acids & bases arrhenius theory 1. in aqueous solution 2. acid: produces h + 3. base: produces oh...
TRANSCRIPT
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ACIDS&
BASES
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Arrhenius Theory
1. in aqueous solution
2. Acid: produces H+
3. Base: produces OH-
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HA H3O+ + A-
Acid
OH2
O
HHHA + O
HHH
+
+ A-
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HCl(g) + H2O H3O+(aq) + Cl-(aq)
CH3COOH(l) + H2O = H3O+(aq) + CH3COO-(aq)
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careless, but often seen
HCl HCl H H++ + Cl+ Cl--
CHCH33COOHCOOH HH++ + CH+ CH33COOCOO--
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BaseNaOH(s) Na+(aq) + OH-(aq) OH2
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Arrhenius acid/base reaction
acid + base H2O + a salt
HA + MOH HOH + MA
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Monoprotic acid: HClHCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)
H+ + Cl- + Na+ + OH- H2O + Na+ + Cl-
H+ + OH- H2O
HCl
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Diprotic acid: H2SO4
H2SO4 (aq) + 2NaOH (aq) 2H2O(l) + Na2SO4 (aq)
H+ + OH- H2O
H2SO4
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Triprotic acid: H3PO4
Polyprotic
H3PO4(aq) + 3NaOH(aq) 3H2O(l) + Na3PO4(aq)
H3PO4 + 3 OH- 3 H2O + PO43-
H3PO4
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Bronsted-Lowry Theory1. aqueous & nonaqueous solutions
2. Acid: species donating a proton
HCl H+ + Cl-
H2SO4 H+ + HSO4-
CH3COOH H+ + CH3COO-
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Bronsted-Lowry Theory3. Base: species accepting a proton
OH- + H+ HOH
H2O + H+ H3O+
NH3 + H+ NH4+
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Conjugate acid-base pairs
acid1 + base1 acid2 + base2
conjugate pairs
HF + HOH
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Conjugate acid-base pairs
conjugate pairs
HF + HOH H3O+ + F-
acid1 + base1 acid2 + base2
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ALL Arrhenius reactions are Bronsted-Lowry
reactions
HCl + NaOH H2O + NaCl
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NOT all Bronsted reactions are Arrhenius reactions
CH3COOH + NH3 NH4+ + CH3COO-
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Amphiprotic = AmphotericCan act as either an acid or a base
HCl + HOH H3O+ + Cl-
NH3 + HOH NH4+ + OH-
NH3 + OH- NH2- + HOH
HOH + HOH H3O+ + OH-
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ACID STRENGTHRelative ability of a
compound to donate a proton
Base strength is considered a result,
not a cause
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Strong acid
100% dissociation
Weak acid
<100% dissociation
Notice this is NOT related to concentration
REVIEW
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Electronegativity is the most significant factor influencing
the strength of acids & bases
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HF > HCl > HBr > HI
as acids in non-aqueous solvents, or as pure gases
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Look at difference inelectronegativities
2.1 H - F 4.02.1 H - Cl 3.02.1 H - Br 2.82.1 H - I 2.5
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Most “ionic” is the most acidic
Nonpolar Polar Ionic
E 0 E 1.7 E 4.0
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However,as acids
in aqueous solution
HF < HCl = HBr = HI
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2.1 H - O 3.5competition!2.1 H - F 4.0
2.1 H - Cl 3.02.1 H - Br 2.82.1 H - I 2.5
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Is methane acidic as a gas or in
aqueous solution?
2.1 H - C 2.5
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The strength of oxy-acids are also
dependent on electronegativity.
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Oxy-acids and bases have the
same fundamental structure
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NaOH: Na - O - H 0.9 3.5 2.1
HClO: Cl - O - H 3.0 3.5 2.1
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In water, the more “ionic” bond
dissociates, forming the acid or base
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NaOH: Na - O - H 0.9 3.5 2.1
HClO: Cl - O - H 3.0 3.5 2.1
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Are alcohols acids or bases?
C - O - H2.5 3.5 2.1
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Acids in homologous series
are of different strength
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Acid StrengthH2SO4 > H2SO3
HNO3 > HNO2
HClO4 > HClO3 > HClO2 > HClO
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Structurally
H2SO4 = O2S(OH)2
H2SO3 = OS(OH)2
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Need to examine formal charge of
central atom.
