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Acids and Bases
Autoionization of Water and the pH Scale
H2O(l) H2O(l)
H3O+(aq) OH-(aq)
+
+
The nature of the hydrated proton.
Brønsted-Lowry Acid-Base Definition
An acid is a proton donor, any species which donates a H+.
A base is a proton acceptor, any species which accepts a H+.
+O H
H
H
H
H
H + N+O
H
N H
H
H
+H H
+ -O H
H
OH
H
O HH + +O H H
Strong acid: HA(g or l) + H2O(l) H2O+(aq) + A-(aq)
The extent of dissociation for strong and weak acids
The extent of dissociation for strong and weak acids
Weak acid: HA(aq) + H2O(l) H2O+(aq) + A-(aq)
The Acid-Dissociation Constant
Weak acids dissociate very slightly into ions in water.
Strong acids dissociate completely into ions in water.
HA(g or l) + H2O(l) H3O+(aq) + A-(aq)
HA(aq) + H2O(l) H3O+(aq) + A-(aq)
Kc >> 1
Kc << 1
Kc = [H3O+][A-]
[H2O][HA]
Kc[H2O] = Ka =[H3O+][A-]
[HA]
stronger acid higher [H3O+]
larger Ka
smaller Ka lower [H3O+]
weaker acid
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Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Kc = [H3O+][OH-]
[H2O]2
Kc[H2O]2 = [H3O+][OH-]
The Ion-Product Constant for Water
Kw =
A change in [H3O+] causes an inverse change in [OH-].
= 1.0 x 10-14 at 250C
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
In an acidic solution, [H3O+] > [OH-]
In a basic solution, [H3O+] < [OH-]
In a neutral solution, [H3O+] = [OH-]
The relationship between [H3O+] and [OH-] and the relative acidity of solutions.
[H3O+] [OH-]Divide into Kw
ACIDIC SOLUTION
BASIC SOLUTION
[H3O+] > [OH-] [H3O+] = [OH-] [H3O+] < [OH-]
NEUTRAL SOLUTION
The pH values of some familiar
aqueous solutions
pH = -log [H3O+]
Th
e re
lati
on
s a
mo
ng
[H
3O
+],
pH
, [O
H- ],
an
d p
OH
Acid/Base Activity Calculating [H3O+], pH, [OH-], and pOH
PROBLEM: In a restoration project, a conservator prepares copper-plate etching solutions by diluting concentrated HNO3 to 2.0M, 0.30M, and 0.0063M HNO3. Calculate [H3O+], pH, [OH-], and pOH of the three solutions at 250C.
Important pKa values to know
Compound Structure pKa
Alkanes (sp3)51
Alkenes44
Alkynes25
Amines33-35
Alcohols15-19
Water15.7
Carboxylic acids3-5
Special Carboxylic acids
-0.2
Strong AcidsHBrHCl
H2SO4
-9-7-5.2 (first ionization)
C H
H
H
H
H
HH
H
HH
N H
H
R
RO
H
OH H
O
ORH
O
OH
FF
F
Brønsted-Lowry Acid-Base Definition
An acid-base reaction can now be viewed from the standpoint of the reactants AND the products.
An acid reactant will produce a base product and the two will constitute an acid-base conjugate pair.
An acid is a proton donor, any species which donates a H+.
A base is a proton acceptor, any species which accepts a H+.
Proton transfer as the essential feature of a Brønsted-Lowry acid-base reaction
(acid, H+ donor) (base, H+ acceptor)
HCl H2O
+
Cl- H3O+
+
Lone pair binds H+
(base, H+ acceptor) (acid, H+ donor)
NH3 H2O
+
NH4+ OH-
+
Lone pair binds H+
The Conjugate Pairs in Some Acid-Base Reactions
Base Acid+Acid Base+
Conjugate Pair
Conjugate Pair
Reaction 4 H2PO4- OH-+
Reaction 5 H2SO4 N2H5++
Reaction 6 HPO42- SO3
2-+
Reaction 1 HF H2O+ F- H3O++
Reaction 3 NH4+ CO3
2-+
Reaction 2 HCOOH CN-+ HCOO- HCN+
NH3 HCO3-+
HPO42- H2O+
HSO4- N2H6
2++
PO43- HSO3
-+
Acid/Base Activity Identifying Conjugate Acid-Base Pairs
PROBLEM: The following reactions are important environmental processes. Identify the conjugate acid-base pairs.
