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WorksheetsUnit 12 Solutions, Acids and Bases
Total questions: 85
Worksheet time: 43mins
Name
Class
Date
1.
Which type of mixture has particles that are < 1 nm and appears clear?
a)
Colloid
b)
Suspension
c)
Solution
d)
Precipitate
e)
Mixture
2.
What is the name for the substance that gets dissolved in a solution?
a)
Solvent
b)
Solute
c)
Precipitate
d)
Colloid
e)
Diluent
3.
What property distinguishes a colloid from a true solution?
a)
It settles over time
b)
It conducts electricity
c)
It is homogeneous
d)
It scatters light
e)
It dissolves easily
4.
Which type of mixture is cloudy and separates over time?
a)
Colloid
b)
Solution
c)
Suspension
d)
Alloy
e)
Saturated mixture
5.
Identify the solute and solvent in vinegar (5% acetic acid in water).
a)
Water = solute, acid = solvent
b)
Both are solvents
c)
Acid = solute, water = solvent
d)
Equal parts solute/solvent
e)
Water is the solution
6.
Which type of mixture shows the Tyndall effect but remains stable over time?
a)
Solution
b)
Colloid
c)
Suspension
d)
Precipitate
e)
Alloy
7.
Which statement about 'miscible' liquids is TRUE?
a)
They do not mix
b)
They separate quickly
c)
They mix in all proportions
d)
They only mix when heated
e)
They require a third substance to dissolve
8.
What is the Tyndall effect?
a)
Precipitation of solids
b)
Separation of mixtures
c)
Scattering of light by particles
d)
Ion exchange
e)
Color change in solutions
9.
A solution that holds more than the maximum amount of solute at a given temp is:
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Diluted
e)
Precipitated
10.
Fill in the blank: A (a) solution holds the maximum amount of solute possible at a given temperature.
11.
What happens to the solubility of gases in liquids as temperature increases?
a)
It increases
b)
It remains constant
c)
It decreases
d)
It depends on pressure
e)
It depends on stirring
12.
Which of the following affects the RATE of dissolving but not solubility?
a)
Temperature
b)
Pressure
c)
Stirring
d)
Solvent polarity
e)
Particle polarity
13.
Fill in the blank: Smaller particles dissolve faster because they have more (a) .
14.
What is the molarity of a solution containing 0.5 mol of NaCl in 1.0 L of water?
a)
0.25 M
b)
0.50 M
c)
1.0 M
d)
2.0 M
e)
0.75 M
15.
Which equation relates concentration and volume before and after dilution?
a)
P₁V₁ = P₂V₂
b)
M₁V₁ = M₂V₂
c)
C₁T₁ = C₂T₂
d)
PV = nRT
e)
n = m/M
16.
If you dilute 2.0 M NaOH to make 0.5 M solution in 4.0 L, how much water did you add?
a)
1.0 L
b)
2.0 L
c)
3.0 L
d)
4.0 L
e)
None
17.
How many moles of HCl are in 2.5 L of a 0.75 M solution?
a)
0.75 mol
b)
1.875 mol
c)
2.25 mol
d)
1.25 mol
e)
3.0 mol
18.
To prepare 250 mL of 0.4 M KNO₃, how many grams are needed? (MM = 101.1 g/mol)
a)
5.06 g
b)
10.11 g
c)
8.76 g
d)
12.62 g
e)
6.25 g
19.
What variable has the greatest effect on molarity in a dilution?
a)
Volume of solvent
b)
Mass of solute
c)
Temperature
d)
Moles of solute
e)
Time mixed
20.
Fill in the blank: Molarity (M) is defined as moles of solute per (a) of solution.
21.
What is the correct unit for molarity?
a)
mol/kg
b)
mol/L
c)
g/L
d)
mol/mL
e)
M/L
22.
Diluting a solution from 3.0 M to 1.0 M triples the _____ of the solvent.
a)
volume
b)
concentration
c)
molarity
d)
solute amount
e)
temperature
23.
Which of the following is true about dilution?
a)
The number of moles of solute increases
b)
The concentration increases
c)
The volume decreases
d)
The amount of solute stays the same
e)
The solute evaporates
24.
Which of the following is NOT a colligative property?
a)
Boiling point elevation
b)
Freezing point depression
c)
Vapor pressure lowering
d)
Molarity
e)
Osmotic pressure
25.
Colligative properties depend on the (a) of solute particles.
26.
Adding salt to water affects boiling and freezing how?
a)
Lowers boiling, raises freezing
b)
Raises boiling, lowers freezing
c)
No change
d)
Raises both
e)
Lowers both
27.
What is the formula for freezing point depression?
a)
ΔT = Kf × m
b)
ΔTf = iKf × m
c)
ΔTf = iKf / m
d)
ΔTf = m / iKf
e)
Tf = ΔT × Kf
28.
Calculate the freezing point of 2.0 mol NaCl in 1.0 kg water. (Kf = 1.86)
a)
−1.86°C
b)
−3.72°C
c)
−7.44°C
d)
−2.0°C
e)
0°C
29.
