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ACID BASE CHEMISTRY
TERMS, ETC.
AMPHOTERIC:Subst. acts as either an acid or a base
Proton (Acidic p+): H+ ion; the acidic hydrogen(s) present in an acid
HNO3: one H+ H2SO4: two H+H3PO4: three H+
MONOPROTIC ACID: An acid w/ one H+
DIPROTIC ACID: An acid w/ two H+
POLYPROTIC ACID: An acid w/ 3 or more H+
HYDRONIUM ION:
H2O (l) + H+1 (aq) ---------> H3O+1 (aq)
Proton:H+; a hydrogen w/ characteristics like a proton itself -----1 p+, 0 n0, 0 e-
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Acid BASE
All acids contain H+; when in water givesolution higher [H+]
All bases contain OH-;when in water givesolution higher [OH-]
Arrhenius
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BRONSTAD – LOWRY
Acid
Any subst. thatdonates a proton; H+
BASE
Any subst. thataccepts a proton; H+
LEWIS Any subst. thataccepts an e- pair
Any subst. thatdonates an e- pair
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ACIDS BASES
•Taste sour•Turns litmus blue -- red•Lowers pH
•Feels slippery•Turns litmus red -- blue•Increases pH
The stronger the acid the better it is at donating H+
STRONG ACIDSSTRONG ACIDS
HCl ; HBr ; HI ; HNO3 ; H2SO4 ; HClO4H+
+Cl-H++I- 2H++SO4
-
2
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0 7 14
pH SCALE
STRONG ACIDIC
STRONG BASIC
MILDACIDIC
MILDBASIC
WEAK ACIDIC
WEAK BASIC
NEUTRAL ( )
Kw: constant for water, 1*10-14
ACID-BASE REACTIONS
HCl (aq) + KOH (aq) ---> KCl (aq) + HOH (l) acid base salt water
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pH -- pOH -- [H+] -- [OH-] CALCULATIONS
Formulas to Use
-w OH H K
pOH pH pK w
Constants
Kw = 1 *10 –14
pH = -log [H+]
pOH = -log [OH-]
pKw = 14
Rules for LOGSLog 1 = 0
Log 10exp = exponent
[H+] = 1*10-pH
[OH-] = 1*10-pOH
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Rules for LOGS
DIVISION
MULTILPLY84.6 Log5.8 Log 84.65.8Log
32.4 Log12.6 Log 32.412.6Log
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Calculate pH for thefollowing solutions
1) [H+] = 1 * 10-9
2) [H+] = 0.001
pH = -log (1*10-9) = -(-9) = 9
0.001 = 1*10-3
pH = -log (1*10-3) = -(-3) = 3
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3) [H+] = 3.6 * 10-2
pH = -log(3.6*10-2) = 1.44
OR-log 10-2 = 2 pH = 2 – log (3.6) = 2 – 0.56 = 1.44
Find pH & pOH
pOH pKw = pH + pOH 14 = 1.44 + pOHpOH = 14 – 1.44 = 12.56
OR
HK OH- w
2
14
10*6.310*1
= 2.78*10-13
pOH = 13 – log 2.78 = 13 – 0.44 =
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If [H+] is 6.7*10-9 mol/L, what is the pH? ACIDIC, BASIC, NEUTRAL
What is the [OH-]? What is the pOH?
pH = -log(6.7*10-9) = 9 – log 6.7 = 9 – 0.83 = 8.17 BASIC
pOH = 14 – 8.17 = 5.83
[OH-] = 1*10-5.83
Find pH Find pOH
Find [OH-]
OR
= 1.49*10-6
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CONJUGATE ACID-BASE PAIRS
Acid, loses H+, form conjugate base
Base, gains H+, forms conjugate acid
)(
-1
42(aq)3)(
-2
4)(
1
4 POH NH HPO NH aqaqaq
acid1 acid2base2 base1
CONJUGATE ACID-BASE PAIRS
(aq)3)(
1
4 NH NH
aq )(
-1
42)(
-2
4 POHHPO aqaq
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TITRATIONS
Strong Acid + Strong Base ------ Neutral
Strong Acid + Weak Base --- Acidic
Weak Acid + Strong Base --- Basic
Weak Acid + Weak Base ---- ???????
