wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Exam 2023-24 Semester 2

Total questions: 129

Worksheet time: 4hrs 43mins

Name
Class
Date
1.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

2.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

3.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

4.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

5.
What is 50 °C in Kelvin?
a)

223.15

b)

323.15

c)

100.15

d)

50.15

6.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
7.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
8.

Match the following units to their names.

a)

Pressure

1.

mmHg

b)

Volume

2.

L

c)

Temperature

3.

K

d)

Pressure

4.

atm

e)

Moles

5.

mol

9.

Your parents decide that it's time you go visit your grandmother who lives an hour away. When you get to her house, your check the tires and notice what about their pressure.

a)

Increase

b)

Decrease

10.

You shake a can of soda & then open it, decreasing its pressure. What happens to the volume of the carbon dioxide in the soda?

a)

Increase

b)

Decrease

11.

You forgot to bring your basketball inside after playing a game with your friends. When the sun when down, the temperature dropped & it got cold outside. What do you think happened to the volume of the ball?

a)

Increase

b)

Decrease

12.

Let's say you go on a cruise & the ship starts sinking. You inflate a rubber life raft so you will be able to stay afloat until help arrives. When you place the raft in the cold water, the raft shrinks slightly, decreasing its pressure. What happens to the volume of the raft?

a)

Increase

b)

Decrease

13.

The burner of a hot air balloon start heating the air inside the envelope. This continues heating the air, until the balloon inflates all the way & starts to lift off the ground. What happens to the pressure of the balloon as it is being inflated?

a)

Increases

b)

Decreases

14.

Isla, James, and Liam are studying physics. They are discussing about pressure. James says that pressure is

a)

defined as the mass that an object exerts when at rest

b)

measured in Newtons

c)

defined as the number of moles of substance divided by the mass of the substance

d)

defined as the force per unit area

e)

measured in grams

15.

Lily, Hannah, and Ethan are conducting an experiment in their chemistry class. They observe that:

a)

Equal amounts of gases occupy the same volume in their balloons at constant temperature and pressure.

b)

The volume of a fixed amount of gas in Ethan's balloon is inversely proportional to its pressure at constant temperature.

c)

The volume of a fixed amount of gas in Hannah's balloon is directly proportional to its temperature in Kelvin at constant pressure.

d)

The total pressure of a mixture of gases in Lily's balloon is the simple sum of the partial pressure of all of the gaseous compounds.

e)

The rates of effusion of gases from their balloons are inversely proportional to the square roots of their molar masses.

16.

Scarlett, Jackson, and Evelyn are conducting a science experiment in their chemistry class. They are studying Avogadro's law. According to this law:

a)

Equal amounts of gases, like the ones Scarlett, Jackson, and Evelyn are using, will occupy the same volume at constant temperature and pressure.

b)

The volume of a fixed amount of gas, like the one in their experiment, is inversely proportional to its pressure at constant temperature.

c)

The volume of a fixed amount of gas, like the one in their experiment, is directly proportional to its temperature in Kelvin at constant pressure.

d)

The total pressure of a mixture of gases, like the one they are creating, is the simple sum of the partial pressure of all of the gaseous compounds.

e)

The rates of effusion of gases, like the ones they are studying, are inversely proportional to the square roots of their molar masses.

17.

During a science experiment, Mia, David, and Benjamin observed that when they heated a fixed amount of gas at constant pressure, its volume changed. This observation is best explained by which of the following laws?

a)

Equal amounts of gases occupy the same volume at constant temperature and pressure.

b)

The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

c)

The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

d)

The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

e)

The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

18.

Ethan is working in a chemical lab and he has a 25.0 L tank of NH3 at 190°C190\degree C and 5.20 atm. He wants to know how many moles of NH3 are contained in the tank?

He remembers the Ideal gas equation is: PV = nRT

R=0.08206 L.atmmol⋅KR=0.08206\ \frac{L.atm}{mol\cdot K} 0 °C = 273.15 K0\ \degree C\ =\ 273.15\ K

a)

(0.08206 L.atmmol⋅K)(463.15 K)(5.20 atm)(25.0 L)\frac{\left(0.08206\ \frac{L.atm}{mol\cdot K}\right)\left(463.15\ K\right)}{\left(5.20\ atm\right)\left(25.0\ L\right)}

= 0.293 moles NH3

b)

Not enough information given.

c)

(5.20 atm)(25.0 L)(0.08206 L.atmmol⋅K)(190°C) \frac{\left(5.20\ atm\right)\left(25.0\ L\right)}{\left(0.08206\ \frac{L.atm}{mol\cdot K}\right)\left(190\degree C\right)}\ = 8.34 moles of NH3

d)

(5.20 atm)(25.0 L)(0.08206 L.atmmol⋅K)(463.15K)\frac{\left(5.20\ atm\right)\left(25.0\ L\right)}{\left(0.08206\ \frac{L.atm}{mol\cdot K}\right)\left(463.15K\right)}

= 3.42 moles of NH3

19.

