Acids, and Bases
Learning Goals
Acids and Bases
1. I can describe acids and bases in terms of their degree of dissociation in water and
concentration of hydronium (H3O+) and hydroxide (OH-) ions. (14.1)
A. I can diagram the dissociation of ions for acids and bases in water at the
molecular level.
2. I can use nomenclature rules to name acids and bases. (14.1)
A. I can name binary acids, (not containing oxygen) using the “hydro” prefix.
B. Given a list of polyatomic ions, I can name oxy-acids using the correct “ic” or
“ous” suffix.
i. I can use “per” and “hypo” prefixes to name derivatives of polyatomic acids.
C. Given names of acids and bases, I can predict chemical formulas.
3. I can use the pH scale to determine the acidic or basic nature of substances. (14.5 & 14.6)
A. I can calculate the pH or pOH from [H3O+] or [OH-].
B. Given the pH or pOH, I can calculate the [H3O+] or [OH-] of a solution.
C. I can use the ion product of water, Kw, to calculate the [H3O+] or [OH-] of a
solution.
4. I can write and predict neutralization reactions for acids and bases. (14.7)
5. I can use titration results to calculate the molarity or volume for a solution of unknown
concentration. (14.8)
Vocabulary
Dissociate
Ionize
Electrolyte
Nonelectrolyte
Hydronium ion
Hydroxide
Acid
Base
Neutral
pH
pOH
Neutralization
Indicator
Titration
Kw (Ion product constant)
[H3O+] / [H+]
[OH-]
Salt
End Point
Titrant
Buret
Erlenmeyer Flask
binary acids
oxy-acids
Achievement Scale
Goal
I can describe the
formation of a
solution at the
molecular level.
C Level
I can identify the
solute and solvent in
a solution.
B Level
I can predict
whether two
substances will be
miscible.
I can identify solutes
as strong
electrolytes, weak
electrolytes or
nonelectrolytes
based on their
degree of
dissociation.
I can use molarity to
calculation
concentration.
I can list which types
of substances are
strong electrolytes,
weak electrolytes,
and nonelectrolytes.
Given a list of
substances, I can
identify which types
of substances are
strong electrolytes,
weak electrolytes,
and nonelectrolytes.
Given the number of
moles and the
volume of solution, I
can calculate the
molarity.
I can calculate the
amount of another
reactant or product
in a chemical
reaction using
stoichiometry and
molarity.
I can describe acids
and bases in terms of
their degree of
dissociation in water
and concentration of
hydronium (H3O+)
and hydroxide (OH-)
ions.
I can use the pH
scale to determine
the acidic or basic
nature of substances.
I can use mole ratio
and molarity to
convert from moles
of one substance to
volume of another
substance.
Given the molarity, I
can calculate the
volume of solution,
moles of a solute, or
grams of a solute
from the given
information.
I can use mole ratio
and molarity to
convert from volume
of one substance to
volume of another
substance.
I can contrast
characteristics of
acids and bases.
I can identify the
acids and bases and
their conjugates in a
chemical reaction.
Given the pH, I can
identify a substance
as an acid, base, or
neutral.
I can calculate pH
and pOH given the
hydronium ion
concentration.
A Level
I can explain using
polarity why
substances are
miscible or
immiscible.
I can explain using
diagram what
occurs when strong
and weak
electrolytes are in
solution.
I can use the
dilution equation to
calculate dilution
quantities and
molarity.
I can use mole ratio,
molar mass, and
molarity to convert
from grams of one
substance to
volume of another
substance.
I can diagram acids
and bases in
aqueous solution
and explain how
strong and weak
acids and bases
dissociate.
I can convert
between pH, pOH,
[H3O+] and [OH-]
given one known
variable.
I can write and
predict
neutralization
reactions for acids
and bases.
I can list the
fundamental
reactants and
products in any
neutralization
reaction.
Given the reactants, I
can predict the
products in a
neutralization
reaction.
Given the reactants,
I can complete and
balance the
neutralization
equation.
Sample Questions
C Level
1)
A
solution of a gas contains 75% nitrogen and 25% oxygen. Which compound is the
solute and which is the solvent?
2)
Li
st three different categories of substances that are strong electrolytes.
3)
W
hat is the molarity of a solution containing 36 moles of HNO3 in 6L of water?
4)
G
iven the following equation, 2NaOH + H2SO4
Na2SO4 + 2H2O, what volume of 6M
NaOH is needed to completely react with 2 moles H2SO4?
5)
Li
st three differences between acids and bases.
6)
A
substance has a pH of 9. Describe the substance as a strong acid, strong base, weak
acid, weak base, or neutral.
7)
W
hat are two products of any neutralization reaction?
B Level
8)
H4 is mixed with water. Will the substances be miscible or immiscible?
C
9)
W
hich of the following substances are weak electrolytes? HNO3, HF, LiOH, NaBr, NH3
10)
W
hat volume of solution is needed to produce a 3M solution from 6 moles of NaOH?
11)
G
iven the following equation, 2NaOH + H2SO4
Na2SO4 + 2H2O, what volume of 6M
NaOH is needed to completely react with 0.5L H2SO4 with a 3M concentration?
12)
I
dentify the acid and base and their conjugate acid and base in the following reaction:
H2O + H3PO4
H2PO4- + H3O+
13)
W
hat is the pH of a solution with a hydronium ion concentration of 2.0 x
14)
10-5M?
W
hat are the products if KOH is mixed with KNO3?
A Level
15)
se a diagram to explain why CH3OH is miscible in water.
16)
U
U
se a diagram to show what happens when KOH is dissolved in water.
17)
Y
our supervisor tells you to make a 3M LiOH solution. If you start with 100mL of a
12M solution, what will your final volume be of the diluted solution?
18)
G
iven the following equation, 2NaOH + H2SO4
Na2SO4 + 2H2O, how many
milliliters of 1M sulfuric acid are needed to completely react with 25.0g NaOH?
19)
E
xplain the difference of dissociation in solution between 6M nitric acid, HNO3, and
6M acetic acid, HC2H3O2. Use diagrams to show the difference.
20)
W
hat is the hydroxide concentration of a solution with a pH of 3.5?
21)
C
omplete and balance a reaction of H3PO4 and Mg(OH)2.
Answers to Sample Problems:
1)
S
olute = oxygen, solvent = nitrogen
2)
St
rong Acids, Strong Bases, Salts
3)
6
M
4)
0.
67L NaOH
5)
A
+
-7
cids: pH<7, pOH>7, [H3O ]>1x10 M, form hydronium ions in water, proton donors,
turn blue litmus red, taste sour; Bases: pH>7, pOH<7, [OH-]>1x10-7M, proton
acceptors, form hydroxide ions in water, turn red litmus blue, feel slippery, taste
bitter
6)
W
eak base
7)
W
ater and salt (ionic compound)
8)
I
mmiscible (polar and nonpolar do not mix)
9)
H
F, NH3
10)
2L
11)
0.5L NaOH
12)
Acid = H3PO4; Base = H2O; Conj. Acid = H3O+; Conj. Base = H2PO4-
13)
14)
15)
16)
17)
4.7
H2O and KNO3
Diagram should show positive and negative polar sections of CH3OH and H2O
aligning.
Diagram should show complete dissociation of K+ and OH- ions.
400mL
18)
19)
20)
21)
312 mL H2SO4
D
iagram should show complete dissociation of the HNO3 and partial dissociation of
HC2H3O2.
3.16 x 10-11M OH2H3PO4 + 3Mg(OH)2
6H2O + Mg3(PO4)2