(a) H2PO4-(aq) + CO3
2-(aq) HPO42-(aq) + HCO3
-(aq)
(b) H2O(l) + SO32-(aq) OH-(aq) + HSO3
-(aq)
Strengths of conjugate acid-
base pairs
HI I-
HBr Br-
HCl Cl-
H2SO4 HSO4-
H2OH3O+
H3PO4 H2PO4-
C6H5COOH C6H5COO-
CH3COOH CH3COO-
H2CO3 HCO3-
H2S HS-
NH3NH4+
C6H5OH C6H5O-
HCO3-
CO32-
CH3NH2CH3NH3+
H2O HO-
CH3CH2OH CH3CH2O-
HC CH HC C-H2 H-NH3 NH2
-CH2=CH2 CH2=CH
-CH3CH3 CH3CH2
-Acid Formula pKa Conjugate BaseEthane
Ammonia
EthanolWater
Bicarbonate ionPhenol
Ammonium ion
Carbonic acidAcetic acid
3525
Benzoic acidPhosphoric acid
Sulfuric acidHydrogen chlorideHydrogen bromideHydrogen iodide
51
38
10.33
15.715.9
4.766.36
9.24
9.95
-5.2-7
-9-8
4.19
2.1-1.74Hydronium ion
Strongerconjugate
base
Weakerconjugate
base
Weaker acid
Stronger acid
Methylammonium ion 10.64
Hydrogen sulfide 7.04
AcetyleneHydrogen
Ethylene 44
3.18 HF
Equilibrium favors reaction of the stronger acid and stronger base to give the weaker acid and weaker base
+ +CH3 CO
O HCH3 C
O
O
N HH
HN H
H
HH
ammoniumacetate ionpKa 4.76 pKa 9.24
acetic acid + sodium bicarbonate (omit Na+ )
6.36pKa= 4.76
CO2
H2O++CH3 C
O
O
C O-H
O
O
H
+CH3 CO
O H
C O-H
O
O
Acid/Base Activity Predicting the K Acid-Base Reaction“Will this deprotonate that”
PROBLEM: Predict the net direction and whether Ka is greater or less than 1 for each of the following reactions (assume equal initial concentrations of all species):
(b) H2O(l) + HS-(aq) OH-(aq) + H2S(aq)
(a) H2PO4-(aq) + NH3(aq) HPO4
2-(aq) + NH4+(aq)
In Class
a) You smell ammonia when NH3 dissolves in water
Use balanced equations showing the net direction of the reaction to describe each of the following observations.
b) The odor goes away when you add an excess of HCl to the solution in part a)
c) The odor returns when you add an excess of NaOH to the solution in part b)
Acid/Base Activity Finding the Ka of a Weak Acid from the pH of
Its Solution
PROBLEM: Phenylacetic acid (C6H5CH2COOH, simplified here as HPAc) builds up in the blood of persons with phenylketonuria, an inherited disorder that, if untreated, causes mental retardation and death. A study of the acid shows that the pH of 0.12M HPAc is 2.60. What is the Ka of phenylacetic acid?
Acid/Base Activity Determining Concentrations from Ka and
Initial [HA]
PROBLEM: Propanoic acid (CH3CH2COOH, which we simplify and HPr) is an organic acid whose salts are used to retard mold growth in foods. What is the [H3O+] of 0.10M HPr (Ka = 1.3x10-5)?
