11
s = 1.4 x 10-4 M
[OH-] = 2s = 2.8 x 10-4 M
pOH = 3.55 pH = 10.45
At pH less than 10.45
Lower [OH-]
OH- (aq) + H+ (aq) H2O (l)
Increase solubility of Mg(OH)2
At pH greater than 10.45
Raise [OH-]
Decrease solubility of Mg(OH)2
Complex Ion Equilibria and Solubility
A complex ion is an ion containing a central metal cation bonded to one or more molecules or ions.
Co2+ (aq) + 4Cl- (aq) CoCl4 (aq)2-
Kf =[CoCl4 ]
[Co2+][Cl-]4
2-
The formation constant or stability constant (Kf) is the equilibrium constant for the complex ion formation.
Co(H2O)62+ CoCl4
2-
Kf
stability of complex
Qualitative Analysis of
Cations
Flame Test for Cations
lithium sodium potassium copper
Chemistry In Action: How an Eggshell is Formed
Ca2+ (aq) + CO32- (aq) CaCO3 (s)
H2CO3 (aq) H+ (aq) + HCO3- (aq)
HCO3- (aq) H+ (aq) + CO3
2- (aq)
CO2 (g) + H2O (l) H2CO3 (aq)carbonic
anhydrase