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Acid Strength
CH3COOH> CH3CH2OH
CF3COOH > CH3COOH
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Need to examine inductive effect of neighboring
atoms.
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pH
pK
Ka , Kb , Kw
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2H2O H3O+ + OH-
KH O OH
H Oeq [ ][ ]
[ ]3
22
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Keq [H2O]2 = [H3O+ ][OH-]
Kw = [H3O+ ][OH-]
whereKw (25oC ) = 1 x 10-14
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in a neutral solution[H3O+ ] = [OH-]
1 x 10-14 = [H3O+ ]2 = [OH-]2
[H3O+ ] = [OH-] = 1 x 10-7
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pX = -log X
pK = -log K pH = -log [H3O+]pOH = -log [OH-]
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leveling effect of H2O limits [H3O+ ] & [OH-] to that
controlled by H2O
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upper limit [H3O+ ] = 1
lower limit [H3O+ ] =
1 x 10-14
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pH scale
0 7 14
acid neutral base
highest [H3O+ ] on left
lowest [H3O+ ] on right
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[H3O+ ] and [OH-]
must be considered together
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Kw = [H3O+ ][OH-]
-log Kw = -log {[H3O+ ][OH-]}
-log Kw = {-log [H3O+ ]} + {-log[OH-]}
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pKw = pH + pOH
but Kw = 1 x 10-14
14 = pH + pOH
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Relationship betweenconjugate
acids & bases
HA + H2O H3O+ + A-
A- + H2O HA + OH-
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KH O A
HA
KHA OH
A
a
b
[ ][ ][ ]
[ ][ ][ ]
3
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]A[
]OH][HA[
]HA[
]A][OH[KK 3
ba
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K KH O A
HAHA OH
Aa b
[ ][ ]
[ ][ ][ ]
[ ]3
Ka x Kb = [H3O+ ][OH-] = Kw
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Ka. Kb = [H3O+ ][OH-] = Kw
Ka. Kb = Kw
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SUMMARYpH = -log [H3O+ ]pOH = -log [OH-][H3O+ ][OH-] = 1 x 10-14
pH + pOH = 14Ka
. Kb = Kw
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Applications ofAcid-BaseConcepts
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for weak acids & bases, refer to
Appendix H for Ka & Appendix I for Kb
values in Kotz & Treichel
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1. What is the pH of a solution that is 0.025 M KOH?
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2. What is the pH of a 0.20 M acetic acid solution?
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3. 100 mL of 0.10 M CH3COOH are mixed with 20.0 mL of 0.10 M NaOH. What is the pH of the solution?
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4. Calculate the percent ionization of 0.10 M methylamine (CH3NH2).
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pH of Salts & Oxides
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What effect does the addition of a
salt to water have upon the pH of the
water?
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H2O equilibrium is the prime factor in
the behavior of solutions.
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pH of a salt solution is dependent upon the strength of the
salt as an electrolyte.
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Example 1
NaCl(s) + HOH NaOH(aq) + HCl(aq)
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Example 1
NaCl(s) + HOH NaOH (aq) + HCl(aq) strong base strong acid
Na+ + OH- + H+ + Cl- Na+ + HOH + Cl-
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thus, NaCl in water has NO effect on pH
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Example 2
NaCN(s) + HOH NaOH(aq) + HCN(aq)
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Example 2
NaCN(s) + HOH NaOH (aq) + HCN(aq) strong base weak acid
Na+ + OH- + HCN
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CN- is the anion of the weak acid HCN
CN- + HOH HCN + OH-
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NaCN(s) + HOH Na+ + OH- + HCN strong base weak acid
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thus, NaCN in water produces a/n ??
solution
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thus, NaCN in water produces a BASIC
solution
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5. What is the pH of a 0.010 M sodium cyanide solution?