Percent HA dissociation = [HA]dissociated
[HA]initial
x 100
Polyprotic acids
acids with more than more ionizable proton
H3PO4(aq) + H2O(l) H2PO4-(aq) + H3O+(aq)
H2PO4-(aq) + H2O(l) HPO4
2-(aq) + H3O+(aq)
HPO42-(aq) + H2O(l) PO4
3-(aq) + H3O+(aq)
Ka1 =[H3O+][H2PO4
-]
[H3PO4]
Ka2 =[H3O+][HPO4
2-]
[H2PO4-]
Ka3 =[H3O+][PO4
3-]
[HPO42-]
Ka1 > Ka2 > Ka3
= 7.2x10-3
= 6.3x10-8
= 4.2x10-13
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Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acid/Base Activity Calculating Equilibrium Concentrations for a Polyprotic Acid
PROBLEM: Ascorbic acid (H2C6H6O6; H2Asc for this problem), known as vitamin C, is a diprotic acid (Ka1 = 1.0x10-5 and Ka2 = 5x10-12) found in citrus fruit. Calculate [H2Asc], [HAsc-], [Asc2-], and the pH of 0.050M H2Asc.
+
CH3NH3+ OH-
methylammonium ion
Abstraction of a proton from water by methylamine
+
CH3NH2H2O
methylamine
Lone pair binds H+
BA
SE
ST
RE
NG
TH
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acid/Base Activity Determining pH from Kb and Initial [B]
PROBLEM: Dimethylamine, (CH3)2NH, a key intermediate in detergent manufacture, has a Kb of 5.9x10-4. What is the pH of 1.5M (CH3)2NH?
Acid/Base Activity Determining the pH of a Solution of A-
PROBLEM: Sodium acetate (CH3COONa, or NaAc for this problem) has applications in photographic development and textile dyeing. What is the pH of 0.25M NaAc? Ka of acetic acid (HAc) is 1.8x10-5.
The effect of atomic and molecular properties on nonmetal hydride acidity.
6A(16)
H2O
H2S
H2Se
H2Te
7A(17)
HF
HCl
HBr
HI
Electronegativity increases, acidity increases
Bon
d st
reng
th d
ecre
ases
, ac
idity
incr
ease
s
H O I H O Br H O Cl< <
H O Cl
O
O
O<<
The relative strengths of oxoacids
H O Cl
Free Ion Hydrated Ion Ka
Fe3+
Sn2+
Cr3+
Al3+
Be2+
Cu2+
Pb2+
Zn2+
Co2+
Ni2+
Fe(H2O)63+(aq)
Sn(H2O)62+(aq)
Cr(H2O)63+(aq)
Al(H2O)63+(aq)
Be(H2O)42+(aq)
Cu(H2O)62+(aq)
Pb(H2O)62+(aq)
Zn(H2O)62+(aq)
Co(H2O)62+(aq)
Ni(H2O)62+(aq)
6 x 10-3
4 x 10-4
1 x 10-4
1 x 10-5
4 x 10-6
3 x 10-8
3 x 10-8
1 x 10-9
2 x 10-10
1 x 10-10
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Ka Values of Some Hydrated Metal Ions at 250C
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Al(H2O)5OH2+Al(H2O)63+
The acidic behavior of the hydrated Al3+ ion
H2O H3O+
Electron density drawn toward Al3+
Nearby H2O acts as base
Acid/Base Activity Predicting Relative Acidity of Salt Solutions
PROBLEM: Predict whether aqueous solutions of the following are acidic, basic, or neutral, and write an equation for the reaction of any ion with water:
(a) Potassium perchlorate, KClO4 (b) Sodium benzoate, C6H5COONa
(c) Chromium trichloride, CrCl3 (d) Sodium hydrogen sulfate, NaHSO4
Acid/Base Activity Predicting the Relative Acidity of Salt Solutions from Ka and Kb of the Ions
PROBLEM: Determine whether an aqueous solution of zinc formate, Zn(HCOO)2, is acidic, basic, or neutral.