Which solution would have the greatest boiling point elevation?
a)
1.0 m glucose
b)
1.0 m NaCl
c)
1.0 m CaCl₂
d)
0.5 m NaCl
e)
1.0 m CH₃OH
30.
What is the effect of adding a nonvolatile solute to a solvent?
a)
Raises vapor pressure
b)
Lowers vapor pressure
c)
Raises density
d)
Lowers conductivity
e)
Increases polarity
31.
Why does salting icy roads help in winter?
a)
Raises vapor pressure
b)
Lowers water’s freezing point
c)
Raises melting point
d)
Prevents condensation
e)
Removes humidity
32.
Which best explains why pure water freezes at 0°C but salt water doesn’t?
a)
Salt is heavier
b)
Salt absorbs heat
c)
Ions interfere with freezing
d)
Salt evaporates quickly
e)
Salt causes condensation
33.
Which real-world system uses freezing point depression?
a)
Water filtration
b)
Baking bread
c)
Antifreeze in radiators
d)
Electroplating
e)
Water electrolysis
34.
What is the pH of pure water at 25°C?
a)
0
b)
3
c)
7
d)
10
e)
14
35.
Which of the following is a strong acid?
a)
CH₃COOH
b)
H₂CO₃
c)
NH₃
d)
HCl
e)
HF
36.
Which of these is a weak base?
a)
NaOH
b)
KOH
c)
Ba(OH)₂
d)
NH₃
e)
LiOH
37.
What is the [H⁺] in a solution with pH = 3?
(a)
38.
If [OH⁻] = 1.0 × 10⁻⁵ M, what is the pH?
a)
5
b)
7
c)
9
d)
11
e)
14
39.
What happens to pH when a base is added to lemon juice?
a)
pH decreases
b)
pH stays the same
c)
pH becomes neutral
d)
pH increases
e)
pH becomes 0
40.
Complete the dissociation: NaOH → ___ + ___
(a)
41.
Which of the following is true for strong acids?
a)
They do not ionize
b)
They partially dissociate
c)
They are weak electrolytes
d)
They fully dissociate
e)
They have low [H⁺]
42.
The [OH⁻] of a solution is 1.0 × 10⁻³ M. What is the pOH?
(a)
43.
If a solution has pH = 11, it is:
a)
Strongly acidic
b)
Weakly acidic
c)
Neutral
d)
Weakly basic
e)
Strongly basic
44.
What is the titration formula for neutralizing an acid with a base?
a)
M₁V₁ = M₂V₂
b)
MaVa = MbVb
c)
PV = nRT
d)
Ka = [H⁺]/[HA]
e)
M = n/V
45.
In a titration, 25.0 mL of 0.10 M NaOH neutralizes 50.0 mL of HCl. What is [HCl]?
a)
0.050 M
b)
0.10 M
c)
0.20 M
d)
0.25 M
e)
0.05 mol
46.
What volume of 0.50 M H₂SO₄ neutralizes 100.0 mL of 1.0 M NaOH?
a)
50.0 mL
b)
100.0 mL
c)
200.0 mL
d)
25.0 mL
e)
75.0 mL
47.
Write the neutralization reaction: HCl + NaOH →
(a)
48.
What is the Ka expression for a weak acid HA?
a)
[H⁺][A⁻]/[HA]
b)
[HA]/[H⁺][A⁻]
c)
[H⁺]/[HA]
d)
[A⁻]/[H⁺]
e)
1/[Ka]
49.
Which buffer system could maintain a near-neutral pH?
a)
HCl/NaCl
b)
NH₃/NH₄⁺
c)
HNO₃/KNO₃
d)
NaOH/NaCl
e)
H₂SO₄/Na₂SO₄
50.
What is the pH of a solution with [H⁺] = 1.0 × 10⁻⁴ M?
(a)
51.
Why is it dangerous to mix bleach and ammonia?
a)
They explode
b)
They form carbon monoxide
c)
They react endothermically
d)
They form toxic gases
e)
They evaporate rapidly
52.
How do antacids relieve stomach acid discomfort?
a)
Raise body temp
b)
Absorb acid
c)
Neutralize excess HCl
d)
Dilute blood
e)
Produce enzymes
53.
Which pH value represents a strong base?
a)
3
b)
6
c)
7
d)
9
e)
13
54.
Which of the following best defines a Bronsted-Lowry acid?
a)
Electron acceptor
b)
Electron donor
c)
Proton donor
d)
Proton acceptor
e)
Base neutralizer
55.
A solution with a pH of 2 has how much more [H⁺] than a pH of 4?
a)
2×
b)
10×
c)
20×
d)
100×
e)
200×
56.
What is the conjugate base of H₂CO₃?
(a)
57.
Which of the following would NOT affect the rate of dissolving?
a)
Stirring
b)
Surface area
c)
Temperature
d)
Volume of container
e)
Crushing solute
58.
