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WorksheetsChem Hon - S2 Final Exam MCQs - Unit 7
Total questions: 72
Worksheet time: 36mins
Name
Class
Date
1.
What is the conjugate base of HF?
a)
F-
b)
H-
c)
HF+
d)
HF2+
2.
Which of the following is NOT a conjugate acid/base pair?
a)
HSO4- and SO42-
b)
NH3 and N3+
c)
HCl and Cl-
d)
H2O and H3O+
3.
Which of the following is the conjugate base in the chemical equation CN- + H2O → HCN + OH-
a)
CN-
b)
H2O
c)
HCN
d)
OH-
4.
HNO3 is a ___ acid.
a)
Monoprotic
b)
Diprotic
c)
Triprotic
d)
Polyprotic
5.
Water is both ___ and ___.
a)
Amphibians and amphiphiles
b)
Amphioxus and amphiprostyle
c)
Amphiploids and amphibrachic
d)
Amphoteric and amphiprotic
6.
Acids ____.
a)
Donate protons
b)
Accept protons
c)
Teleport protons
d)
Explode protons
7.
Which of the following is a conjugate acid/base pair?
a)
HF and F2-
b)
HCl and Cl2-
c)
NaOH and H3O
d)
HNO3 and NO3-
8.
Which of the following is not a name used for acids and bases?
a)
Arrhenius
b)
Brønsted-Lowry
c)
Lewis
d)
Rutherford
9.
Which term is not used interchangeably with the other three?
a)
Proton
b)
Hydrogen ion
c)
Hydroxide ion
d)
Hydronium ion
10.
What is the difference between Arrhenius acids and Brønsted-Lowry acids?
a)
Arrhenius acids produce hydrogen ions in solutions, and Bronsted-Lowry acids donate hydrogen ions in solutions.
b)
Arrhenius acids donate hydrogen ions in solutions, and Bronsted-Lowry acids produce hydrogen ions in solutions.
c)
Arrhenius acids produce hydroxide ions in solutions, and Bronsted-Lowry acids donate hydroxide ions in solutions.
d)
Arrhenius acids donate hydroxide ions in solutions, and Bronsted-Lowry acids produce hydroxide ions in solutions.
11.
What is the formula for a hydronium ion?
a)
H3O2+
b)
HO3+
c)
H3O+
d)
H2O2+
12.
What happens when Arrhenius acids are added to water?
a)
H+ is produced
b)
CO2 is produced
c)
OH- is produced
d)
OH+ is produced
13.
What happens when Bronsted-Lowry bases are added to water?
a)
H+ is accepted
b)
CO2 is accepted
c)
OH- is accepted
d)
OH+ is accepted
14.
Water is a ___? (Select all that apply)
a)
Acid
b)
Base
c)
Conjugate acid
d)
Conjugate base
15.
A conjugate acid/base pair differs by ___.
a)
A neutron
b)
A proton
c)
An electron
d)
An alpha particle
16.
Which of the following is a property of an acid?
a)
Low pH
b)
Releases hydrogen ions in water
c)
Reacts with bases to produce salt and water
d)
All of the above
17.
Which of these is an acid?
a)
NaOH
b)
KOH
c)
LiOH
d)
HCl
18.
Classify the reaction: HCl + NaOH → NaCl + H2O
a)
Acid + Base
b)
Acid + Metal
c)
Acid + Metal Oxide
d)
Acid + Carbonate
19.
Classify the reaction: 2HCl + Zn → ZnCl2 + H2
a)
Acid + Base
b)
Acid + Metal
c)
Acid + Metal Oxide
d)
Acid + Carbonate
20.
Which of the following is a single-replacement reaction?
a)
Acid + Base
b)
Acid + Metal
c)
Acid + Metal Oxide
d)
Acid + Carbonate
21.
What is the molarity of hydrochloric acid if 100 mL of 0.25M NaOH solution is needed to neutralize 50 mL of HCl?
a)
0.25 M
b)
0.5 M
c)
1 M
d)
2 M
22.
What is the name of the acid HNO3, given that NO3- is called nitrate?
a)
Nitric acid
b)
Nitrous acid
c)
Hydronitric acid
d)
Hydrogen nitride
23.
What is the name of the base KOH?
a)
Potassic acid
b)
Potassous acid
c)
Hydropotassic acid
d)
Potassium hydroxide
24.
