Acids

1
Acids Bases
I. Properties of Acids Bases
-_____ taste ____ and produce a _______
sensation to the touch
acids
sour
burning
-______ acid and ________ acid, (also known as
_______ __), are _____ _____ responsible for the
_______ of ______ and other ______, while
______ ____ makes _______ taste ____, and in
our body, the unpleasant ________ and _______
_________ produced by our _____ is due to
___________ ____ in our ________
citric
ascorbic
Vitamin
C
weak
acids
tartness
citrus
fruits
acetic
acid
vinegar
sour
sourness
Hydrangea the color varies depending on the
relative acidity or basicity of the soil
burning
sensation
vomit
hydrochloric
acid
stomach
2
Acids Bases
I. Properties of Acids Bases
-because _____ ____ and _______ ________, (and
all ______ ______ are made of _______), in
______, they are often used as a _______
acids
burn
denature
proteins
living
things
proteins
nature
defense
-____, ____, ______, and ______ all use ______
____ to ______ themselves, while the human
_______ is guarded against _______ by
___________ ____, the human ______ is guarded
against _______ by ______ ____ (produced by
_____- _________ _______ of the genus
___________), and even human ____ is guarded by
____ ____ in our _____
bees
ants
nettles
onions
formic
acid
defend
stomach
bacteria
hydrochloric
acid
vagina
bacteria
lactic
acid
sugar
fermenting
bacteria
Lactobacillus
skin
uric
acid
sweat
Stinging Nettle
3
Acids Bases
I. Properties of Acids Bases
-_____ react with ______, especially the more
______ ______, to produce ________ ___
acids
metals
active
metals
hydrogen
gas
2HCl (aq)
1ZnCl2 (aq)
1Zn (s)

1H2 (g)

6HNO3 (aq)
2Al(NO3)3 (aq)
2Al (s)

3H2 (g)

acids
carbonates
-_____ react with _________ and ________
_________ to produce ______ _______
hydrogen
carbonates
carbon
dioxide
They dont just taste chalky, they are chalk!
2HCl (aq)
1CaCl2 (aq)
1CaCO3 (s)

1H2O (l)

1CO2 (g)

HC2H3O2 (aq)
1NaC2H3O2 (aq)
1NaHCO3 (s)

1H2O (l)

1CO2 (g)

4
Acids Bases
I. Properties of Acids Bases
Write the balanced thermochemical equation for
the reaction that occurs between
1. Magnesium and Nitric acid
2HNO3 (aq)
1Mg(NO3)2 (aq)
1Mg (s)

1H2 (g)

2. Aluminum and Sulfuric acid
3H2SO4 (aq)
1Al2(SO4)3 (aq)
2Al (s)

3H2 (g)

3. Calcium carbonate and Hydrobromic acid
2HBr (aq)
1CaBr2 (aq)
1CaCO3 (s)

1H2O (l)

1CO2 (g)

4. Potassium Hydrogen carbonate and Hydrochloric
acid
1HCl (aq)
1KCl (aq)
1KHCO3 (s)

1H2O (l)

1CO2 (g)

5
Acids Bases
I. Properties of Acids Bases
1. Hypothesis
Which common household materials are acids or
bases?
2. Prediction
3. Gather Data
A. Safety
The acids and bases used in this lab are mildly
corrosive and cause irritation of the skin, eyes,
and mucous membranes. Avoid contact. Use
caution. Goggles mandatory.
B. Procedure
1. Using a pipette, place 3 or 4 drops of each
solution in a separate test well of a
microplate.
6
Acids Bases
I. Properties of Acids Bases
3. Gather Data
B. Procedure
2. Test each liquid with litmus paper. Record
results.
3. Test each liquid with 2 drops of
phenolphthalein. Record results.
7
Acids Bases
II. Ions in Solutions of Acids Bases
-the relative amounts of ____ and ____ ions in
________ _______ determine the _______ ______,
_______, or ________ of the ________
H
OH-
aqueous
solution
relative
acidity
basicity
neutrality
solution
-an _______ _______ that contains more ___ than
____ is an ______ _______
aqueous
solution
H
OH-
acidic
solution
Red tulip changes color in varying pH
aqueous
solution
-an _______ _______ that contains more ____ than
___ is an _____ _______
OH-
H
basic
solution
-an _______ _______ that contains _____ amounts
of ___ and ____ is _______
aqueous
solution
equal
Purple iris changes color in varying pH
H
OH-
neutral
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8
Acids Bases
II. Ions in Solutions of Acids Bases
-_______ ________ that are neither ______ or
_____ are _______, but _____ is _______ because
it is ____ an ____ and a ____ at the same time,
containing _____ amounts of ___ and ____
aqueous
solutions
acids
bases
neutral
water
neutral
both
acid
base
equal
H
OH-
polarity
-because of its _______, _____ ___________
Purple carnation changes color in varying pH
water
self-ionizes
1H2O(l)
1H (aq)

