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T1-ADV. Chemistry Final Revision Quiz

Total questions: 144

Worksheet time: 3hrs 17mins

Name
Class
Date
1.

What is an example of a homogeneous mixture?

a)

A mixture of oil and water

b)

A mixture of sand and water

c)

A mixture of iron filings and sulfur

d)

A solution of salt and water

2.

Give an example of a heterogeneous mixture.

a)

Milk

b)

Pure water

c)

Sugar

d)

Salad

3.

What are the properties of homogeneous mixtures?

a)

Visible boundaries between the substances

b)

Non-uniform composition

c)

The properties of homogeneous mixtures include uniform composition, even distribution of components, and no visible boundaries between the substances.

d)

Uneven distribution of components

4.

List the properties of heterogeneous mixtures.

a)

Heterogeneous mixtures are always in a gaseous state

b)

The properties of heterogeneous mixtures include the ability to be separated by physical means, such as filtration or settling, and the components do not have a uniform composition throughout the mixture.

c)

The components of heterogeneous mixtures have a uniform composition throughout the mixture

d)

Heterogeneous mixtures cannot be separated by physical means

5.

Name a common homogeneous mixture found in households.

a)

Saltwater

b)

Pepperjuice

c)

Sugarmilk

d)

Mudwater

6.

Identify a heterogeneous mixture commonly found in nature.

a)

Soil

b)

Pure water

c)

Iron

d)

Air

7.

How do the particles in a homogeneous mixture distribute?

a)

Evenly throughout the mixture

b)

Only at the bottom of the mixture

c)

Only at the top of the mixture

d)

In random clumps within the mixture

8.

Explain the distribution of particles in a heterogeneous mixture.

a)

Particles in a heterogeneous mixture are only found in the top layer and cannot be separated by physical means.

b)

Particles in a heterogeneous mixture are evenly distributed and can only be separated by chemical means.

c)

Particles in a heterogeneous mixture are unevenly distributed and can be separated by physical means.

d)

Particles in a heterogeneous mixture are evenly distributed and cannot be separated by physical means.

9.

What are the characteristics of a homogeneous mixture?

a)

Uniform composition and properties throughout

b)

Uneven distribution of substances

c)

Varied appearance and texture

d)

Different composition and properties throughout

10.

Describe the characteristics of a heterogeneous mixture.

a)

A heterogeneous mixture contains only one type of substance and cannot be separated by physical means.

b)

A heterogeneous mixture has no visible differences between substances or phases and cannot be separated by physical means.

c)

A heterogeneous mixture has uniform composition and cannot be separated by physical means.

d)

A heterogeneous mixture has visibly different substances or phases and can be separated by physical means.

11.

What are the physical properties of a homogeneous mixture?

a)

Different composition and inconsistent physical properties throughout the mixture.

b)

Visible separation of components and varying physical properties.

c)

Uniform composition and consistent physical properties throughout the mixture.

d)

Unpredictable composition and unstable physical properties.

12.

What are the physical properties of a heterogeneous mixture?

a)

The physical properties of a heterogeneous mixture are uniform throughout the sample

b)

All substances in a heterogeneous mixture are evenly distributed

c)

Heterogeneous mixtures have consistent color, texture, and density

d)

The physical properties of a heterogeneous mixture can vary throughout the sample, such as different colors, textures, and densities.

13.

Provide an example of a homogeneous mixture in the field of chemistry.

a)

Sand and water

b)

Iron filings and sulfur

c)

Sugar and sand

d)

Salt water

e)

Vinegar and oil

14.

Give an example of a heterogeneous mixture in the field of biology.

a)

Milk

b)

Blood

c)

Salad

d)

Air

15.

How can you separate the components of a homogeneous mixture?

a)

Adding more components to the mixture

b)

Shaking the mixture vigorously

c)

Using a hammer to break the mixture into pieces

d)

Using techniques such as filtration, distillation, chromatography, or evaporation.

16.

The breaking apart of the solute by the solvent is

a)

Dissociation

b)

Hydration

c)

Nonpolar

d)

Solvation

17.

