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CP U13 - Solutions

Total questions: 36

Worksheet time: 6hrs 0mins

Name
Class
Date
1.
What is the universal solvent?
a)
salt
b)
sugar
c)
water
d)
ice
2.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

3.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

4.

Which of the following is NOT a unit used to express concentration?

a)

Molality

b)

Molarity

c)

Mass percent

d)

Density

5.

The moles of solute can be determined by multiplying the molarity of the solute by the volume of solvent.

a)

True

b)

False

6.

The formula M1V1 = M2V2 is used when:

a)

dissolving a solute in a solvent

b)

diluting a solution

c)

reacting an acid with a base

d)

determining the pH of an acid

7.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
8.
Molarity is the ratio between moles and ____. 
a)
Grams
b)
Liters
c)
atoms
d)
milliliters
9.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

10.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

11.
Which of the following substances is a heterogeneous substance?
a)
baby oil
b)
rocky road ice cream
c)
salt water
d)
milk
12.
Which of the following substances is a homogeneous solution?
a)
chocolate chip cookie
b)
italian dressing
c)
apple juice
d)
orange juice
13.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

14.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

15.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

16.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

17.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
18.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
19.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
20.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
21.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

22.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

23.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
24.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

25.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

26.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
27.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
28.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
29.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
30.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
31.

Which one of the following diagrams has the lowest vapor pressure?

a)

1

b)

2

c)

3

d)

4

e)

5

32.

Compared to a 0.1 M aqueous solution of NaCl, a 0.8 M aqueous solution of NaCl has a

a)

higher boiling point and a higher freezing point

b)

higher boiling point and a lower freezing point

c)

lower boiling point and a higher freezing point

d)

lower boiling point and a lower freezing point

33.

Compared to the freezing point and boiling point of water at 1 atmosphere, a solution of a salt and water at 1 atmosphere has a

a)

lower freezing point and a lower boiling point

b)

lower freezing point and a higher boiling point

c)

higher freezing point and a lower boiling point

d)

higher freezing point and a higher boiling point

34.

Which one of the following diagrams has the highest boiling point?

a)

1

b)

2

c)

3

d)

4

e)

5

35.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
36.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than

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