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Chem 1 Unit 11 Review: Solutions

Total questions: 47

Worksheet time: 47mins

Name
Class
Date
1.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

2.

The process of dissolving a substance in solution

a)

solvotion

b)

salvation

c)

solvation

d)

salvution

3.

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

4.

When no more solute dissolves the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

supercalifragilisticexpialidocious

5.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

6.

Molality is defined as ________ divided by _____________

a)

liters solution, mols solute

b)

mols solute, liters solvent

c)

kg solvent, mols solute

d)

mols solute, kg solvent

7.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

8.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

9.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

10.
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
11.
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
12.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
13.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
14.
When Koolaid mix is light colored and tastes watery it is a _______ solution.
a)
saturated 
b)
diluted
15.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
16.
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
17.
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
18.
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
19.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
20.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
21.
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. 
22.

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

23.

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

24.

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.

25.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

26.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
27.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
28.
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
29.

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

30.

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

31.

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

32.

What is a suspension?

a)

A mixture of two or more materials that separate on standing.

b)

How hard of soft an object is when it hits against another object.

c)

A mixture between two or more materials that mix together.

33.

Fog

a)

solution

b)

Suspension

c)

Colloid

d)

alloy

34.

sand in water

a)

solution

b)

colloid

c)

suspension

d)

alloy

35.

snow globe

a)

solution

b)

suspension

c)

alloy

d)

colloid

36.

What is it called when light passes through a colloid and scatters/spreads out

a)

tyndall effect

b)

spreading out effect

c)

fog effect

d)

substance effect

37.

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

38.

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

39.

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

40.

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

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

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

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

43.

Adding a nonvolatile solute to a liquid will ___.

a)

depress both the freezing point and the boiling point

b)

elevate both the freezing point and the boiling point

c)

depress the freezing point and elevate the boiling point

d)

elevate the freezing point and depress the boiling point

44.

Covalent/molecular species always have a van’t Hoff factor of (a)   .

45.
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
46.
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
47.

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

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