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Chapter 15 Review

Total questions: 30

Worksheet time: 3hrs 30mins

Name
Class
Date
1.

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

2.

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

3.

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

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

4.
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
5.

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

6.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

7.

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

8.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

9.

The _____ is the thing being dissolved.

a)

solute

b)

solvent

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.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
12.

Using the graph above, solubility of which compound is influenced the most by changes in temperature?

a)

KCl

b)

NaCl

c)

K2Cr2O7

d)

KClO3

13.

The molal boiling point elevation and freezing point depression constants depend upon...

a)

enthalpy change.

b)

nature of the solvent.

c)

nature of solute.

d)

vapour pressure of the solution.

14.

. We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and ‘C’ with concentrations 0.1M, 0.01M and 0.001M, respectively. The value of van’t Hoff factor for these solutions will be in the order __________ .

a)

iA < iB > iC

b)

iA = iB = iC

c)

A < iB < iC

d)

iA > iB > iC

15.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

16.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

17.

How could you change a saturated solution to an unsaturated solution?

a)

Add solvent

b)

Add solute

18.

Determine the solubility for the substances at 55'C and arrange them in order from lowest to highest solubility.

a)

NaCl, NH4Cl, KBr, NaNO3

b)

NaCl, NH4Cl, NaNO3, KBr

c)

NH4Cl, NaCl, NaNO3, KBr

d)

NaNO3, KBr, NH4Cl, NaCl

19.

Colligative properties of solutions are those properties that depend on

a)

the amount of solute only

b)

the identity of solute only

c)

both the identity and the amount of solute

20.

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

a)

1

b)

2

c)

3

d)

4

e)

5

21.

Styrene glycol (C8H10O2) is a plasticizer. How many grams of stryrene glycol must be dissolved in 98.7 g of benzene to raise the boiling point by 8.57 degrees C? Kb for benzene is 2.67 degrees C / m.

a)

.098 g

b)

138 g

c)

3.21 g

d)

43.8 g

22.

Ethylene Glycol (C2H6O2) is the principal ingredient in antifreeze. How many grams of ethylene glycol will be needed to lower the freezing point of 2100 grams of water by 20 Co? Kf for water is 1.86 Co/m

a)

10.75 g

b)

1400 g

c)

22.58 g

d)

62 g

23.

Using the graph above, solubility of which compound is influenced the most by changes in temperature?

a)

KCl

b)

NaCl

c)

K2Cr2O7

d)

KClO3

24.

Which of the following statements is TRUE?

a)

Ionic solutes affect colligative properties more than covalently bonded solutes because they produce more moles of solute in solution.

b)

Ionic solutes affect colligative properties less than covalently bonded solutes because they produce less moles of solute in solution.

c)

Covalent solutes affect colligative properties more than ionically bonded solutes because they produce more moles of solute in solution.

d)

Covalent solutes affect colligative properties less than ionically bonded solutes because they produce more moles of solute in solution.

25.

At the same concentration, which of the following will elevate (increase) boiling point the most?

a)

CH3OH

b)

C6H12O6

c)

KNO3

d)

SrCl2

26.

Examine the models below. Assuming the same concentration, which would affect colligative properties more?

a)

beaker A

b)

beaker B

27.
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
28.
What observation(s) reflect(s) colligative properties?
I. A 0.5 m NaBr soln has a higher vapor pressure than 0.5 m BaCl2 soln.
II. A 0.5 m NaOH soln freezes at a lower T. than pure water.
III. Pure water freezes at a higher T than pure methanol.
a)
only I
b)
only II
c)
only III
d)
1 & II
29.
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
30.

142 g of sodium sulfate, Na2SO4, are dissolved in 875 g of H2O. (Assume 100% ionization)

What will be the freezing point of the resulting solution?

(MM Na2SO4 = 142 g/mol; Kf =1.86)

a)

−4.3 oC

b)

−4.5 oC

c)

−3.8 oC

d)

−6.4 oC

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