Acids & Bases
Water and acid combine in
an exothermic reaction releasing large amounts
of heat.
Water and acid combine in
an exothermic reaction releasing large amounts
of heat.
Acid - Base Theories
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Lavoisier
Arrhenius
Bronsted-Lowry
Lewis
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Antoine
Lavoisier
Lavoisier - 1777
Acidity is caused by
the presence of
oxygen in the
compound.
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Lavoisier - 1777
He even created the word
oxygen - from the
Greek oxys, "sour"
and genes, "born"
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Lavoisier - 1777
Oxygen means
"acid maker".
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Lavoisier - 1777
Lavoisier's idea about
acids turned out
to be wrong...
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Lavoisier - 1777
but it is historically important
since it is the first scientific
attempt to chemically
characterize acids
and bases.
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Arrhenius
Bronsted-Lowry
Lewis
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Svante
August
Arrhenius
Arrhenius Acid
Any substance
that produces
hydrogen ions,
+
H , in water
solution.
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Arrhenius Base
Any substance
that produces
hydroxide ions,
OH , in water
solution.
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In a formula, such as HCl,
the positive part of a
Arrhenius acid
will ALWAYS
be hydrogen.
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In a formula, such as
NaOH, the negative part
of a Arrhenius
base will
ALWAYS
be hydroxide.
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Arrhenius acids and
bases, and soluble salts,
are called electrolytes.
When each dissolves,
ions are released that
conduct electricity.
If a solution has
NO ions, it cannot
conduct electricity.
Bronsted-Lowry Theory
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Johannes
Nicolaus
Bronsted
Bronsted-Lowry Theory
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Thomas
Martin
Lowry
Bronsted-Lowry Acid
Any substance that
acts as a proton donor.
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Bronsted-Lowry Acid
A B-L acid MUST have
hydrogen somewhere
in its
formula.
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Bronsted-Lowry Acid
When an electron is
removed from a
hydrogen atom...
+
-
Bronsted-Lowry Acid
a hydrogen ion is
produced - a proton.
+
Bronsted-Lowry Base
Any substance that
acts as a proton
acceptor.
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Bronsted-Lowry Base
Most negative ions can
acts as B-L bases.
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Bronsted-Lowry Theory
The acid/base definitions
are broadened because no
specific ion must be formed,
although hydrogen is the
only source of protons.
What is the
formula for the
hydronium ion?
+
H3O
Bronsted-Lowry Theory
The hydronium ion is formed
by combining a hydrogen
ion and a water molecule.
H2O + H
+
H3O
+
Bronsted-Lowry Theory
conjugate base
Bronsted-Lowry Theory
A conjugate base is the
particle that remains
AFTER an acid gives
up a proton.
Bronsted-Lowry Theory
conjugate acid
Bronsted-Lowry Theory
A conjugate acid is the
particle formed when a
base accepts a proton.
HCl + H2O
-
+
Cl + H3O
Identify the B-L acid
in this equation.
What gives up a proton from
the left side to the right?
HCl + H2O
-
+
Cl + H3O
HCl donates a proton,
it is the B-L acid.
HCl + H2O
-
+
Cl + H3O
Identify the B-L base
in this equation.
What gains a proton from
the left side to the right?
HCl + H2O
-
+
Cl + H3O
H2O accepts a proton,
it is the B-L base.
HCl + H2O
-
+
Cl + H3O
Identify the conjugate
base in this equation.
What is left when the
acid gives up a proton?
HCl + H2O
Cl
-
+
Cl + H3O
is left when HCl
gives up a proton, it
is the conjugate base.
HCl + H2O
-
+
Cl + H3O
Identify the conjugate
acid in this equation.
What is formed when the
base accepts a proton?
HCl + H2O
+
O
-
+
Cl + H3O
H3 is formed when
water accepts a proton,
it is the conjugate acid.
HCl + H2O
-
+
Cl + H3O
acids have
conjugate bases
HCl + H2O
-
+
Cl + H3O
bases have
conjugate acids
Remove a proton from an
acid to get its conjugate
base.
H2SO4
HI
H2 O
Remove a proton from an
acid to get its conjugate
base.
H2SO4
HI
H2 O
HSO4
-
Remove a proton from an
acid to get its conjugate
base.
H2SO4
HSO4
HI
I
H2 O
-
Remove a proton from an
acid to get its conjugate
base.
H2SO4
HSO4
HI
I
H2 O
OH
-
Add a proton to a base to
get its conjugate acid.
Cl
H2 O
NO3
-
Add a proton to a base to
get its conjugate acid.
Cl
HCl
H2 O
NO3
-
Add a proton to a base to
get its conjugate acid.
Cl
HCl
H2 O
NO3
-
H3
+
O
Add a proton to a base to
get its conjugate acid.
Cl
HCl
H2 O
NO3
-
H3
+
O
HNO3
The Lewis Theory
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Gilbert
Newton
Lewis
Lewis Acid
Any substance that
acts as an
electron-pair
acceptor.
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Lewis Base
Any substance that
acts as an
electron-pair
donor.
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The Lewis Theory
This theory is the
broadest of all.
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The Lewis Theory
Any reaction that
involves the exchange
of electrons WILL
have a Lewis acid
and Lewis base.
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The Lewis Theory
In an equation, the Lewis
acid gets
MORE NEGATIVE
from the left side to the
right side - it gains e .
The Lewis Theory
In an equation, the Lewis
base gets
MORE POSITIVE
from the left side to the
right side - it loses e .
Cl2 + I-
Cl- + I2
Identify the Lewis acid
in this equation.
What gets more negative?
Cl2 + I-
Cl- + I2
Cl2 gets more negative
from the left side to the
right, it is the Lewis acid.