1OH-(aq)
H
covalent
-but the ___ forms a _______ _____ with a ______
_____ ________, producing the __________ ____
bond
another
water
molecule
hydronium
ion
Peony changes color in varying pH
2H2O(l)
1H3O(aq)

1OH-(aq)
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9
Acids Bases
III. The Arrhenius Model of Acids and
Bases
-according to ______ _________, an ____ is a
________ that contains ________ and _______ to
produce ________ ____ in _______ _______
Svante
Arrhenius
acid
substance
hydrogen
ionizes
hydrogen
ions
aqueous
solution
-according to _________, ________ ________ is an
_____
Hydrogen
Arrhenius
chloride
acid
1HCl (g)
1H (aq)
1Cl- (aq)

-according to _________, a _____ is a ________
that contains a _________ _____ and _________ to
produce _________ _____ in _______ ________
Arrhenius
base
substance
hydroxide
group
dissociates
hydroxide
ions
aqueous
solution
-according to _________, ________ _________ is a
_____
Arrhenius
Sodium
hydroxide
base
1NaOH (s)
1Na (aq)
1OH- (aq)

Svante August Arrhenius 1859 - 1927
10
Acids Bases
IV. The Brønsted Lowry Model of Acids
and Bases
-according to ________-______, an _____ is a
_________-____ ______ and a _____ is a
________- ____ ________
Brønsted
Lowry
acid
hydrogen
ion
donor
base
hydrogen
ion
acceptor
1H2O (l)
1H3O(aq)
1HX (aq)

1X- (aq)

Base
Acid
Conjugate Acid
Conjugate Base
-the _____, ______, _________ in _____ and
_______ a ________ ____ to a ______ ________,
which acts as a _____ by ________ the ________
____
acid
HX (aq)
dissolves
water
donates
hydrogen
ion
water
molecule
base
accepting
hydrogen
ion
base
accepted
H
-a ____ that has ________ a ___ now has the
ability to ______ a ___, and so becomes an
_____ the _________ _____
donate
H
acid
Johannes Nicolaus Brønsted 1879 - 1947
Thomas Martin Lowry 1874 - 1936
conjugate
acid
11
Acids Bases
IV. The Brønsted Lowry Model of Acids
and Bases
-according to ________-______, a _________ ____
is the ______ produced when a ____ accepts a
________ ___ from an ____
Brønsted
Lowry
conjugate
acid
species
base
hydrogen
ion
acid
1H2O (l)
1H3O(aq)
1HF (aq)

1F- (aq)

Base
Acid
Conjugate Acid
Conjugate Base
-a _________ ____ is the ______ that is left
over from the ____ after it donates a ________
____
conjugate
base
species
acid
hydrogen
ion
How is playing Hacky Sack Like Conjugate Acid-Base
Pairs?
Conjugate acid
Player who passed Footbag
Player passing Footbag
Acid
Footbag
Hydrogen ion
Player receiving Footbag
Base
Playing Hacky Sack in Zurich, Switzerland
Conjugate base
Player who received Footbag
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-sack.html
12
Acids Bases
IV. The Brønsted Lowry Model of Acids
and Bases
Label the acid, base, conjugate acid, and
conjugate base in the following
1H2O (l)
1NH4(aq)
1NH3 (aq)

1OH- (aq)

Substances that can act as both an acid and a
base are called amphoteric, as water is in these
examples.
Base
Acid
Conjugate Acid
Conjugate Base
1H2O (l)
1H3O(aq)
1HBr (aq)

1Br- (aq)

Acid
Base
Conjugate Acid
Conjugate Base
1H2O (l)
1HCO3-(aq)
1CO32- (aq)

1OH- (aq)

Conjugate Acid
Conjugate Base
Acid
Base
1H2O (l)
1H3O(aq)
1HSO4- (aq)

1SO42- (aq)

