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Solutions Test Review

Total questions: 53

Worksheet time: 11hrs 57mins

Name
Class
Date
1.
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
2.
When one of the parts of the solution is water we call it _________. 
a)
water stuff 
b)
water mixture 
c)
aqua-man
d)
aqueous 
3.

Which one of the following should be increased in order to increase the solubility of a gas?

a)

Temperature

b)

Pressure

4.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

5.

The process of breaking a solute into postive and negative ions by a solvent to produce a solution is called ______.

a)

solvation

b)

immisciblation

c)

dissociation

d)

dispersion

6.

Water is polar. Which bonds will it dissolve (more than 1 must be checked)?

a)

ionic

b)

metallic

c)

nonpolar

d)

polar

7.
What is the correct formula to solve for the Molarity of a solution that has .4 moles of HCl in 9.5 L of solution?
a)
M = 9.5 L / .4 mol
b)
M1V1=M2V2
c)
M = .4 mol / 9.5 L
d)
none of the other choices
8.

How could you increase the rate of solvation for a solid solute?

a)

Agitating the mixture

b)

use small pieces of solute

c)

increase the temperature of the solvent

d)

all of the above answers will increase the rate of solvation.

9.

The process by which solvent particles surround solute particles

a)

dissociation

b)

molarity

c)

saturated

d)

solvation

10.

Which of the following solutions is the MOST concentrated?

a)

1 M

b)

1.5 M

c)

2.0 M

d)

2.5 M

11.

How can you increase the solubility of a gas?

a)

stir the solution ( agitate)

b)

decrease the pressure

c)

decrease the temperature of the solvent

d)

increase the temperature of the solvent

12.

If more solute is added to a saturated solution....

a)

some of the solute would dissolve

b)

all of the solute would sink to the bottom undissolved

c)

a chemical reaction will occur

d)

everything will dissolve

13.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

14.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

15.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

16.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
17.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

18.

What is occurring in the picture?

a)

dissociation of salt, such as NaCl

b)

crystallization of a supersaturated solution

c)

solvation of sugar

d)

evaporation of glucose

19.

The ___ does the dissolving, while the ____ gets dissolved.

a)

solvent, solute

b)

solute, solvent

c)

solute, solution

d)

solution, solute

20.

There is always more ____ than _____.

a)

solute, solvent

b)

solvent, solute

c)

solvent, solution

d)

solute, solution

21.

The process where solvent particles surround solute particles is called _________.

a)

dissociation

b)

solvation

c)

hydration

d)

solubility

22.

What is shown in the picture?

a)

dissociation

b)

hydration

c)

both dissociation and hydration

d)

neither dissociation nor hydration

23.

At 50°C, 30.0 grams of potassium dichromate can be dissolved into 100 grams of water. If one dissolves 15 grams of potassium dichromate in 100 grams of water at this temperature, a(an) ____ solution forms.

a)

saturated

b)

unsaturated

c)

supersaturated

d)

isotonic

24.

At 50°C, 30.0 grams of potassium dichromate can be dissolved into 100 grams of water. If one dissolves 30 grams of potassium dichromate in 100 grams of water at this temperature, a(an) ____ solution forms.

a)

saturated

b)

unsaturated

c)

supersaturated

d)

isotonic

25.

Ethanol is a polar solvent. Which of the following statements is true?

a)

Water will dissolve into ethanol because water is polar too.

b)

Water will dissolve into ethanol because water is nonpolar.

c)

Oil will dissolve into ethanol because oil is polar too.

d)

Oil will dissolve into ethanol because oil is nonpolar.

26.

Table salt (NaCl) dissolves into water because...

a)

table salt is polar and water is polar too.

b)

table salt is ionic and water is polar.

c)

table salt is nonpolar and water is nonpolar too.

d)

table salt is ionic and water is nonpolar.

27.

To dissolve more oxygen into water, one should...

a)

decrease the pressure and increase the temperature.

b)

increase the pressure and decrease the temperature.

c)

increase the pressure and increase the temperature.

d)

decrease the pressure and decrease the temperature.

28.

Stirring a solution increases the rate of solvation because...

a)

the process brings fresh solvent near the solute.

b)

it increases the kinetic energy of the particles, which increases the solubility.

c)

the process breaks the particles into smaller pieces.

d)

it decreases the surface area of the solute particles.

29.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

30.
Which of the following is LEAST likely to dissolve in water?
a)
nonpolar fats and oils
b)
polar sugar molecules
c)
salt made of a positive sodium ion and a negative chloride ion
d)
all of the substances will dissolve easily in water
31.

In general, which types of compounds dissolve easily in water?

a)
Polar and Nonpolar
b)
Polar and Ionic
c)
Nonpolar and Ionic
d)
Covalent and Nonpolar
32.

How does NaCl dissolve in water? (check all that apply)

a)

the Na ion is attracted to the hydrogen in the water molecule

b)

the Cl ion is attracted to the hydrogen in the water molecule

c)

the Na ion is attracted to the oxygen in the water molecule

d)

the Cl ion is attracted to the oxygen in the water molecule

33.

The separation of ions that occurs when an ionic compound dissolves is called

a)

ionization

b)

dissociation

c)

electronegativity

d)

spectation

34.

The ability of a solute to dissolve into a solvent.

a)

Immiscible

b)

Saturated

c)

Dissociation

d)

Solubility

35.

A substance that is a good conductor of electricity when in solution.

a)

Electrolyte

b)

Miscible

c)

Solute

d)

Suspension

36.

Gases are most soluble at _______ temperatures.

a)

High

b)

Low

c)

Medium

37.

Solids are most soluble at ________ temperatures.

a)

High

b)

Low

c)

Medium

38.

What is the molarity of 0.068 mol of NaCl in 3.8 L of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

39.

How many grams of solute are dissolved in 0.125 L of 5.00 M NaCl (MM = 58.45)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

40.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

8.47 %

e)

11.8 %

41.

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

42.

How many grams of KCl are needed to make 5.50 L of a 0.250 M solution of KCl? (molar mass of KCl = 74.55 g/mol)

a)

1.48 g

b)

103 g

c)

1640 g

d)

3.39 g

43.

How many grams of solute are needed to make125.0 mL of 5.00 M NaCl?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

44.
What will allow more solute to be dissolved in a solvent.
a)
adding more solute
b)
stiring
c)
cooling solution
d)
heat
45.
How does a solution become supersaturated?
a)
dissolve lots of solute 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. 
46.
According to the table which solute is nonpolar.
a)
ammonium chloride
b)
naphthalene
c)
ethanol
d)
urea
47.

What is the percent by mass of a solution made by dissolving 10.0 g of NaCl into 180.0 g of water?

a)

5.26 %

b)

5.56 %

c)

180.0 %

d)

20.0 %

48.
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
49.
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
50.
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
51.

The vapor pressure of a pure solvent is ___________ that of a solution

a)

more than

b)

less than

c)

equal to

52.

Which of the following solutions will have the lowest freezing point?

a)

1.0 mol/L sucrose (C12H22O11)

b)

1.0 mol/L lithium chloride (LiCl)

c)

1.0 mol/L sodium phosphide (Na3P)

d)

1.0 mol/L magnesium fluoride (MgF2)

53.

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

a)

1

b)

2

c)

3

d)

4

e)

5

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