Immiscible

a)

describes two liquids that are soluble in one another

b)

describes two liquids that are not soluble in one another

c)

describes a solid or gaseous solute that can be dissolved

d)

the substance that is doing the dissolving

18.

Insoluble

a)

means a solid or gaseous solute cannot be dissolved in a liquid solvent

b)

means a solid or gaseous solute can be dissolved in a liquid solvent

c)

particles that have no regions of opposite charges

19.

What does Aqueous mean?

a)

dissolved in water

b)

dissolved in oil

c)

insoluble

d)

dissolved in a solid

20.

What does it mean when two liquids are soluble in one another?

a)

Hydration

b)

Solute

c)

Miscible

d)

Solvent

21.

When particles have regions of opposite charges, it said to be...?

a)

Polar

b)

Saturated

c)

Solute

d)

Nonpolar

22.

What is the Universal Solvent?

a)

Corn Syrup

b)

Gasoline

c)

Oil

d)

Water

23.

Unsaturated means

a)

the solution has less than the maximum amount of solute being dissolved

b)

the solution has more than the maximum amount of solute being dissolved

c)

the solution has the maximum amount of solute being dissovled

24.

Particles that have no regions of opposite charges are

a)

bipolar

b)

nonpolar

c)

polar

25.

A solution with the maximum amount of solute dissolved

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Solution

26.

What is solubility ?

a)

The substance being dissolved

b)

The maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure

c)

The substance doing the dissolving

d)

The minimum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure

27.

Solution is...?

a)

The general term for a liquid, homogeneous mixture combined physically

b)

The general term for the process of the solvent surrounding the solute particles

c)

The general term for a liquid, heterogeneous mixture combined physically

28.

Solute is

a)

The substance doing the dissolving

b)

Usually water

c)

The substance that is being dissolved

29.

Solvent is

a)

The substance being dissolved

b)

The substance that is doing the dissolving

30.

When a solid solute that can be dissolved in a liquid, the solute is ...?

a)

nonpolar

b)

polar

c)

insoluble

d)

soluble

31.

A __________mixture is a type of mixture with a uniform composition.

a)

homogenous

b)

heterogenous

c)

hypotonic

d)

hypertonic

32.

It is a type of solution into which gases can spontaneously mix in any proportion.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

33.

It is a type of solution which are generally called alloys, where two or more metals are present.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

34.

It is the most common and it can be obtained by the dissolution of a gaseous, liquid, or solid solute.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

35.

#1

a)

Unsaturated

b)

Saturated

c)

Supersaturated

36.

#2

a)

Unsaturated

b)

Saturated

c)

Supersaturated

37.

#3

a)

Unsaturated

b)

Saturated

c)

Supersaturated

38.

When you make a dilution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

39.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

40.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

41.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

42.

Which of the following molarity equations is the correct one for solving for volume

a)

V = M × nV\ =\ M\ \times\ n

b)

V = M÷ nV\ =\ M\div\ n

c)

V = n ÷ MV\ =\ n\ \div\ M

d)

V = n × MV\ =\ n\ \times\ M

43.

You need to make 12.0 L of a 1.7 M solution of sodium bicarbonate, how many moles of sodium bicarbonate would you need for this solution?

a)

0.142 moles NaHCO3

b)

7.96 moles NaHCO3

c)

13.7 moles NaHCO3

d)

20.4 moles NaHCO3

44.

What is the molarity of a solution of HNO3 that contains 0.500 mol of HNO3 and 250 ml of water?

a)

0.002 M

b)

0.5 M

c)

2 M

d)

500 M

45.

What does it mean to dilute a solution?

a)

lower the concentration of solute per solvent

b)

increase the concentration of solute per solvent

c)

increase the amount of solute in solvent

d)

decrease the amount of solvent

e)

none are correct

46.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 mL of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

e)

none are correct

47.

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl?

a)

0.625 g NaCl

b)

36.52 g NaCl

c)

36.5 g NaCl

d)

0.625 mol NaCl

e)

none are correct

48.