Acid
Base
Conjugate Acid
Conjugate Base
13
Acids Bases
V. Monoprotic Polyprotic Acids
-____ and ___ are _____ according to the
_________ _____ because they both contain
_________ and they both donate a ________ ___ to
an _______ ________
HCl
HF
acids
Arrhenius
model
hydrogen
hydrogen
ion
aqueous
solution
-both ____ and ___ are also __________ _____
because each donates only ____ _________ ___
per ________
HCl
HF
monoprotic
acids
Chemical burns caused by Hydrofluoric acid
one
http//www.emedicine.com/emerg/topic804.htm
hydrogen
ion
molecule
-_____ (______ _____), ______ (_________ _____),
____ (____________ _____), and _________
(______ or ________ _____) are other
__________ ______
HNO3
Nitric
acid
HClO4
Perchloric
acid
HBr
Hydrobromic
acid
CH3COOH
acetic
Even though acetic acid has 4 hydrogen atoms,
only 1 of the 4 has a polar enough bond to be
ionizable. The other 3 are practically nonpolar
bonds.
ethanoic
acid
monoprotic
acids
14
Acids Bases
V. Monoprotic Polyprotic Acids
-_____ that donate _____ than ____ _________ ___
are called _________
acids
more
one
hydrogen
ion
polyprotic
-______(_______ _____) and ______(________
_____) are both _______ _____, while ______
(__________ ____) and ______ (______ _____) are
both _________ ______
H2SO4
Sulfuric
acid
H2CO3
Carbonic
acid
diprotic
acids
H3PO4
Phosphoric
acid
H3BO3
Boric
acid
triprotic
acids
Benzene has 6 hydrogen atoms, but none of the
covalent bonds are polar enough to be
ionizable, so benzene is not an acid at all.
Sulfuric acid contains 2 highly polar
ionizable covalent bonds
Phosphoric acid contains 3 highly polar
ionizable covalent bonds
15
Acids Bases
V. Monoprotic Polyprotic Acids
-__________ _____ donate more than ____ ________
____ to _______ _______ in more than ___ step
polyprotic
acids
one
hydrogen
ion
aqueous
solution
one
-the ________ ____ __________ ____ donates __
________ ____ in __ steps
triprotic
acid
Phosphoric
3
hydrogen
ions
acid
3
1H2O (l)
1H3O(aq)
1H3PO4 (aq)

1H2PO4- (aq)

1H2O (l)
1H3O(aq)
1H2PO4- (aq)

1HPO42- (aq)

1H2O (l)
1H3O(aq)
1HPO42- (aq)

1PO43- (aq)

16
Acids Bases
V. Monoprotic Polyprotic Acids
Write the steps for complete ionization of the
following polyprotic acids
H2Se (aq)
H2O (l)
H3O(aq)

1HSe- (aq)

H2O (l)
H3O(aq)
HSe- (aq)

Se2- (aq)

H3AsO4 (aq)
H2O (l)
H3O(aq)

H2AsO4- (aq)

H2O (l)
H3O(aq)
H2AsO4- (aq)

HAsO42- (aq)

H2O (l)
H3O(aq)
HAsO42- (aq)

AsO43- (aq)

H2SO3 (aq)
H2O (l)
H3O(aq)

HSO31- (aq)

H2O (l)
H3O(aq)
HSO31- (aq)

SO32- (aq)

17
Acids Bases
VI. Acid Base Anhydrides
-__________ are _______ that form _____ and
_____ when added to ______
anhydrides
oxides
acids
bases
water
1H2O (l)
1H2CO3 (aq)
1CO2 (g)

1H2O (l)
1HNO3 (aq)
2NO2 (g)


1HNO2 (aq)
1H2O (l)
1H2SO3 (aq)
1SO2 (g)

1H2O (l)
1H2SO4 (aq)
1SO3 (g)

oxides
nonmetallic
-______ of ___________ elements produce _____ in
_______ _______, while ______ of ________
elements produce _____ in _______ ________
acids
aqueous
solution
oxides
metallic
bases
aqueous
solution
1H2O (l)
1Ca2 (aq)
1CaO (s)


2OH- (aq)
1H2O (l)
1Mg2 (aq)
1MgO (s)


2OH- (aq)
18
Acids Bases
VII. Strength of Acids
-______ _____ are _____ that ______ _________
strong
acids
acids
ionize
completely
1H2O (l)
1H3O (aq)
1HCl (aq)