Molecular Structure and AcidityMolecular Structure and Acidity
relative acidities the more A:(-) stable, greater the acidity of H-A
Ways to stabilize A:(-) the negative charge
ON a more electronegative atomON larger atomRESONANCE delocalized STABILIZED by inductive effectIN an orbital with more s character
+ +CH3 CO
O HCH3 C
O
O
N HH
HN H
H
HH
A:-A-H :B H-B+
within a period - the greater the electronegativity of A:(-)
the more A:(-) is stablized
the stronger the acid
Conjugate baseAcid
Molecular Structure and AcidityMolecular Structure and Acidity
pKa 38
pKa 16
pKa 51
CH3 OH3C O H
CH3 NH3C N HH H
CH3 CH3C C HH H
H H
Size of A:(-) Within a column - the larger the atom bearing the (-), the greater its stability
Molecular Structure and AcidityMolecular Structure and Acidity
CH3 O
pKa 7.0 pKa 16
+ +H3C S H H3C O HCH3 S
Resonance delocalized of charge in A-
Compare alcohol and carboxylic acid acidity
Molecular Structure and AcidityMolecular Structure and Acidity
CH3 CO
O
+ pKa = 15.9C OC
H H
HH
HH
OH
H
+
alkoxide ion
C OC
H H
HH
H OH
HH
+ pKa = 4.76OH
H
CH3 CO
OH
CH3 CO
O+ O
H
HH
resonance stabilization
curved arrows show the flow of electrons in an acid-base reaction
+ +CH3 CO
O HCH3 C
O
O
N HH
HN H
H
HH
ammoniumacetate ion
Molecular Structure and AcidityMolecular Structure and Acidity
+HSO4-C
OH3C
O
H
HORC
OH3C
OH
H
C
O+H3C
OH
H OSO3H
Molecular Structure and AcidityMolecular Structure and Acidity
molecules may have 2 or more sites that can accept a H+
e.g. carboxylic acids, esters, and amidesprotonation favored where the charge is more delocalized
which oxygen is protonated?
Molecular Structure and AcidityMolecular Structure and Acidity
resonance
octets greater contribution even with plus charge on O
C
O+ H2SO4 +HSO4
-H3C
OH
C
OH3C
OH
H
C
OH3C
O
H
HOR
C
OH3C
OH
H
C
OH3C
OH
H
C
O+ H2SO4 +HSO4
-H3C
OH
C
OH3C
OH
H
C
OH3C
O
H
HOR
C
OH3C
OH
H
C
OH3C
OH
H
Molecular Structure and AcidityMolecular Structure and Acidity
H+ on the hydroxyl
C
OH3C
O
H
H
can “write” contributing structures create & separate charge
H+ on the carbonyl
:B
C C
F
F
F
H
H
O
inductive effect, electron-withdrawing
covalent bonds transmit electronegativity (polarizing) effects push or pull shared e(-)s of adjacent atoms
Molecular Structure and AcidityMolecular Structure and Acidity
pKa: 15.9
C C
H
H
H
H
H
OH
C C
F
F
F
H
H
OH
12.4
C C
H
C
H
H
H
OH
FF
F
14.6
C C
H
C
H
H
H
OH
HC
H
F
FF
15.4
:B
C C
H
H
H
H
H
O
decreases w/ distance
inductive effect: butanoic and chlorobutanoic acids
Molecular Structure and AcidityMolecular Structure and Acidity
pKa 4.82 pKa 4.52 pKa 3.98 pKa 2.83
OH
O
OH
O
OH
O
OH
O
Cl
ClCl
Hybridization
greater the % s character with (-) the more stable the anion
Molecular Structure and AcidityMolecular Structure and Acidity
HO-H HO–
Weak Acid
alkyne
alkene
alkane
water
25
44
51
15.7
ConjugateBase pKa
H C C H H C C
HC C
H H
HC C
H H
H
HC C
H H
HH H
HC C
H HH H
Molecules as Lewis Acids
F
B
F F
H
N
H H
+
F
B
F F
H
N
H H
acid base adduct
An acid is an electron-pair acceptor.
A base is an electron-pair donor.
M2+
H2O(l)
M(H2O)42+(aq)
adduct
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