Using the supplied solubility curve diagram, determine the temperature at which KNO3 and NH4Cl have the same solubility.

a)

16°C

b)

39°C

c)

25°C

d)

73°C

49.

Using the supplied solubility curve diagram, determine what type of solution would be present if 50 grams of NH3 was dissolved in 100 grams of water at 30°C.

a)

saturated

b)

unsaturated

c)

supersaturated

50.

Using the supplied solubility curve diagram, determine which compound listed below is least soluble at 70°C.

a)

NH4Cl

b)

NaCl

c)

KCl

d)

KNO3

51.

Using the supplied solubility curve, determine the temperature that Ce2(SO4)3 and KClO3 have the same solubility.

a)

26°C

b)

3°C

c)

57°C

d)

80°C

52.

Using the supplied solubility curve, determine the type of solution that is formed if 80 grams of NaNO3 were dissolved in 100 grams of water at 30°C.

a)

saturated

b)

unsaturated

c)

supersaturated

53.

Using the supplied solubility curve, determine which compound listed below is most soluble at 20°C.

a)

NH3

b)

KCl

c)

KClO3

d)

NaNO3

54.

Using the supplied solubility curve, determine the type of solution formed if 10 grams of Ce2(SO4)3 were dissolved in 100 grams of water at 50°C.

a)

saturated

b)

unsaturated

c)

supersaturated

55.

Using the supplied solubility curve, determine how many grams of KNO3 will need to be dissolved in 100 grams of water at 60°C to make a saturated solution.

a)

103 grams

b)

85 grams

c)

124 grams

d)

140 grams

56.

Using the supplied solubility curve, determine the type of solution formed when 60 grams of NH4Cl are dissolved in 100 grams of water at 80°C.

a)

saturated

b)

unsaturated

c)

supersaturated

57.

The the supplied solubility curve shows that when 79 grams of NaNO3 is dissolved in 100 grams of water at 10°C, that a saturated solution will be formed.

a)

True

b)

False

58.

___________ refers to the amount of solute dissolved in a given amount per volume of solution

a)

Concentration

b)

Dilution

c)

Precipitation

d)

None of the above

59.

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 %

60.

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

a)

400 g

b)

40 g

c)

0.25 g

d)

25 g

61.

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 %

62.

How many grams of NaNO3 are needed to prepare 100 g of 15.0 % by mass NaNO3 solution? (MM = 85 g/mol)

a)

15 g

b)

1275 g

c)

12.75 g

d)

150 g

63.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
64.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
65.

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

66.

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

67.

Calculate the molarity of the following solution: 1.0 mole of KCl in 0.750 L of solution.

a)

0.750 M

b)

99 M

c)

1.3 M

d)

2.0 M

68.

What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 0.5 L?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

69.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
70.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

71.

As you remove solvent (evaporate the water) from the solution, the concentration (M) will...

a)

increase

b)

decrease

c)

stay the same

72.

What would be the final volume of a solution if you dissolved 2.5 mol of solute to make 7.5 M solution?

a)

0.33 Liter

b)

18.75 Liter

c)

3 Liter

73.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

74.
If you start with atoms of NaOH and are going to moles of NaOH, how many steps is it?
a)
1
b)
2
c)
3
d)
4
75.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
76.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

77.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
78.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
79.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
80.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
81.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
82.
Mg(s) + 2 HCl(aq)  -->  MgCl₂(aq)   + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
83.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
84.
 CaC₂(s) + 2H₂O(l)   -->   C₂H₂(g)   + Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
85.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of iodine can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
86.
Using the following equation:
4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l)
How many grams of oxygen gas are needed to react with 56.8 grams of ammonia?
a)
45.08 g O2
b)
133.33 g O2
c)
260.77 g O2
d)
75.92 g O2
87.

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

a)

1

b)

2

c)

3

d)

4

e)

6

88.

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

a)

1

b)

2

c)

3

d)

4

e)

5

89.

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

a)

1

b)

3

c)

4

d)

5

e)

6

90.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
91.
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
92.
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
93.

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

a)

more than

b)

less than

c)

equal to

94.

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

a)

1

b)

2

c)

3

d)

4

e)

5

95.