1Cl- (aq)
-____ (___________ _____), ______ (__________
_____), _____ (______ ____), ____ (____________
_____), ______ (________ _____), and ___
(___________ _____) are all ______ _____
HCl
Hydrochloric
acid
HClO4
Hydrofluoric acid is considered a weak acid
because it doesnt ionize completely it is
expected to be a strong acid, because it is so
corrosive, but its corrosiveness is due to the
chemical reactivity of its anion, the fluoride
ion. The strongest acids, the carborane
superacids, are a million times stronger than
concentrated sulfuric acid, but not at all
corrosive because the anion to the acid is so
unreactive.
Perchloric
acid
HNO3
Nitric
acid
HBr
Hydrobromic
acid
H2SO4
Sulfuric
acid
HI
Hydroiodic
acid
strong
acids
-______ _____ are _____ that ______ only ________
weak
acids
acids
ionize
partially
HC2H3O2 (aq)
H2O (l)
H3O(aq)

C2H3O2- (aq)

-________ (______ _____), ______ (________
_____), ___ (___________ ____), ______ (_____
_____), and _____ (___________ ____) are _____
_____
HC2H3O2
Acetic
acid
H2CO3
Carbonic
acid
HF
Hydrofluoric
acid
H3BO3
Boric
acid
HCN
Hydrocyanic
acid
weak
acids
19
Acids Bases
VII. Strength of Acids
-according to ______________, the ____ on the
_______ side of the ________ _______ produces a
________ ____ on the ________ side of the
_______ _______ by _______ a ________ ___
Brønsted-Lowry
acid
reactant
forward
reaction
conjugate
base
product
forward
reaction
donating
hydrogen
ion
1H2O (l)
1H3O(aq)
1HX (aq)

1X- (aq)

Acid
Conjugate Base
-if the ____ is a ______ ____, then its
_________ ____ is _____, that is, if the ____
readily _______ a ________ ___, then its
________ ____ is not very good at ________a
________ ___, or holding on to one, while a
____ ____, which is not very good at _______ a
________ ___ has a ______ ________ ____
acid
strong
acid
conjugate
base
weak
acid
donates
hydrogen
ion
conjugate
base
accepting
hydrogen
ion
weak
acid
donating
hydrogen
ion
strong
conjugate
base
20
Acids Bases
VII. Strength of Acids
-the _________ ________ for ___________ _____ is
ionization
equation
Hydrocyanic
acid
1HCN (aq)
1H2O (l)
1H3O(aq)

1CN- (aq)

equilibrium
constant
expression
-the __________ ________ __________ for the
_________ of ____________ _____ is
ionization
Hydrocyanic
acid
H3O1
CN-1
Keq

HCN1
H2O1
concentration
liquid
water
-the ___________ of ______ _____ is considered
to be _______, and so can be _________ with ___
to give the _____ _________ _______, or ___
constant
combined
Keq
acid
ionization
constant
Ka
H3O1
CN-1
Ka

HCN1
21
Acids Bases
VII. Strength of Acids
Write ionization equations and acid ionization
constant expressions for the following acids
H2O (l)
H3O(aq)
HClO2 (aq)

ClO2- (aq)

H3O1
ClO2-1
Ka

HClO21
HNO2 (aq)
H2O (l)
H3O(aq)

NO2- (aq)

H3O1
NO2-1
Ka

HNO21
HIO (aq)
H2O (l)
H3O(aq)

IO- (aq)

H3O1
IO-1
Ka

HIO1
22
Acids Bases
VIII. Strength of Bases
-______ _____ are _____ that _________ _________
strong
bases
bases
dissociate
completely
1Na (aq)
1NaOH (s)

1OH- (aq)
-______ (_______________), _____
(_________________), ______ (_________
_________), _____ (_______________), _______
(________________), and ______ (_______________)
are all ______ _____
NaOH
Sodium hydroxide
KOH
Potassium hydroxide
RbOH
Rubidium
hydroxide
CsOH
Cesium hydroxide
Ca(OH)2
Calcium hydroxide
Ba(OH)2
Barium hydroxide
strong
bases
-______ _____ are _____ that ________ only
________
weak
bases
bases
dissociate
partially
CH3NH2 (aq)
H2O (l)
CH3NH3(aq)

OH- (aq)

-________ (___________), ________ (__________),
____ (________), and ________ (______) are all
_____ ______
CH3NH2
methylamine
C2H5NH2
ethylamine
NH3
ammonia
C6H5NH2
aniline
weak
bases
23
Acids Bases
VIII. Strength of Bases
-the ________ ________ for __________ is
ionization
equation
hexylamine
1C6H13NH2 (aq)
1H2O (l)
1OH-(aq)

1C6H13NH3 (aq)

Conjugate Acid
Conjugate Base
Base
Acid
acid
ionization
constant
-the ____ __________ ________ __________ for
the _________ of ___________ is
expression
ionization
hexylamine
OH-1
C6H13NH31
Kb