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Example 3
NH4Cl(s) + HOH NH4OH (aq) + HCl(aq)
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Example 3
NH4Cl(s) + HOH NH4OH (aq) + HCl(aq) weak base strong acid
NH4OH + H+ + Cl-
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NH4+ is the cation of the
weak base NH4OH
NH4+ + HOH NH3 + H3O+
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NH4Cl(s) + HOH -> NH4OH + H+ + Cl-
weak base strong acid
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thus, NH4Cl in water produces a/n ??
solution
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thus, NH4Cl in water produces an ACID
solution
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6. What is pH of a 0.10 M ammonium chloride solution?
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Example 4
NH4CN(s) + HOH NH4OH (aq) + HCN(aq) weak base weak acid
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NH4+ is the cation of
the weak base NH4OH
NH4++ HOH NH3 + H3O+
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CN- is the anion of the weak acid HCN
CN- + HOH HCN + OH-
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thus, NH4CN in water produces a/n
?? solution
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The pH of a solution formed from the cation of a weak base and the anion
of a weak acid is dependent on the relative strength of the weak acid
and weak base.
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Ka(HCN) = 6.2 x 10-10
[Text: Table 5.1] Appendix H A-23
Kb(NH4OH) = 1.8 x 10-5
[Text: Table 5.3] Appendix I A-25
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thus, NH4CN in water produces a/n
?? solution
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thus, NH4CN in water produces a BASIC
solution, because the weak base is stronger (ionizes more) than the
weak acid
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Acidity of Oxides
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SO2 + HOH ??
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SO2 + HOH H2SO3
[O2]
H2SO4
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SO2 + HOH H2SO3
[O2]
H2SO4
Covalent oxides are acidic & are referred to as acid anhydrides
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Na2O + HOH ??
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Na2O + HOH 2NaOH(aq)
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Na2O + HOH 2NaOH(aq)
Ionic oxides are basic& are referred to as
basic anhydrides
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Lewis Acid-Base
Theory
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Acid
substance capable of accepting an e- pair
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Lewis acidmust have an empty
valence level orbital
i.e. H+ has an empty 1s orbital which can accept an e- pair
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Thus, H+ is an acid under all three theories
Arrhenius
Bronsted-Lowry
Lewis
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Lewis Acid-Base TheoryAcid: substance capable
of accepting an e- pair
Base
substance capable of donating an e- pair
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Examples of Lewis bases
OH- , NH3 , F-
all have unbonded pairs of e- available for
donation
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Elements of Group 13 (3A) form compounds
that make excellent Lewis acids
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another “typical”Lewis acid-base
reaction:
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Reaction of a Lewis Acid and Lewis Base
New bond formed using electron pair from the Lewis base.
Coordinate covalent bond
Notice geometry change on reaction.
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Formation of hydronium ion is also an excellent example.
Lewis Acids & Bases
•Electron pair of the new O-H bond originates on the Lewis base.
HH
H
BASE
••••••
O—HO—H
H+
ACID
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Lewis Acid/Base Reaction
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H3BO3 + H2O H2BO3- + H3O+
?
NO!
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H3BO3 + 2H2O B(OH)4- + H3O+
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is Al(OH)3 an
acid or base?
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Amphoterism of Al(OH)3
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This explains AMPHOTERIC nature of some metal hydroxides.
Al(OH)3(s) + 3 H+ Al3+ + 3 H2O
Here Al(OH)3 is a Brønsted base.
Al(OH)3(s) + OH- Al(OH)4-
Here Al(OH)3 is a Lewis acid.
Al3+ O—H-••••
••Al3+ O—H-
••••
••
Lewis Acids & Bases
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Transition metal ions also very good
Lewis Acids
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Other good examples involve metal ions.
Lewis Acids & Bases
HH
••
BASE
••••••
Co2+
ACID
O—HO—H
Co2+
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Zn2+ + HOH ?..
Zn2+ => [Ar] 4s0 3d10 4p0
Zn(H2O)42+
..
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Reaction of NH3 with Cu2+
(aq)
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Formation of complexions is a Lewis
acid-base reaction
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Lewis Acid-Base Interactions in Biology
The heme group in hemoglobin can interact with O2 and CO.
The Fe ion in hemoglobin is a Lewis acid
O2 and CO can act as Lewis bases
Heme group
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LewisBronsteadArrhenius
Inclusiveness of the Acid/Base Definitions