Solutions, Acids, and Bases
I Can Statements
Solutions
1. I can describe the formation of a solution at the molecular level. (12.1)
A. I can use polarity to describe and diagram solubility and predict which substances
are miscible.
2. I can identify solutes as strong electrolytes, weak electrolytes or nonelectrolytes based
on their degree of dissociation. (12.2)
A. I can predict whether solutions will conduct electricity based on the nature of the
solute.
B. I can predict the degree to which solutes will dissociate in solution.
3. I can distinguish between an unsaturated, saturated, and supersaturated solution. (12.3)
4. I can calculate the molarity of a solution. (12.5)
A. I can use molarity as a conversion factor to calculate the moles of a solute or the
volume needed to prepare of a solution.
B. I can use molarity to prepare dilutions.
5. Given the volume and molarity of a solution I can calculate the amount of another
reactant or product in a chemical reaction using stoichiometry. (12.6)
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 compare the relative amount of dissociation for strong and weak acids and
bases. (14.3)
B. I can compare the electrolytic nature of strong and weak acids and bases. (14.3)
C. I can diagram the dissociation of ions for acids and bases in water at the
molecular level.
2. I can use the pH scale to determine the acidic or basic nature of substances. (14.6)
A. I can calculate the pH from [H3O+].
B. Given the pH, I can calculate the [H3O+] or [OH-] of a solution.
3. I can write and predict neutralization reactions for acids and bases. (14.7)
4. I can use titration results to calculate the molarity or volume for a solution of unknown
concentration. (14.8)
Vocabulary
Solution
Solute
Solvent
Concentration
Molarity
Dilution
Soluble
Miscible
Dissociate
Ionize
Electrolyte
Nonelectrolyte
Saturated
Unsaturated
Supersaturated
Hydronium
Hydroxide
Acid
Base
Conjugate Acid
Conjugate Base
Neutral
pH
pOH
Neutralization
Indicator
Titration
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 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.
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 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 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.
I can write and
predict
neutralization
reactions for acids
and bases.
I can list the
fundamental
reactants and
products in any
neutralization
reaction.
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.
Given the reactants, I Given the reactants,
can predict the
I can complete and
products in a
balance the
neutralization
neutralization
reaction.
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)
C
H4 is mixed with water. Will the substances be miscible or immiscible?
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 10-5M?
14)
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
cids: pH<7, pOH>7, [H3O+]>1x10-7M, 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 = H2PO413)
14)
15)
16)
17)
18)
19)
20)
21)
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
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