Vaporization is the change from

a)

Liquid to Gas

b)

Solid to Liquid

c)

Gas to Solid

d)

Solid to Gas

20.

The fact that water floats in the solid state is know as

a)

Solid

b)

Freezing

c)

Boating

d)

Density Anomaly

21.

A substance with a HIGH specific heat capacity:

a)

Take a long time to heat up and cool down

b)

Never freezes

c)

Takes a short time to heat up and cool down

d)

Is always a solid

22.

What changes for a phase to go through a phase change?

a)

Temperature

b)

Altitude

c)

Location

d)

Energy

23.

Three basic states of matter

a)

Energy, Solids, Gases

b)

Solids, Gases, Plasma

c)

Solids, Gases, Liquids

d)

Solids, Liquids, Plasma

24.

Heterogeneous Mixture

a)

Particles are distributed non-uniformly (Chocolate chip cookie)

b)

Particles are distributed uniformly (Milk, coffee)

25.

Homogeneous Mixture

a)

Particles are distributed non-uniformly (Chocolate chip cookie)

b)

Particles are distributed uniformly (Milk, Coffee)

26.

Match the following

a)

Pure Substance

1.

One element or one compound.

b)

Mixture

2.

Two or more substances not combined.

c)

Element

3.

Contains only one kind of atom.

d)

Compound

4.

Contains two or more kinds of atoms.

27.
Define a Chemical Property
a)
A property which depends on the objects size or matter.
b)
A property of matter not involving in its manifestation a chemical change
c)
A property or behavior of a substance which undergoes a chemical change or reaction.
d)
A property which makes the object smell or taste different.
28.
Boiling point,melting point, and density are some of an element's
a)
pure properties
b)
physical properties
c)
chemical properties
29.

What is the charge of an electron?

a)

-1

b)

0

c)

+1

30.

Which characteristic defines an atom as belonging to a particular element?

a)

atomic mass

b)

atomic number

c)

neutron count

d)

charge

31.

Why do electrons repel other electrons?

a)

They hate each other

b)

They have the same electrical charge

c)

They have opposite electrical charge

32.

Which physicist claimed that electrons are quantized?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

33.

Who claimed that electrons act like a wave?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

34.

The claim that electrons act like a circular standing wave was made by...

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

35.

Which scientist claimed that the location of a particle is uncertain and therefore, unknown?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

36.

All of the following are orbitals EXCEPT:

a)

f

b)

p

c)

d

d)

r

e)

s

37.

How many atomic orbitals are in the f level?

a)

7

b)

14

c)

5

d)

10

38.

How many atomic orbitals are in the p level?

a)

3

b)

6

c)

5

d)

10

39.

How many electrons can the d-sublevel hold?

a)

2

b)

6

c)

5

d)

10

40.

How many electrons can an s orbital hold?

a)

2

b)

1

c)

3

d)

6

41.

Which groups on the periodic table represent the s-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

42.

Which groups on the periodic table represent the d-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

43.

Which groups on the periodic table represent the d-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

44.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
45.

Which subshell letter corresponds to a spherical orbital?

a)

s

b)

p

c)

d

d)

f

e)

not enough information

46.

Which statement is true about "p" orbitals?

a)

A subshell that contains three "p" orbitals.

b)

These orbitals are shaped like dumbbells.

c)

A 3p orbital has a higher energy than a 2p orbital.

d)

All of these statements are true

47.

A principle that states that each electron

occupies the lowest energy orbital available.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

48.

What does Hund's rule state?

a)

An orbital can contain two electrons only if the electrons have opposite spins.

b)

An orbital can contain two electrons only if all other orbitals at that sublevel are empty.

c)

An orbital can contain two electrons only if the electrons have different energy levels.

d)

An orbital can contain two electrons only if all other orbitals in that sublevel contain at least one electron.

49.

The filling of which orbital is represented by the transition metals in period 4?

a)

3d

b)

3s

c)

2s

d)

2p

50.

According to the Pauli exclusion principle, when can two electrons occupy the same orbital?

a)

only if there is no place else to put them

b)

only if they have the same spin

c)

only if they have opposite spins

d)

only if they are alike in all their properties

51.

Which orbital is displayed correctly?

a)

A

b)

B

c)

C

d)

D

52.

Does this orbital diagram follow the Pauli-Exclusion Principle?

a)

YES

b)

NO

53.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
54.