Which of the following solutions will have the lowest freezing point? (Hint: who makes the most particles when dissolved?)

a)

1.0 M C12H22O11

b)

1.0 M LiCl

c)

1.0 M Na3P

d)

1.0 M MgF2

96.

Which of the following compounds will be most effective in melting the ice on the roads when the air temperature is below zero?


a)

sodium iodide (NaI)

b)

magnesium sulfate (MgSO4)

c)

potassium bromide (KBr)

d)

all will be equally effective

97.

Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point?

a)

0.1 mol of C2H5OH

b)

0.1 mol of LiBr

c)

0.2 mol of C6H12O6

d)

0.2 mol of CaCl2

98.

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

99.

Compared to the freezing point of 1.0 M KCl(aq) at standard pressure, the freezing point of 1.0 M CaCl2(aq) at standard pressure is

a)

lower

b)

higher

c)

the same

100.

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

101.

Which solution has the highest boiling point at standard pressure?

a)

0.10 M KCl(aq)

b)

0.10 M K2SO4(aq)

c)

0.10 M K3PO4(aq)

d)

0.10 M KNO3(aq)

102.

The table above gives information about four aqueous solutions at standard pressure.

Which list of solutions is arranged in order from highest boiling point to lowest boiling point?

a)

A, B, D, C

b)

A, C, B, D

c)

C, D, B, A

d)

D, B, C, A

103.

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

a)

1

b)

2

c)

3

d)

4

e)

5

104.

Which solution below has the highest boiling point?

a)

NaCl 1 M

b)

CaCl2 1 M

c)

C6H12O6 1 M

d)

AlCl3 1 M

105.
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
106.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

107.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
108.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
109.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
110.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
111.
In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
112.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
113.
What is the result of the reaction between potassium bromide and ammonium sulfide?
a)
potassium sulfide precipitates
b)
ammonium bromide precipitates
c)
potassium ammonium precipitates
d)
no precipitate is formed
114.

Which is the correct net ionic equation for the reaction of:

AgNO3 (aq) + CaCl2 (aq) -> AgCl (s) + Ca(NO3)2 (aq)

a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
115.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
116.

What is the correct net ionic equation for the reaction between HBr(aq) and LiOH(aq) that produces LiBr(aq) and H2O(l)?

a)

2 H+(aq) + O2-(aq) → H2O(l)

b)

2 H2 (aq) + O2(aq) → 2 H2O(l)

c)

2 H2 (g) + O2(g) → 2 H2O(l)

d)

H+(aq) + OH-(aq) → H2O(l)

117.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq) that produces K2SO4 (aq) and Cu3(PO4)2 (s)?

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

118.

Which is the correct net ionic equation for this reaction?

3KOH(aq) + FeCl3(aq) → 3KCl(aq) + Fe(OH)3(s)

a)

3K+ (aq) + 3Cl- (aq) → 3KCl (s)

b)

Fe3+ (aq) + 3OH- (aq) → Fe(OH)3 (s)

c)

Fe3+ (aq) + Cl- (aq) → Fe(OH)3 (s)

d)

3K+ (aq) + 3OH- (aq) + Fe3+ (aq) + 3Cl- (aq) → Fe(OH)3 (s)

119.

How many moles of particles (what is "i") for the substance Na2CO3?

(a)  

120.

Molality is

a)

the moles of solute in 1g of solvent

b)

the moles of solute in 1g of solution

c)

the moles of solute in 1kg of solvent

d)

the moles of solute in 1kg of solution

121.

What is the molality of a solution containing 2.35g of NaCl in 0.55Kg of water?

a)

0.0731

b)

4.27

c)

0.427

d)

7.31

122.

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

123.

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

124.

What type of substance dissolves in water but does not form ions or conduct electricity?

a)

electrolyte

b)

nonelectrolyte

c)

saturated

d)

insoluble

125.

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

a)

1

b)

2

c)

3

d)

4

e)

5

126.

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

a)

1

b)

2

c)

3

d)

4

e)

5

127.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

128.