+/- ions of acid not react w/ H2O
“+” ion of strong acid reacts w/ H2O, produces H3O+
“-” ion of strong base reacts to produce OH- ions
Both +/- ions react w/ H2O
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STRENGTH
Strong Acid/Base ionize completely equilibrium lies far to the right HCl ------> H+ + Cl-
NaOH -----> Na+ + OH-
Weak Acid slightly ionize equilibrium lies far to the leftHC2H3O2 + H2O <-----> H+ + C2H3O2
-
]OH[HC
]OHC][OH[KO]H[K
O]H][OH[HC
]OHC][OH[K
232
-
2323a2eq
2232
-
2323eq
Ka: acid dissociation constantKb: base dissociation constant
IONIZATION CONSTANTS
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Ka acetic acid = 1.8*10-5
Ka nitrous acid = 4.4*10-4nitrous acid more ionized in soln
BASE
NH3 + H2O <---> NH4+ +OH-
][NH
]OH][NH[KO]H[K
O]H][[NH
]OH][NH[K
3
-
4b2eq
23
-
4eq
Kb ammonia = 1.8*10-5
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Find the Missing Part ???
CN-1
H2O
SO4-2
HC2H3O2
HC2O4-1
NH4+1
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S.A.S.A. yields weak conjugate baseW.A.W.A. yields strong conj. base
MONOPROTIC ACIDS pg. 300
Ka Acid
1.2*10-2 HSO4-
1.2*10-2 HClO2
7.2*10-4 HF
1.8*10-5 HC2H3O2
3.5*10-8 HOCl
5.6*10-10 NH4+
8.3*10-13 SO4-2
8.3*10-13 ClO2-
1.4*10-11 F-
5.56*10-10 C2H3O2-
2.9*10-7 OCl-
1.8*10-5 NH3
Kb Conj. Base
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Very Strong Very Weak
Strong
Weak
Weak
Strong
Very Weak Very Strong
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Diprotic & Triprotic Acids
H2CO3: 2 acidic protons Ka values for each H+
H CO HCO
H HCO COH2-
3
-
3
-
332Ka1 = 4.3*10-7
Ka2 = 5.6*10-11
typically weak polyprotic acid Ka1 > Ka2 > Ka3
means???? -each step of dissociation is successively weaker-loss of 2nd & 3rd proton occurs less readily
Why???? should not be surprising think in terms of charges, +/- being attracted
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S.A. : Ka 10-1 --- 10-3
W.A.: Ka 10-4 & smaller
Polyprotic acid: Ka value lowers w/ each H+ lost Loss of each additional H+ more difficult
H3PO4 + H2O <-----> H3O+ + H2PO4- Ka1
H2PO4- + H2O <-----> H3O+ + HPO4
-2 Ka2
HPO4-2 + H2O <-----> H3O+ + PO4
-3 Ka3
Ka1 > Ka2 > Ka3
10-3 10-8 10-
13
S.B.: Kb????
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Ka: acid dissociation constant
HA + H2O <-----> H3O+ + A-
HA
AOH K
-
3
a
HNO3 + H2O <-----> H3O+ + NO3-
3
-
33
aHNO
NOOH K
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BUFFER-used to control pH level of a soln.-either remove H+ or add OH- ions-usually W.A. & conj. Base
TITRATIONS.A. + W.B. -------> AcidicW.A. + S.B. -------> BasicS.A. + S.B. -------> NeutralW.A. + W.B. -----> ?? more info.
S.A. ------> weak conjugate BaseW.A. -----> strong conj. Base
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Various Ways to Describe Acid Strength
Property S.A. W.A.
Ka value Ka is large Ka is small
Position of dissociation equilibrium
Far to right Far to left
Equilibrium [H+] compared to [HA]o
[H+] [HA]o [H+]<<[HA]o
Strength of conj.base compared to H2O
A- much weaker acid than H2O
A- much stronger base than H2O
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INTERMOLECULAR FORCES
Forces that act between diff. molecules
Gases: <<< forces, act independently of each other
Liquids/Solids: >>>> Forces
KEY PTS.
Stronger the Force -------- more difficult to separate atoms/molecules
---- higher melting/boiling pts of subst.
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3 MAJOR FORCES
Dipole-DipoleDipole-Dipole London DispersionLondon Dispersion
Polar Cov. Bonds “net polarity”
Weak Force
+/- ends of molecules align together
Dipole-Dipole London Dispersion Hydrogen Bonding
All molecules; behavior due to e- movement w/i subst.
Nonpolar molecules form temporary Polarity
Weak Force; as mole.wt.
Surface Area: > S.A. ---- > Force stronger the molecule held together
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Hydrogen BondingHydrogen Bonding
Strong bond Force
H bonded to an O, N, or F of one molecule; that H will be attracted to unsharede- pair of O, N, or F of another molecule
O
H H
....O
HH
.. ..N
F....
..
..
Cl.. ....H
H F.. ....