Which electron configuration rule describes how every electron configuration after helium starts with 1s2?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

55.

____: the three dimensional region in an atom where electrons are located.

a)

Atom

b)

Nucleus

c)

Atomic Orbital

d)

Electron Configuration

56.

Which orbital has the greatest amount of energy?

a)

4p

b)

4f

c)

4s

d)

4d

57.

What is the electron configuration of magnesium?

a)

1s2 2s2 2p6 3s3

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p5 3s2

d)

1s2 2s2 2p6 3s2

58.

What is the shape of the p orbital?

a)

Spherical shape

b)

Dumbbell shape

c)

Cubic shape

d)

Tetrahedral shape

59.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

60.

Which of the following units is represented simply by a letter?

a)

orbital

b)

energy level

c)

sublevel

d)

quantum number

61.

Lateral overlap of p-orbitals leads to the formation of

a)

(a) pi-bond

b)

(b) Metallic bond

c)

(c) sigma -bond

d)

(d) lonic bond

62.

This overlapping leads to form

a)

sigma bond

b)

pi-bond

c)

ionic bond

d)

None of these

63.

Two or more atoms bonded together is a....

a)

element

b)

atom

c)

molecule

d)

bond

64.

In an Ionic Bond Valence Electrons are what?

a)

created

b)

destroyed

c)

gained or lost

d)

shared

65.

How many valence electrons does an atom need to become stable?

a)

2

b)

4

c)

6

d)

8

66.

Ionic Bonds occur between what two types of atoms?

a)

metals and metals

b)

Non metals and Non metals

c)

Metals and Non Metals

d)

unknown

67.

Positively charged Atoms are called?

a)

cations

b)

anions

68.

negatively charged atoms are called?

a)

cations

b)

anions

69.

At atom that GAINS 1 electron will have what charge?

a)

+1

b)

+2

c)

-1

d)

-2

70.

At atom loses 2 electrons, its charge becomes what

a)

+1

b)

+2

c)

-1

d)

-2

71.
The roman numeral in a compound name indicates ___________________.
a)
the number of metal ions
b)
the charge of the metal ion
c)
nothing
d)
the number of total ions
72.

Mendeleev was the first person to arrange the elements into a table. How did he arrange the rows?

a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
73.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

74.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
75.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
76.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
77.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

78.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
79.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
80.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
81.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
82.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
83.

What do the periods (rows) represent?

a)

an additional energy level

b)

an additional proton

c)

an additional group

d)

an additional electron

84.

Put the groups of the periodic table in order from group 1A to group 8A (18).

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

1)
2)
3)
4)
85.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

86.

Match the following

a)

lithium

1.

2 energy levels

b)

helium

2.

1 energy level

c)

aluminum

3.

3 energy levels

d)

bromine

4.

4 energy levels

e)

strontium

5.

5 energy levels

87.

​ (a)   is a loss of electrons, which means the element becomes more ​ (b)   . ​ (c)   is a gain of electrons which means the element becomes more ​ (d)  

Choose from the below words
oxidation
positive
reduction
negative
88.

Given the following reaction in acid, what is the coefficient of water in the balanced equation? Fe+2 + Cr2O72- --> Fe3+ + Cr3+

a)

1

b)

3

c)

5

d)

7

e)

none of these

89.

Match the following elements an their oxidation numbers

a)

O2

1.

zero

b)

N in NH3

2.

-3

c)

K in KMnO4

3.

+1

d)

H in H2O

4.

+1

e)

Cl in KClO4

5.

+7

90.

How many electrons are transferred in the following reaction (acid)?

Cd + 2HCl --> CdCl2 + H2

a)

0

b)

1

c)

2

d)

4

e)

none of these

91.

Which of the following is false?

a)

The pattern is that the cation is expressed first in a formula, and then the anion is written.

b)

The oxidation number of any given free element always has to be 0

c)

The oxidation number of a monatomic ion equals the value of the charge of the ion.

d)

The sum of the value of oxidation numbers of all the present atoms in any neutral compound is 0.

e)

None of these is false

92.

Reorder the following steps in balancing a redox reaction in an acidic solution.

a)

Write the half reactions

b)

Balance all elements that are not O or H

c)

Balance O with H2O and H with H+

d)

Determine electrons and balance charge

e)

Combine equations and cancel like terms

1)
2)
3)
4)
5)
93.

To find an oxidizing agent, you need to check the oxidation number of an atom that is before and after the chemical reaction. If the oxidation number is ​ (a)   in the product, then it has ​ (b)   electrons, and the substance went through ​ (c)   . If the oxidation number is ​ (d)   , then it has ​ (e)   electrons and was reduced.