How many grams of pyrazine (C4H4N2) would have to be dissolved in 1.50 kg of carbon tetrachloride to lower the freezing point by 4.4 °C? The freezing point constant for carbon tetrachloride is 30. °C/m.

a)

16.7 g

b)

17.6 g

c)

14.8 g

d)

8.3 g

129.

When 0.258 g of a molecular compound, benzoic acid, was dissolved in 40.0 g of benzene, the freezing point of the solution was lowered to 5.23 °C. What is the molecular weight of the benzoic acid?

a)

120 g/mol

b)

122 g/mol

c)

16.4 g/mol

d)

112 g/mol

130.

If 90.0 g of nonionizing C6H12O6, are dissolved in 255 g of H2O, what will be the boiling point of the resulting solution?

a)

101.1 °C

b)

100.1 °C

c)

112.3 °C

d)

102.2°C

131.

What is the osmotic pressure developed by seawater at 25 ◦C. Assume that seawater is a 0.53 M solution of NaCl.

a)

24.3 atm

b)

25.2 atm

c)

25.9 atm

d)

92.25 atm

132.

The colligative property of a solution is

a)

Vapour pressure

b)

Osmotic pressure

c)

Boiling point

d)

Freezing point

133.

The measurement of osmotic pressure can also be used to determine

a)

molecular weights of compounds

b)

atomic weights of compounds

c)

empirical formula of compound

d)

chemical formula

134.

A membrane which only allows solvent molecules to flow through it is called

a)

permeable membrane

b)

transparent membrane

c)

elastic membrane

d)

semipermeable membrane

135.
Ideally, your cells should be in a(n) _______ solution
a)
isotonic
b)
hypertonic
c)
hypotonic
d)
isometric
136.

What is the formula for calculating osmotic pressure?

a)

π=MRT\pi = MRT

b)

π=MRT\pi = \frac{M}{RT}

c)

π=RTM\pi = \frac{RT}{M}

d)

π=M+RT\pi = M + RT

137.

In the osmotic pressure formula π=MRT\pi = MRT , what does RR represent?

a)

Reaction rate

b)

Gas constant

c)

Rate of diffusion

d)

Molar mass

138.

If the osmotic pressure of a solution is 5 atm at 300 K, what is the molarity of the solution? (Assume R = 0.0821 L atm / (mol K))

a)

0.203 M

b)

2.03 M

c)

0.0203 M

d)

20.3 M

139.

What is the osmotic pressure of a 0.5 M NaCl solution at 298 K? (Assume R = 0.0821 L atm / (mol K) and that NaCl fully dissociates into Na+ and Cl-)

a)

12.3 atm

b)

24.6 atm

c)

49.2 atm

d)

6.15 atm

140.

How would the osmotic pressure change if the molarity of the solution is doubled?

a)

It would double

b)

It would halve

c)

It would quadruple

d)

It would remain the same

141.

If the osmotic pressure of a solution is 10 atm at 273 K, what will be the osmotic pressure at 546 K, assuming the molarity remains constant?

a)

5 atm

b)

10 atm

c)

20 atm

d)

40 atm

142.

Given the osmotic pressure ( π\pi ) of a solution, the gas constant (R), and the temperature (T), how can you calculate the molarity (M) of the solution?

a)

M=πRTM = \frac{\pi}{RT}

b)

M=πRTM = \pi RT

c)

M=RTπM = \frac{RT}{\pi}

d)

M=π+RTM = \pi + RT

143.

What is the effect of increasing the temperature on the osmotic pressure of a solution, assuming the molarity remains constant?

a)

Increases the osmotic pressure

b)

Decreases the osmotic pressure

c)

No effect on the osmotic pressure

d)

Initially increases then decreases the osmotic pressure

144.

Which of the following statements is true regarding osmotic pressure?

a)

Osmotic pressure is independent of the nature of the solute.

b)

Osmotic pressure decreases with increase in solute concentration.

c)

Osmotic pressure is a colligative property that depends on the number of solute particles.

d)

Osmotic pressure can be calculated using the formula π=MRT\pi = \frac{M}{RT} .

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