Cl2 + I-
Cl- + I2
Identify the Lewis base
in this equation.
What gets more positive?
Cl2 + II
Cl- + I2
gets more positive
from the left side to the
right, it is the Lewis base.
End
Acid - Base
Theories
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Binary Acids
Acids composed of
two elements:
hydrogen and a halogen
Naming Binary Acids
First:
Determine the stem word.
The stem word comes from
the negative element.
Naming Binary Acids
First:
Determine the stem word.
Example - HCl
chlorine is the negative
element - CHLOR is the stem.
Naming Binary Acids
Second:
Add the prefix hydro
to the stem.
Naming Binary Acids
Second:
Add the prefix hydro
to the stem.
Example - hydro + chlor
Naming Binary Acids
Third:
Change the ending
of the stem to ic.
Naming Binary Acids
Third:
Change the ending
of the stem to ic.
Example - hydro + chlor + ic
Naming Binary Acids
Final name:
hydrochloric acid
Naming Binary Acids
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HCl
HF
HBr
HI
Naming Binary Acids
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HCl
HF
HBr
HI
hydro chlor ic acid
Naming Binary Acids
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HCl
HF
HBr
HI
hydro chlor ic acid
hydro fluor ic acid
Naming Binary Acids
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HCl
HF
HBr
HI
hydro chlor ic acid
hydro fluor ic acid
hydro brom ic acid
Naming Binary Acids
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HCl
HF
HBr
HI
hydro chlor ic acid
hydro fluor ic acid
hydro brom ic acid
hydro iod ic acid
Naming Ternary Acids
Ternary acids composed of
three elements:
hydrogen, oxygen,
and a nonmetal
Naming Ternary Acids
First:
Determine the stem
part of the name of
the third element
Naming Ternary Acids
First:
Determine the stem
Example - H2SO4
sulfur is the third element,
SULFUR is the stem.
Naming Ternary Acids
Second:
The most common form of the
acid is given the suffix ic.
Naming Ternary Acids
Second:
The most common form of the
acid is given the suffix ic.
Example - sulfur + ic acid
Naming Ternary Acids
Third:
If the acid is NOT in its
most common form,
do the following:
Naming Ternary Acids
Add the prefix per if the acid
has one more oxygen than
the most common form.
Naming Ternary Acids
Add the prefix per if the acid
has one more oxygen than
the most common form.
Example - H2SO5
per + sulfuric acid
Naming Ternary Acids
Add the suffix ous if the acid
has one less oxygen than
the most common form.
Naming Ternary Acids
Add the suffix ous if the acid
has one less oxygen than
the most common form.
Example - H2SO3
sulfur + ous acid
Naming Ternary Acids
Add the prefix hypo if the acid
has two less oxygen atoms
than the most common form.
Naming Ternary Acids
Add the prefix hypo if the acid
has two less oxygen atoms
than the most common form.
Example - H2SO2
hypo + sulfur + ous acid
Naming Ternary Acids
HClO3
Chloric Acid
Naming Ternary Acids
HClO4
HClO3
Chloric Acid
Naming Ternary Acids
HClO4
HClO3
Perchloric Acid
Chloric Acid
Naming Ternary Acids
HClO4
HClO3
HClO2
Perchloric Acid
Chloric Acid
Naming Ternary Acids
HClO4
HClO3
HClO2
Perchloric Acid
Chloric Acid
Chlorous Acid
Naming Ternary Acids
HClO4
HClO3
HClO2
HClO
Perchloric Acid
Chloric Acid
Chlorous Acid
Naming Ternary Acids
HClO4
HClO3
HClO2
HClO
Perchloric Acid
Chloric Acid
Chlorous Acid
Hypochlorous Acid
Strong
or
Weak
Strong or Weak
Strong acids and bases
ionize completely in
water solution.
Strong or Weak
HCl, HBr, and HI are the
only Strong binary acids.
Strong or Weak
In Strong ternary acids,
the number of oxygen
atoms exceeds the
number of...
Strong or Weak
hydrogen atoms by
two or more.
H2SO4 and HNO3 are strong.
H3PO4 is weak.
Strong or Weak
Hydroxides of
groups 1 and 2,
except Be, are
Strong bases.
Amphoteric
A substance that acts
as either an acid or
base, depending on
what it reacts with.
HOH
Water is the most
common amphoteric
substance.
Anhydrous Without H2O
Acid Anhydride an oxide that produces
an acid in water.
Acid Anhydride oxides of nonmetals
SO2 + H2O
H2SO3
Basic Anhydride an oxide that produces
a base in water.
Basic Anhydride oxides of metals
Na2O + H2O
2NaOH
Anhydrous - Without H2O
Write the anhydrous form of:
1.
2.
3.
4.
H2SO3
H 2 C 2 O4
H3PO4
H 4 C 2 O2
Anhydrous - Without H2O
Write the anhydrous form of:
1.
2.
3.
4.
H2SO3
H 2 C 2 O4
H3PO4
H 4 C 2 O2
SO2
Anhydrous - Without H2O
Write the anhydrous form of:
1.
2.
3.
4.
H2SO3
H 2 C 2 O4
H3PO4
H 4 C 2 O2
SO2
C2O3
Anhydrous - Without H2O
Write the anhydrous form of:
1.
2.
3.
4.
H2SO3
H 2 C 2 O4
H3PO4
H 4 C 2 O2
SO2
C2O3
HPO3
Anhydrous - Without H2O
Write the anhydrous form of:
1.
2.
3.
4.
H2SO3
H 2 C 2 O4
H3PO4
H 4 C 2 O2
SO2
C2O3
HPO3
C2