Question 1

Question

A)When salt dissolves completely into water, which term is used to describe the water? (1 point)
Responses

concentration
concentration

solvent
solvent

solute
solute

solution
solution
Question 2
A)Which statement best describes what happens when oil and water are stirred together?(1 point)
Responses

Oil molecules will repel each other electrically, leading to complete mixing of the two substances.
Oil molecules will repel each other electrically, leading to complete mixing of the two substances.

Water and oil molecules have opposite electrical charges, causing them to repel each other and separate.
Water and oil molecules have opposite electrical charges, causing them to repel each other and separate.

Oil and water molecules have like charges, causing them to repel each other and separate.
Oil and water molecules have like charges, causing them to repel each other and separate.

Water molecules will attract each other electrically, but they will not attract oil molecules, causing separation.
Water molecules will attract each other electrically, but they will not attract oil molecules, causing separation.
Question 3
A)Salt is dissolved into a water solvent. Can the salt be extracted, and will it retain its properties?(1 point)
Responses

No, it cannot be extracted through any means. It retains its original properties.
No, it cannot be extracted through any means. It retains its original properties.

Yes, it can be extracted through evaporation. It retains its original properties.
Yes, it can be extracted through evaporation. It retains its original properties.

Yes, it can be extracted through evaporation. It does not retain its original properties.
Yes, it can be extracted through evaporation. It does not retain its original properties.

No, it cannot be extracted through any means. It does not retain its original properties.
No, it cannot be extracted through any means. It does not retain its original properties.
Question 4
A)Crystals are made using supersaturated solutions of solids in water. These solutions hold more of the solute than they would at room temperature. How are these solutions made? (1 point)
Responses

The water would need to be heated to a higher temperature, which would give molecules and ions more kinetic energy, increasing solubility.
The water would need to be heated to a higher temperature, which would give molecules and ions more kinetic energy, increasing solubility.

The water would need to be chilled to a lower temperature, which would give molecules and ions more kinetic energy, increasing solubility.
The water would need to be chilled to a lower temperature, which would give molecules and ions more kinetic energy, increasing solubility.

The water would need to be heated to a higher temperature, which would take kinetic energy away from molecules and ions, increasing solubility.
The water would need to be heated to a higher temperature, which would take kinetic energy away from molecules and ions, increasing solubility.

The water would need to be chilled to a lower temperature, which would take kinetic energy away from molecules and ions, increasing solubility.
The water would need to be chilled to a lower temperature, which would take kinetic energy away from molecules and ions, increasing solubility.
Question 5
A)Which substance is most likely to dissolve in greater quantities in cold water? (1 point)
Responses

oxygen
oxygen

sugar
sugar

sodium chloride
sodium chloride

potassium chloride
potassium chloride
Question 6
A)How is a mole related to concentration?(1 point)
Responses

The mass of the solute in a solution is measured in moles.
The mass of the solute in a solution is measured in moles.

The number of particles of solute in a solution is measured in moles.
The number of particles of solute in a solution is measured in moles.

The saturation point of a solution is measured in moles.
The saturation point of a solution is measured in moles.

The volume of particles of solute in a solution is measured in moles.
The volume of particles of solute in a solution is measured in moles.
Question 7
A)How are ionic compounds similar to polar compounds?(1 point)
Responses

Both compound types have oppositely charged regions.
Both compound types have oppositely charged regions.

Both compound types are held together by covalent bonds.
Both compound types are held together by covalent bonds.

Neither compound type is neutral.
Neither compound type is neutral.

Neither compound type dissolves in polar solvents.
Neither compound type dissolves in polar solvents.
Question 8
A)Which feature do polar compounds have that nonpolar compounds lack?(1 point)
Responses

electrons
electrons

ends that have the same charge
ends that have the same charge

oppositely charged ends
oppositely charged ends

ions
ions
Question 9
A)Which statement best describes what it means when something is classified as a strong acid?(1 point)
Responses

It easily dissociates into ions in solution.
It easily dissociates into ions in solution.