Choose from the below words
more positive
lost
oxidization
more negative
gained
94.

Match the following

a)

oxidation

1.

loss of electrons

b)

reduction

2.

gain of electrons

c)

reducing agent

3.

element that is oxidized

d)

oxidizing agent

4.

element that is reduced

e)

Noodles

5.

The best golden retriever on the planet

95.

This is just reading a diagram--it's to help you "see" how redox works in a battery. Draw a rectangle around the Anode (oxidation portion of the battery)

A
B
96.

Draw a rectangle around the reduction portion (cathode) portion of the battery.

A
B
97.

Match the following using the knowledge you gained from the electrochemical cell questions.

a)

This happens at the anode

1.

oxidation

b)

This happens at the cathode

2.

reduction

c)

The anode becomes

3.

more positive

d)

The cathode becomes

4.

more negative

98.
For the equilibrium reaction
2NH3(g) + 22 kJ ↔ N2(g) + 3H2(g),
which of the following changes would result in the formation of more N2 and H2 at equilibrium?

a)
increasing pressure
b)
increasing temperature
c)
adding N2
d)
removing NH3
99.
2.In the Haber process, gaseous ammonia is produced on an industrial scale by combining nitrogen and hydrogen gases, according to this equation: 
N2(g) + 3H2(g) ↔ 2NH3(g)
The process is exothermic. Which of the following actions will shift the reaction in the forward (product) direction?

a)
Decrease the pressure of the reaction.
b)
Increase the temperature of the reaction.
c)
Reduce ammonia concentration by removing ammonia from the reaction chamber.
d)
Reduce hydrogen concentration by reducing the amount of hydrogen in the reaction chamber.
100.
The principle that states that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:
a)
The principle of equilibrium
b)
Priestley’s principle
c)
Le Chatelier’s principle
d)
Faraday’s principle
101.
What is the effect of changing the concentration of one of the reactants in an equation at equilibrium?
a)
the reaction will stay at equilibrium
b)
the reaction will stop
c)
the reaction will continue to completion
d)
the reaction will shift to re-establish equilibrium.
102.
A system at equilibrium means it is still reacting.
a)
True
b)
False
103.
For an endothermic reaction, heat can be thought of as:
a)
a reactant
b)
a product
c)
either it has no effect
d)
neither it effects both sides equally.
104.
Increasing the concentration of the reactants will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
105.
Increasing the temperature of an exothermic reaction will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
106.
Increasing the pressure on the reaction:
2NO2 (g) ↔ N2O4 (g)
will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
107.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
108.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
109.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
110.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  NO is removed  from the system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
111.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
112.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium will _______.
a)
shift left
b)
shift right
c)
not shift
113.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse
114.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
115.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
116.

Consider the reaction:

PCl5 (g) + heat ⇌ PCl3 (g) + Cl2 (g)

What effect will increasing the temperature have on the equilibrium?

a)

shift to the left

b)

shift to the right

c)

no shift

117.
If the equilibrium constant is much greater than one (K >> 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
118.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
119.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
120.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

vinegar

b)

milk

c)

water

d)

bleach

121.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

122.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

123.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
124.

According to Brønsted-Lowry acid base theory, an acid ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces H+ when added to water

d)

turns phenolphthalein pink

125.

According to Arrhenius acid-base theory, an acid ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

126.

Which reactant in the following equation is acting as a Brønsted-Lowry acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

127.

CO32-(aq) + H2O(l) → HCO3-(aq) + OH-(aq)

Using the above reaction, which species is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

128.

According to Brønsted-Lowry acid base theory, a base ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces OH- when added to water

d)

has a bitter taste

129.

According to Arrhenius acid-base theory, a base ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces OH- in water

d)

turns litmus paper red

Similar Resources on Wayground

Unit 5 Food for All

131 questions

Unit 5 Food for All

quiz

Worksheet

•

9th Grade

APES Unit 3: Ecology

133 questions

APES Unit 3: Ecology

quiz

Worksheet

•

10th - 12th Grade

Combo Q1-3

132 questions

Combo Q1-3

quiz

Worksheet

•

9th - 12th Grade

Meteorology Practice

127 questions

Meteorology Practice

quiz

Worksheet

•

9th - 12th Grade

EC_Semister 1 Exam revision

130 questions

EC_Semister 1 Exam revision

quiz

Worksheet

•

12th Grade

Ag Chem Semester 1 Review

128 questions

Ag Chem Semester 1 Review

quiz

Worksheet

•

9th - 12th Grade

Animal Science review

126 questions

Animal Science review

quiz

Worksheet

•

11th - 12th Grade

Try me

125 questions

Try me

quiz

Worksheet

•

11th Grade