C6H13NH21
Hexylamine
24
Acids Bases
VIII. Strength of Bases
Write ionization equations and base ionization
constant expressions for the following bases
H2O (l)
OH-(aq)
C3H7NH2 (aq)

C3H7NH3 (aq)

OH-1
C3H7NH31
Kb

C3H7NH21
CO32-(aq)
H2O (l)
OH-(aq)

HCO3- (aq)

OH-1
HCO3-1
Kb

CO32-1
HSO3- (aq)
H2O (l)
OH-(aq)

H2SO3 (aq)

OH-1
H2SO31
Kb

HSO3-1
25
Acids Bases
IX. Ion Product Constant for Water
-the ________ ________ for ______ is
ionization
equation
water
H2O (l)
OH-(aq)
H2O (l)

H3O (aq)

Conjugate Acid
Conjugate Base
Base
Acid
ionization
equation
-the ________ ________ can be simplified to
H2O (l)
OH-(aq)
H (aq)

equilibrium
constant
-the __________ _______ __________ is
expression
OH-1
H1
Keq

H2O1
26
Acids Bases
IX. Ion Product Constant for Water
-since _____ is a ______, its _____________ is
equal to its _______, which is _______ at a
_______ ___________ and ________, so the
__________ _______ _________ can be simplified
by __________ both sides by ______, creating
the ___ _______ _______ ___ _____, ___
water
liquid
concentration
density
constant
Kw

OH-1
H1
constant
temperature
pressure
equilibrium
Kw

(1 x 10-7)1
(1 x 10-7)1
constant
expression
Kw

1 x 10-14
multiplying
H2O
ion
product
constant
for
water
Kw
298 K
self
ionization
-at _____, the ____- _________ of _____ produces
____ _________ and a ______ _________, so
___ _______
H
water
OH-
1 x 10-7 M
Kw
1 x 10-7 M
1 x 10-14
27
Acids Bases
IX. Ion Product Constant for Water
What is the concentration of the hydroxide ion in
an aqueous solution with a hydrogen ion
concentration of 1 x 10-5 M? Is the solution
acidic, basic, or neutral?
Kw

H
OH-
1 x 10-14

OH-
(1 x 10-5)
OH-

1 x 10-9 M
The solution is acidic, because the H is
greater (104) than the OH-
What is the concentration of the hydrogen ion in
an aqueous solution with a hydroxide ion
concentration of 1 x 10-3 M? Is the solution
acidic, basic, or neutral?
Kw

H
OH-
1 x 10-14

H
(1 x 10-3)
H

1 x 10-11 M
The solution is basic, because the OH- is
greater (108) than the H
28
Acids Bases
X. pH (pondus hydrogenii)
-in 1909, _____ ________ developed the ___
(________ _________) _____ as a way of
conveniently expressing the ___________ of _____
and _____
Søren
Sørensen
pH
potential
hydrogen
scale
concentration
acids
bases
pH

-log H
What is the pH of water?
pH

-log H
The number of decimal places in the pH is equal
to the number of significant digits in the H
pH

-log (1 x 10-7)
pH

7.0
1 sig. fig. in H, 1 decimal place in pH
What is the pH of an aqueous solution in which
the H 1.0 x 10-2 M?
pH

-log H
pH

-log (1.0 x 10-2)
pH

2.00
2 sig. figs. in H, 2 decimal place in pH
Søren Sørensen 1868 - 1939
29
Acids Bases
X. pH (pondus hydrogenii)
1. Hypothesis
What is the relationship between the
concentration of an acid and its pH?
2. Prediction
3. Gather Data
A. Safety
The acids used in this lab are corrosive and
cause irritation and damage to the skin, eyes,
and mucous membranes. Avoid contact. Use
caution. Goggles mandatory.
B. Procedure Serial Dilution
1. Using a pipette, place 10 drops of 1.0 M HCl
in test well 1A of a microplate.
30
Acids Bases
X. pH (pondus hydrogenii)
3. Gather Data
B. Procedure
2. Rinse the pipette, and transfer 1 drop of
acid solution from test well 1A to test well
2A, and add 9 drops of distilled water.
3. Repeat Step 2, transferring 1 drop of acid
solution from test well 2A to test well 3A
and adding 9 drops of distilled water .
4. Repeat Step 2 six more times, each time
transferring 1 drop of acid solution from
the previous test well and adding 9 drops of
distilled water.
31
Acids Bases
X. pH (pondus hydrogenii)
3. Gather Data
B. Procedure
5. Test the pH in each well with pH indicator
paper. Record.
6. Test the pH in each well with 1 drop of
universal indicator solution. Record.
32
Acids Bases
X. pH (pondus hydrogenii)
4. Analyze Data
A. What is H in test well A4?
________________.
B. What is H in test well A6?
________________.
C. What is the theoretical pH in test well A2?
_______________.
D. What is the theoretical pH in test well B2?
_______________.
E. The color of pH paper in test well A1 was
_______, indicating an approximate pH of
_______.
F. In test well A2 universal indicator was
________ in color.
5. Draw Conclusions
A. Each step in the serial dilution ____________
the concentration of the hydrogen ion by a
factor of _______ and __________ the pH
by a factor of _______
33
Acids Bases
XI. pOH (potential Hydroxide)
-the _______, or ________, of a _______ can be
expressed by the ____, or ________ _________
basicity
alkalinity
solution
pOH
potential
Hydroxide
pOH