What is the [OH⁻] if the pH is 3?
a)
1.0e−3
b)
1.0e−11
c)
1.0e−7
d)
1.0e−5
e)
1.0e−14
59.
Which lab item is best for accurate acid/base titrations?
a)
Beaker
b)
Graduated cylinder
c)
Buret
d)
Erlenmeyer flask
e)
Watch glass
60.
A titration curve with a pH endpoint of ~8.5 suggests:
a)
Strong acid/strong base
b)
Weak acid/strong base
c)
Weak base/strong acid
d)
Neutral solution
e)
Buffer solution
61.
Which of the following acids would produce the highest conductivity?
a)
HF
b)
HNO₃
c)
H₂CO₃
d)
CH₃COOH
e)
H₃PO₄
62.
Diluting a strong acid affects which of the following?
a)
Ka
b)
Molarity
c)
pKa
d)
Dissociation
e)
Acid strength
63.
Calculate the pOH if [OH⁻] = 6.3 × 10⁻⁶ M.
(a)
64.
If pKa = 4.8 for an acid, which statement is TRUE?
a)
It is a strong acid
b)
It fully dissociates
c)
It is weaker than an acid with pKa = 3.0
d)
It has low Ka
e)
It is neutral
65.
Adding water to an acid makes the solution:
a)
More acidic
b)
More basic
c)
More concentrated
d)
Less concentrated
e)
Neutral
66.
Which describes a buffer solution?
a)
Neutralizes all acids
b)
Made from strong acid/base
c)
Resists pH change
d)
Only works once
e)
Contains water only
67.
Which expression defines pOH?
a)
−log[H⁺]
b)
−log[OH⁻]
c)
log[OH⁻]
d)
1/[OH⁻]
e)
−log Ka
68.
The strongest base among the following is:
a)
NH₃
b)
KOH
c)
NaHCO₃
d)
CH₃NH₂
e)
Ca(OH)₂
69.
A 1.0 M solution of which would be most corrosive?
a)
NaCl
b)
NaOH
c)
HCl
d)
CH₃COOH
e)
H₂O
70.
Ka × Kb = ?
a)
Kw
b)
pH
c)
1
d)
Ka²
e)
10⁻⁷
71.
Which of the following can act as both acid and base?
a)
HCl
b)
H₂O
c)
NH₄⁺
d)
NaCl
e)
CH₄
72.
The color change of an indicator depends on:
a)
Ka
b)
pKa
c)
pH of solution
d)
OH⁻ presence only
e)
Salt concentration
73.
Which factor increases the solubility of a solid solute in water?
a)
Lower temp
b)
Stirring
c)
Larger particle size
d)
More pressure
e)
Less volume
74.
A weak acid has a Ka of 1.0 × 10⁻⁵. What can you infer?
a)
It fully dissociates
b)
It produces strong conjugate base
c)
It only partially dissociates
d)
It is neutral
e)
It has a high pH
75.
Which species is the conjugate acid of NH₃?
(a)
76.
A student adds too much base to a titration. What should they do to correct it?
a)
Keep going
b)
Add more indicator
c)
Restart with new acid sample
d)
Add acid to neutralize
e)
Dilute base
77.
Which of the following is NOT a property of acids?
a)
Sour taste
b)
pH < 7
c)
Slippery feel
d)
Reacts with metals
e)
Turns litmus red
78.
Which value would indicate a weak base?
a)
Ka = 1.0 × 10⁻²
b)
Kb = 1.0 × 10⁻¹²
c)
pKa = 1.0
d)
pH = 13
e)
Kb = 1.0
79.
What is the formula to convert pOH to [OH⁻]?
a)
[OH⁻] = 10^−pOH
b)
[OH⁻] = log pOH
c)
[OH⁻] = 10 × pOH
d)
[OH⁻] = pOH/14
e)
[OH⁻] = −log(pOH)
80.
When 1.0 mol of a strong base dissolves in water, it produces:
a)
No ions
b)
OH⁻ only
c)
H⁺ only
d)
OH⁻ and counterion
e)
Salt and water
81.
Which of the following is a diprotic acid?
a)
HCl
b)
HNO₃
c)
H₂SO₄
d)
H₃PO₄
e)
HF
82.
What volume of 6.0 M HCl is needed to make 500 mL of 1.0 M HCl?
a)
50.0 mL
b)
83.3 mL
c)
100.0 mL
d)
250.0 mL
e)
500.0 mL
83.
Which pair forms a buffer?
a)
HCl + NaOH
b)
HNO₃ + KNO₃
c)
CH₃COOH + CH₃COONa
d)
NaOH + KOH
e)
NH₄Cl + NaCl
84.
Which lab error would most affect titration accuracy?
a)
Using tap water
b)
Using indicator
c)
Overfilling buret
d)
Misreading endpoint color
e)
Using a beaker
85.
How is pKa related to acid strength?
a)
Lower pKa = weaker acid
b)
Higher pKa = stronger acid
c)
Lower pKa = stronger acid
d)
pKa is unrelated
e)
Only Ka matters
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