It is present in low quantities in a solution.
It is present in low quantities in a solution.

It is present in large quantities in a solution.
It is present in large quantities in a solution.

It resists dissociating into ions in solution.
It resists dissociating into ions in solution.
Question 10
A)The pH of a substance is measured. Which value would identify the substance as a strong base?(1 point)
Responses

7.0
7.0

2.5
2.5

11.0
11.0

8.3
8.3
Question 11
A)
Use the periodic table to answer the question.

























Based on patterns in the periodic table, which list shows the acids in order from strongest to weakest?

(3 points)
Responses

H2S, PH3, HCl
H 2 S, PH 3 , HCl

HCl, H2S, PH3
HCl, H 2 S, PH 3

HCl, PH3, H2S
HCl, PH 3 , H 2 S

PH3, H2S, HCl
PH 3 , H 2 S, HCl
Question 12
A)Which statement correctly explains why H2S is a stronger acid than water?(1 point)
Responses

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, stronger acid than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS – is a more stable, stronger acid than OH – .

Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, stronger acid than H 2 O.

Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, weaker base than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, weaker base than H 2 O.

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, weaker base than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS – is a more stable, weaker base than OH – .
Question 13
A)What is the pH of a 1×10−4
mol HCl solution?(1 point)
Responses

6
6

4
4

8
8

2
2
Question 14
A)A small amount of sodium hydroxide is added to water. When the chemical reaction reaches equilibrium, the pH is 12. Which statement and conclusion about sodium hydroxide is correct?(2 points)
Responses

The negative log of the concentration of OH– ions is 2. Sodium hydroxide is a strong base.
The negative log of the concentration of OH – ions is 2. Sodium hydroxide is a strong base.

The negative log of the concentration of OH– ions is 12. Sodium hydroxide is a strong acid.
The negative log of the concentration of OH – ions is 12. Sodium hydroxide is a strong acid.

The negative log of the concentration of OH– ions is 12. Sodium hydroxide is a strong base.
The negative log of the concentration of OH – ions is 12. Sodium hydroxide is a strong base.

The negative log of the concentration of OH– ions is 2. Sodium hydroxide is a strong acid.
The negative log of the concentration of OH – ions is 2. Sodium hydroxide is a strong acid.
Question 15
A)Ammonia is a weak base. Potassium hydroxide is a strong base. Which statement is correct?(1 point)
Responses

A solution of potassium hydroxide will always have a lesser concentration of solute than a solution of ammonia.
A solution of potassium hydroxide will always have a lesser concentration of solute than a solution of ammonia.

A solution of potassium hydroxide will always have a higher pH than a solution of ammonia.
A solution of potassium hydroxide will always have a higher pH than a solution of ammonia.

A solution of potassium hydroxide will always have greater conductivity than a solution of ammonia.
A solution of potassium hydroxide will always have greater conductivity than a solution of ammonia.

A solution of potassium hydroxide will always have more OH– ions than a solution of ammonia.
A solution of potassium hydroxide will always have more OH – ions than a solution of ammonia.
Question 16
A)A scientist has 500 mL of a 2.1 M stock solution. She dilutes the solution, and the volume of the solution after the dilution is 3.25 L. What is the molarity (M) of the diluted solution? (2 points)
Responses

13.65 M
13.65 M

0.01 M
0.01 M

0.32 M
0.32 M

323.08 M
323.08 M
Question 17
A)
Use the graph to answer the question.

























Which statement is the best explanation for the graph?

(2 points)
Responses

As temperature rises, the space between liquid particles increases, allowing more room for gas particles.
As temperature rises, the space between liquid particles increases, allowing more room for gas particles.

As temperature rises, the space between liquid particles decreases, leaving less room for gas particles.
As temperature rises, the space between liquid particles decreases, leaving less room for gas particles.