-log OH-
What is the pOH of water?
What is the pH of an aqueous solution in which
the OH- 1.0 x 10-3 M?
pOH

-log OH-
pOH

-log OH-
pOH

-log (1 x 10-7)
pOH

-log (1.0 x 10-3)
pOH

7.0
pOH

3.00
What is the pOH of an aqueous solution in which
the OH- 1.00 x 10-6 M?
Kw

OH-
H
pOH

-log OH-

(1 x 10-7)
(1 x 10-7)
1 x 10-14
pOH

-log (1.00 x 10-6)

14
pH

pOH
pOH

6.000
pH

11.00
34
Acids Bases
XI. pOH (potential Hydroxide)
What is the pH and the pOH of an aqueous solution
with a hydroxide ion concentration of 1.0 x 10-6
M? Is the solution acidic, basic, or neutral?
pOH

-log OH-
pOH

6.00
pH

8.00
pOH

-log (1.0 x 10-6)

14
pH

pOH
basic
What is the pH and the pOH of an aqueous solution
with a hydroxide ion concentration of 6.5 x 10-4
M? Is the solution acidic, basic, or neutral?
pOH

-log (6.5 x 10-4)
pH

10.81
pOH

3.19
basic
What is the pH and the pOH of an aqueous solution
with a hydrogen ion concentration of 3.6 x 10-9
M? Is the solution acidic, basic, or neutral?
pH

-log (3.6 x 10-9)
pOH

5.56
pH

8.44
basic
35
Acids Bases
XI. pOH (potential Hydroxide)
What is the hydrogen ion concentration and the
hydroxide ion concentration of a persons blood
that has a pH of 7.40 at 298 K?
pH

-log H
H

4.0 x 10-8 M
6.60

-log OH-
7.40

-log H

14
7.40

pOH
OH-

2.5 x 10-7 M
What is the hydrogen ion concentration and the
hydroxide ion concentration of an aqueous
solution that has a pH of 2.37 at 298 K?
Multiply HOH- to check your answer
2.37

-log H
11.63

-log OH-
H

4.3 x 10-3 M
OH-

2.3 x 10-12 M
(4.3 x 10-3)
(2.3 x 10-12)

Kw
What is the hydrogen ion concentration and the
hydroxide ion concentration of an aqueous
solution that has a pH of 11.05 at 298 K?
Multiply HOH- to check your answer
11.05

-log H
2.95

-log OH-
H

8.9 x 10-12 M
OH-

1.1 x 10-3 M
(8.9 x 10-12)
(1.1 x 10-3)

Kw
36
Acids Bases
XII. Calculating pH of Strong Acids and
Strong Bases
What is the pH of a 1.0 M HI solution?
pH

-log H
1H (aq)
1HI (aq)

1I- (aq)
pH

-log (1.0)
pH

0.00
1.0 M
1.0 M
1.0 M
What is the pH of a 0.050 M HNO3 solution?
pH

-log H
pH

-log (0.050)
1H (aq)
1HNO3 (aq)

1NO3- (aq)
pH

1.30
0.050 M
0.050 M
0.050 M
What is the pOH of a 2.4 x 10-5 M Mg(OH)2
solution?
1Mg2 (aq)
1Mg(OH)2 (s)

2OH- (aq)
pOH

-log OH-
pOH

-log (4.8 x 10-5)
2.4 x 10-5 M
2.4 x 10-5 M
4.8 x 10-5 M
pOH

4.32
pH

9.68
37
Acids Bases
XIII. Calculating pH of Weak Acids and
Weak Bases
What is Ka of a 0.100 M formic (methanoic) acid
solution with pH 2.38?
1HCOO-(aq)
1HCOOH (aq)
1H (aq)