What is the molarity of nitric acid if 20 mL of 0.25M KOH solution is needed to neutralize 50 mL of HNO3?
a)
0.1 M
b)
0.25 M
c)
0.5 M
d)
1 M
25.
Chemically, an acid is always in the form of _____.
a)
HX
b)
H2X
c)
XOH
d)
XOH2
26.
What products are released if hydrochloric acid reacts with calcium carbonate?
a)
Water
b)
Water and Salt
c)
Water and Salt and Oxygen
d)
Water and Salt and Carbon Dioxide
27.
Which of the following reactions create salts?
a)
Acid + Base
b)
Acid + Metal/Metal Oxide
c)
Acid + Carbonate/Bicarbonate
d)
All of the above
28.
What is the name of NaOH?
a)
Sodium hydroxide
b)
Hydrosodic acid
c)
Sodious acid
d)
Sodic acid
29.
Which of these reactions is classified as a neutralization reaction?
a)
Acid + Base
b)
Acid + Carbonate
c)
Acid + Metal
d)
Acid + Bicarbonate
30.
Neutralization reactions are _____.
a)
Double replacement reactions
b)
A combination of an acid with a base or a metal oxide
c)
All of the above
d)
None of the above
31.
Which of these are a characteristic of a strong acid?
a)
Low concentration of ions
b)
React slower
c)
Completely dissociates/ionizes
d)
Less vigorous reactions
32.
High concentration of ions
a)
High concentration of ions
b)
React slower
c)
More vigorous reactions
d)
More vigorous reactions
33.
For weak acids/bases in a reaction, what type of arrow is used?
a)
Single headed arrow
b)
Double headed arrow
c)
Triple headed arrow
d)
No arrow
34.
For strong acids/bases in a reaction, what type of arrow is used?
a)
Single headed arrow
b)
Double headed arrow
c)
Triple headed arrow
d)
No arrow
35.
How many moles of a strong acid would you need to neutralize a strong base?
a)
Less moles
b)
Same number of moles
c)
More moles
d)
No moles
36.
How many hydrogen atoms do monoprotic atoms contain to donate?
a)
0
b)
1
c)
2
d)
3
37.
What does conductivity measure?
a)
The strength of electrolytic solutions and the relative strength of acids and bases
b)
The volume of a solution
c)
The concentration of a solution
d)
The amount of a solution
38.
Are all weak acids safe?
a)
Yes
b)
No, they are all more dangerous than strong acids.
c)
No, they are all deadly to humankind.
d)
No, some weak acids are not safe.
39.
What is acid/base concentration?
a)
Determining factor that tells how much the acid/base dissociates
b)
How much acid/base is put in a solution
c)
How hard it is to remove an acid/base from a solution
d)
The type of acid/base
40.
What is acid/base strength?
a)
How much acid/base is put in a solution
b)
How hard it is to put an acid/base into a solution
c)
Property of the type of acid/base which indicates how much will dissociate
d)
How many pounds of metal an acid/base can lift above them
41.
If a weak acid is neutralized by a strong base, then what is a possible pH that the solution can be?
a)
pH = 2
b)
pH = 1
c)
pH = 8
d)
pH = 3
42.
If a weak base is neutralized by a strong acid, then what is a possible pH that the solution can be?
a)
pH = 4
b)
pH = 8
c)
pH = 14
d)
pH = 13
43.
When a weak base is neutralized with a weak acid, what is most likely going to be the pH?
a)
pH = 0
b)
pH = 7
c)
pH = 14
d)
pH = 32
44.
What is the pH of a solution with a hydrogen ion concentration of 1 x 10-4 M?
a)
4.0
b)
5.0
c)
6.0
d)
7.0
45.
If the pH of a solution decreases from 5 to 3, how does the hydrogen ion concentration change?
a)
It increases by 2 times.
b)
It increases by 100 times.
c)
It decreases by 2 times.
d)
It decreases by 100 times.
46.
What is the pOH of a solution with a hydroxide ion concentration of (1 x 10-2) M?
a)
2.0
b)
4.0
c)
10.0
d)
12.0
47.
Which of the following is true for a neutral solution at 25°C?
a)
[H+] > [OH-]
b)
[H+] < [OH-]
c)
pH + pOH = 7
d)
pH + pOH = 14
48.
What is the pH of a 0.01 M HCl solution?
a)
1.0
b)
2.0
c)
3.0
d)
4.0
49.
If the pH of a solution is 8, what is the pOH?
a)
6.0
b)
7.0
c)
8.0
d)
14.0
50.