As temperature rises, gas particles are moving faster and may leave the solution.
As temperature rises, gas particles are moving faster and may leave the solution.

As temperature rises, gas particles are moving faster and are more likely to enter the solution.
As temperature rises, gas particles are moving faster and are more likely to enter the solution.
Question 18
A)
Use the periodic table to complete the activity.

























Hydrogen selenide (H2Se) reacts with water according to the following equation.

H2Se + H2O → SeH– + H3O+

Identify the acid, base, conjugate acid, and conjugate base in this reaction

(4 points)
H2Se is a(n)


H2O is a(n)

SeH– is a(n)

H3O+ is a(n)

Question 19
A)Which phrase best defines a covalent bond?(1 point)
Responses

weak polar attraction
weak polar attraction

electrons shared between atoms
electrons shared between atoms

strong polar attraction
strong polar attraction

electrons transferred between atoms

Answer 1

Here are the correct answers for the questions you have provided:

Question 1:
A) When salt dissolves completely into water, which term is used to describe the water?
Answer: solvent

Question 2:
A) Which statement best describes what happens when oil and water are stirred together?
Answer: Water molecules will attract each other electrically, but they will not attract oil molecules, causing separation.

Question 3:
A) Salt is dissolved into a water solvent. Can the salt be extracted, and will it retain its properties?
Answer: Yes, it can be extracted through evaporation. It retains its original properties.

Question 4:
A) Crystals are made using supersaturated solutions of solids in water. These solutions hold more of the solute than they would at room temperature. How are these solutions made?
Answer: The water would need to be heated to a higher temperature, which would give molecules and ions more kinetic energy, increasing solubility.

Question 5:
A) Which substance is most likely to dissolve in greater quantities in cold water?
Answer: oxygen

Question 6:
A) How is a mole related to concentration?
Answer: The number of particles of solute in a solution is measured in moles.

Question 7:
A) How are ionic compounds similar to polar compounds?
Answer: Both compound types have oppositely charged regions.

Question 8:
A) Which feature do polar compounds have that nonpolar compounds lack?
Answer: oppositely charged ends

Question 9:
A) Which statement best describes what it means when something is classified as a strong acid?
Answer: It easily dissociates into ions in solution.

Question 10:
A) The pH of a substance is measured. Which value would identify the substance as a strong base?
Answer: 11.0

Question 11:
A) Based on patterns in the periodic table, which list shows the acids in order from strongest to weakest?
Answer: HCl, H2S, PH3

Question 12:
A) Which statement correctly explains why H2S is a stronger acid than water?
Answer: Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, stronger acid than OH–.

Question 13:
A) What is the pH of a 1×10−4 mol HCl solution?
Answer: 4

Question 14:
A) A small amount of sodium hydroxide is added to water. When the chemical reaction reaches equilibrium, the pH is 12. Which statement and conclusion about sodium hydroxide is correct?
Answer: The negative log of the concentration of OH– ions is 2. Sodium hydroxide is a strong base.

Question 15:
A) Ammonia is a weak base. Potassium hydroxide is a strong base. Which statement is correct?
Answer: A solution of potassium hydroxide will always have more OH– ions than a solution of ammonia.

Question 16:
A) A scientist has 500 mL of a 2.1 M stock solution. She dilutes the solution, and the volume of the solution after the dilution is 3.25 L. What is the molarity (M) of the diluted solution?
Answer: 0.32 M

Question 17:
A) Which statement is the best explanation for the graph?
Answer: As temperature rises, gas particles are moving faster and may leave the solution.

Question 18:
A) Identify the acid, base, conjugate acid, and conjugate base in the reaction.

• H2Se is a(n) acid
• H2O is a(n) base
• SeH– is a(n) conjugate base
• H3O+ is a(n) conjugate acid

Question 19:
A) Which phrase best defines a covalent bond?
Answer: electrons shared between atoms

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