0.100 M
4.2 x 10-3 M
4.2 x 10-3 M
pH

-log H
H

4.2 x 10-3 M
2.38

-log H
HCOO-

4.2 x 10-3 M
HCOOH

4.2 x 10-3 M
0.100 M
-
HCOOH

0.0042 M
0.100 M
-
HCOOH

0.096 M
HCOO-
H
(4.2 x 10-3 )
(4.2 x 10-3 )
Ka

Ka

HCOOH
(0.096 )
Ka

1.8 x 10-4
38
Acids Bases
XIII. Calculating pH of Weak Acids and
Weak Bases
What is Ka of a 0.220 M arsenic acid solution
with pH 1.50?
1H2AsO4-(aq)
1H3AsO4 (aq)
1H (aq)

0.220 M
3.2 x 10-2 M
3.2 x 10-2 M
pH

-log H
H

3.2 x 10-2 M
1.50

-log H
H2AsO4-

3.2 x 10-2 M
H3AsO4

3.2 x 10-2 M
0.220 M
-
H3AsO4

0.032 M
0.220 M
-
H3AsO4

0.188 M
H2AsO4-
H
(3.2 x 10-2 )
(3.2 x 10-2 )
Ka

Ka

H3AsO4
(0.188 )
Ka

5.4 x 10-3
39
Acids Bases
XIII. Calculating pH of Weak Acids and
Weak Bases
What is Ka of a 0.0400 M chlorous acid solution
with pH 1.80?
1ClO2-(aq)
1HClO2 (aq)
1H (aq)

0.0400 M
1.6 x 10-2 M
1.6 x 10-2 M
pH

-log H
H

1.6 x 10-2 M
1.80

-log H
ClO2-

1.6 x 10-2 M
HClO2

1.6 x 10-2 M
0.0400 M
-
HClO2

0.016 M
0.0400 M
-
HClO2

0.024 M
ClO2-
H
(1.6 x 10-2 )
(1.6 x 10-2 )
Ka

Ka

HClO2
(0.024 )
Ka

1.1 x 10-2
40
Acids Bases
XIII. Calculating pH of Weak Acids and
Weak Bases
What is Ka of a 1.000 M propanoic acid solution
with pH 2.43?
1C3H5O2-(aq)
1HC3H5O2 (aq)
1H (aq)

1.000 M
3.7 x 10-3 M
3.7 x 10-3 M
pH

-log H
H

3.7 x 10-3 M
2.43

-log H
C3H5O2-

3.7 x 10-3 M
HC3H5O2

3.7 x 10-3 M
1.000 M
-
HC3H5O2

0.0037 M
1.000 M
-
HC3H5O2

0.9963 M
C3H5O2-
H
(3.7 x 10-3 )
(3.7 x 10-3 )
Ka

Ka

HC3H5O2
(0.9963 )
Ka

1.4 x 10-5
41
Acids Bases
XIV. Neutralization
-when an ____ and a ____ _____, the resulting
_______ has _________ that are characteristic of
_______ an ____ or a ____
acid
base
react
solution
properties
neither
acid
base
neutralization
reaction
double
-a ____________ _______ is a ______- ___________
_______ in which an ____ and a ____ react in
_______ ________ to produce a ____ and _____
replacement
acid
reaction
base
aqueous
solution
salt
water
2HCl (aq)
1MgCl2 (aq)
1Mg(OH)2 (aq)


2H2O (l)
base
acid
salt
water
Milk of Magnesia is a Magnesium
hydroxide suspension used to neutralize stomach
acid
-a ____ is an _____ _________ made up of the
______ from the ____ and the _____ from the ____
salt
ionic
compound
cation
base
anion
acid
net
ionic
equation
neutralization
-the ___ _____ ________ for a ____________
_______ is
reaction
H (aq)
OH- (aq)

H2O (l)
42
Acids Bases
XIV. Neutralization
Write the complete balanced thermochemical
equations for the following neutralization
reactions and name the products
Nitric acid

Cesium hydroxide
1HNO3 (aq)
1CsNO3 (aq)
1CsOH (aq)


1H2O (l)
base
acid
Cesium nitrate
water
Hydrobromic acid

Calcium hydroxide
2HBr (aq)
1CaBr2 (aq)
1Ca(OH)2 (aq)


2H2O (l)
acid
base
Calcium bromide
water
Sulfuric acid

Potassium hydroxide
2KOH (aq)
1K2SO4 (aq)
1H2SO4 (aq)


