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Worksheets

Solutions

Total questions: 56

Worksheet time: 1hrs 2mins

Name
Class
Date
1.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
2.
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
3.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
4.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
5.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
6.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
7.
When Koolaid mix is light colored and tastes watery it is a _______ solution.
a)
saturated 
b)
diluted
8.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
9.
To make a solute dissolve more quickly i n a solvent which would you do?
a)
Put it in cold water and stir it
b)
Put it in warm water and stir it
10.
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
11.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
12.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
13.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
14.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
15.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
16.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
17.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
18.

Which of the following actions will NOT

increase the rate of dissolution

(dissolving)?

a)

Stirring the solution

b)

Decreasing the temperature

c)

Increasing the surface area of the

solute

d)

Increasing the temperature

19.

You are given a small beaker of solution at room temp. You add a bit of solute to the solution and it dissolves. The solution was:

a)

saturated

b)

unsaturated

c)

concentrated

d)

warm

20.

How do you know when you have a saturated solution?

a)

You don't see anymore material in the solution. It has dissolved.

b)

The material dissolves and no more will dissolve because you see it collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

The solution is clear and there is nothing at the bottom.

21.
Which solution would be least likely to carry an electric current?
a)
NaCl
b)
HCl
c)
C6H12O6
d)
CsI
22.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
23.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
24.
Which of the following is an electrolyte?
a)
sodium chloride
b)
sugar
c)
water
25.
If an electrical current can run through a solution, it is said to contain
a)
magic
b)
nonelectrolytes
c)
electricity
d)
electrolytes
26.
An example of a nonelectrolyte is
a)
sugar water
b)
salt water
c)
sodium chloride
d)
hydrogen chloride
27.
Which of the following is a non-electrolyte?
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
28.

When the ends of two wires, from a circuit containing a battery and a lightbulb, are placed into a beaker containing an aqueous solution the light bulb glows brightly. From this observation, you can conclude the solution is probably —

a)

a concentrated but weak base

b)

a strong acid

c)

a pH neutral sample of a polar compound

d)

an acid added to a base

29.

Which of the following describes a solution containing an electrolyte?

a)

The solute particles are so firmly bonded that they do not

break apart.

b)

The solute particles permit the passage of an electric current.

c)

It is unstable, and all the solute will precipitate if the solution

is disturbed.

d)

It cannot contain any more solute particles

30.

Four chemical solutions are shown above. Which of the following solutions would correspond to a weak electrolyte?

a)

IV

b)

III

c)

II

d)

I and II

31.

Which diagram best illustrates the ion-molecule attractions that occur when the ions of NaCl(s) are added to water?

a)

1

b)

2

c)

3

d)

4

32.

As water is added to a 0.10 M NaCl aqueous solution, the conductivity of the resulting solution

a)

decreases because the concentration of ions decreases

b)

decreases, but the concentration of ions remains the same

c)

increases because the concentration of ions decreases

d)

increases, but the concentration of ions remains the same

33.

A solid substance was tested in the laboratory. The test results are listed below.

• dissolves in water

• is an electrolyte

• melts at a high temperature

Based on these results, the solid substance could be

a)

Cu

b)

CuBr2

c)

C

d)

C6H12O6

34.

Which of the following solutes will result in a solution with the strongest conductivity?

a)

1.0 M C6H12O6

b)

1.0 M MgBr2

c)

2.0 M NaCl

d)

2.0 M CaF2

35.

Which of the following is not an electrolyte?

a)

KBr

b)

LiOH

c)

RbNO3

d)

CH4

36.

When CH3OH is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

3

c)

4

d)

5

e)

6

37.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

38.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

39.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

40.

The graph above is a heating curve of water. Which number in the graph represents the process of freezing?

a)

1

b)

2

c)

3

d)

4

e)

5

41.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
42.
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
43.
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
44.

The van't Hoff factor measures the number of particles formed in solution. What is the van't Hoff factor for the compound Na2SO4?

a)

1

b)

3

c)

5

d)

7

45.

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

a)

are volatile

b)

have higher boiling points

c)

produce fewer moles of solute particles per mole of solvent

d)

produce more moles of solute particles per mole of solvent

46.

The freezing point of water is...

a)

100oC

b)

0oC

c)

-10oC

d)

150oC

47.

The units for molality are _______ of _____ per ____ of ______. (separate four answers with commas)

(a)  

48.

When 11.0 g of CaCl2 dissolves in 45.0 g of water, what is the boiling point of the solution? (Kb = 0.512 oC/m)

a)

3.4

b)

103.4

c)

101.1

d)

1.1

e)

101.4

49.

Find the boiling point of a solution containing 15.0 g sucrose (molar mass = 342.3g/mol), in 100g of water. (Kb = 0.512 oC/m)

a)

100.2

b)

99.8

c)

0.2

d)

-0.2

50.

When 26.0 g of NaCl, are dissolved in 0.5 kg of water, what is the freezing point of this solution? (Kf = 1.86 oC/m)

a)

-3.3

b)

103.3

c)

-1.7

d)

-0.8

51.

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

a)

1

b)

2

c)

3

d)

4

e)

5

52.
Molality is measured in
a)
mols per kg
b)
mols per L
c)
mols per kJ
d)
mols per mL
53.
What is the freezing point of a 1.5 m solution of sucrose in water? (Kf = 1.86°C/m)
a)
-2.8°C
b)
-1.2°C
c)
-0.81°C
d)
0.81°C
54.
A solution has 10 moles of ammonia in 2L of solution. What is the molarity? 
a)
5.0 M
b)
20 M
c)
0.5 M
d)
0.2 M
55.

What mass of Iodine, (molar mass= 253.80 g/mol), must be used to prepare a .960m solution if 100.0g of ethanol, CH3CH2OH, is used? molality= moles of solutekg solventmolality=\ \frac{moles\ of\ solute}{kg\ solvent}  

a)

50.0 g

b)

96.0 g

c)

2.54 g

d)

24.4 g

56.

Colligative properties include

a)

freezing point

b)

boiling point

c)

osmotic pressure

d)

all of the above

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