How does the hydrogen ion concentration change if the pH of a solution changes from 4 to 6?
a)
It decreases by 10 times.
b)
It decreases by 100 times.
c)
It increases by 10 times.
d)
It increases by 100 times.
51.
A solution has a pOH of 3. What is its pH at 25°C?
a)
3.0
b)
7.0
c)
11.0
d)
14.0
52.
Which statement is true for a basic solution at 25°C?
a)
pH > 7
b)
pH < 7
c)
pOH > 7
d)
[H+] = [OH-]
53.
What is the pH of a 0.1 M NaOH solution?
a)
1.0
b)
10.0
c)
12.0
d)
13.0
54.
How does the pOH of a solution change if the hydroxide ion concentration increases from (1 x 10-5) M to (1 x 10-3) M?
a)
It increases by 2 units.
b)
It decreases by 2 units.
c)
It increases by 10 units.
d)
It decreases by 10 units.
55.
What type of solution follows the ratio pH > 7?
a)
Neutral solutions
b)
Acidic solutions
c)
Alkaline or basic solutions
d)
None of the above
56.
Which of the following solutions is most acidic?
a)
pH = 1
b)
pH = 4
c)
pH = 7
d)
pH = 10
57.
At what pH do [H+] and [OH-] concentrations equal each other at 25°C?
a)
1.0
b)
5.0
c)
7.0
d)
14.0
58.
What are the characteristics of pH?
a)
Normally positive with units
b)
Normally negative and no units
c)
Normally positive and no units
d)
Normally neutral and no units
59.
Which of the following statements correctly describes the endpoint of a titration?
a)
The point at which the volume of the titration equals the volume of the analyte
b)
The point at which the pH of the solution is neutral
c)
The point at which the indicator permanently changes color
d)
The point at which all the analyte have been dissolved
60.
In an acid-base titration, what is the purpose of using an indicator?
a)
To increase the rate of reaction
b)
To accurately measure the volume of the titrant
c)
To visually signal the equivalence point of the titration
d)
To neutralize the solution after titration
61.
What does a buffer solution do?
a)
It neutralizes all acids and bases
b)
It creates a zone where pH will not change a lot
c)
It is the strongest acid
d)
It is the strongest base
62.
How do you create a buffer solution? (Select all that apply)
a)
Mixing a strong acid with a strong base in equal concentration
b)
Adding weak acid to water and neutralizing with a strong base
c)
Combining a weak acid/base with equal parts conjugate salt
d)
Half neutralizing a weak acid/base with a strong base/acid
63.
What does a pH testing strip do?
a)
To measure the temperature of the solution
b)
To determine the concentration of the solution
c)
To indicate the acidity or alkalinity of a solution
d)
To identify the element in the solution
64.
Which of the following statements is true for indicators?
a)
All indicators have the same properties
b)
Indicators have a specific range to measure the pH of the substance
c)
Indicators only change color in acids or bases
d)
Indicators are not affected by temperature
65.
What is the purpose of titration?
a)
To determine the boiling point of a solution
b)
To measure the concentration of a solution
c)
To separate components of a mixture
d)
To change the color of a solution
66.
Which of the following is typically used as an indicator in acid base titration?
a)
Sodium chloride
b)
Phenolphthalein
c)
Potassium
d)
Copper sulfate
67.
During titration the point at which the indicator changes color is known as
a)
End point
b)
Finish point
c)
Equilibrium point
d)
Neutral point
68.
Which of the following is a common piece of equipment used to deliver the titration in a titration experiment?
a)
Buret
b)
Pipette
c)
Beaker
d)
Graduated cylinder
69.
You have 30 mL of 0.1M solution of HCl (titrant) and a 0.2M solution of NaOH (analyte). How many moles of HCl are used in titration?
a)
0.003 moles
b)
0.006 moles
c)
0.03 moles
d)
0.06 moles
70.
Which of the following best describes an analyte?
a)
A substance used to cause a reaction
b)
A component of a sample being measured or detected
c)
The instrument used to measure chemical substances
d)
A reagent used to calibrate analytical instrument
71.
What does a volumetric pipet do?
a)
To get a specific volume of the analyte solution
b)
Get the mass of the analyte
c)
Get the mole of analyte
d)
To find the temperature of the analyte
72.
An example of buffer solution
a)
Blood
b)
Water
c)
Coke
d)
Coffee
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