2H2O (l)
acid
base
Potassium sulfate
water
43
Acids Bases
XV. Titration
-a _______is a method for determining an
________ ____________ of a solution by _______ a
______ ______ of a _______ solution of ______
____________
titration
unknown
concentration
reacting
known
volume
different
known
concentration
-to find the ________ ___________ of a ______
______ of ____ solution, you can ______ the
solution with a ______ ______ of an ____ solution
of ______ ____________
unknown
concentration
known
volume
base
titrate
known
volume
acid
known
concentration
electronic pH meter
1HCl (aq)
1NaCl (aq)
1NaOH (aq)


1H2O (l)
base
acid
salt
water
1 L HCl sol.
1 mole HCl
1 mole NaOH
1 mL HCl sol.
x
______________

0.001 mole NaOH
x
___________
x
_______________
1000 mL HCl sol.
1 L HCl sol.
1 mole HCl
0.001 mole NaOH
1000 mL NaOH sol.
M

_______________
x
_______________

0.1 M NaOH
10 mL NaOH sol.
1 L NaOH sol.
44
Acids Bases
XV. Titration
What is the molarity of a CsOH solution if 30.0
mL of the solution is neutralized by 26.4 mL of
0.250 M HBr solution?
1HBr (aq)
1CsBr (aq)
1CsOH (aq)


1H2O (l)
1 L HBr sol.
0.250 mole HBr
1 mole CsOH
26.4 mL HBr sol.
x
______________

0.00660 mole CsOH
x
___________
x
_______________
1000 mL HBr sol.
1 L HBr sol.
1 mole HBr
0.00660 mole CsOH
1000 mL CsOH sol.
M

_______________
x
_______________

0.220 M CsOH
30.0 mL CsOH sol.
1 L CsOH sol.
What is the molarity of a nitric acid solution if
20.00 mL of the solution is neutralized by 43.33
mL of 0.1000 M KOH solution?
1HNO3 (aq)
1KNO3 (aq)
1KOH (aq)


1H2O (l)
1 L KOH sol.
0.1000 mole KOH
1 mole HNO3
43.33 mL KOH sol.
x
______________

4.333 x 10-3 mole HNO3
x
______________
x
_______________
1000 mL KOH sol.
1 L KOH sol.
1 mole KOH
4.333 x 10-3 mole HNO3
1000 mL HNO3 sol.
M

_______________
x
_______________

0.2167 M HNO3
20.00 mL HNO3 sol.
1 L HNO3 sol.
45
Acids Bases
XV. Titration
-during the course of a _______, a known _______
of a _______ of known ___________ is added until
the __________ _____ is reached, at which the
_______ of ______ of ____ equals the _______ of
______ of _____
titration
volume
solution
concentration
equivalence
point
number
moles
H
number
moles
OH-
-corresponding closely with the __________ _____
is the ___ _____, at which the ________ changes
_____
equivalence
point
end
point
indicator
color
Adding indicator
Titrating
End Point
46
Acids Bases
XVI. Buffered Solutions
-_______ are _________ that _____ changes in ___
buffers
solutions
resist
pH
buffer
mixture
weak
acid
-a ______ is a _______ of a _____ ____ and its
_________ ____
conjugate
base
Weak acid
Conjugate base
HF (aq)
H (aq)

F- (aq)
Human blood is buffered by the weak acid carbonic
acid (H2CO3) and its conjugate base, hydrogen
carbonate (HCO3-)
HF (aq)
H (aq)

F- (aq)
Equilibrium shifts to the left, lowering H
H2O (l)
H (aq)

OH- (aq)
H2O (l)
H (aq)

OH- (aq)
Equilibrium shifts to the left, lowering OH-
47
Acids Bases
XVI. Buffered Solutions
-a ______ can also be a _______ of a _____ ____
and its _________ ____
buffer
mixture
weak
base
conjugate
acid
Weak base
Conjugate acid
NH3 (aq)
NH4 (aq)

OH- (aq)

H2O (l)
NH3 (aq)
NH4 (aq)

OH- (aq)

H2O (l)
Equilibrium shifts to the left, lowering OH-
H2O (l)
H (aq)

OH- (aq)
H2O (l)
H (aq)

OH- (aq)
Equilibrium shifts to the left, lowering H
48
Acids Bases
XVI. Buffered Solutions
What is the pH of buffer system made by mixing
equal amounts of H2PO4- and HPO42-?
H2PO4- (aq)
H(aq)
HPO42- (aq)

H
HPO42-
Ka

H2PO4-
H
HPO42-
6.2 x 10-8

H2PO4-
6.2 x 10-8

H
(6.2 x 10-8)

pH
-log
pH

7.21