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HONORS Unit 5 Solutions

Total questions: 160

Worksheet time: 4hrs 47mins

Name
Class
Date
1.

Solid or liquid that is being dissolved? (a)  

Choose from the below words

solute

solvent

solution

solubility

2.

When no more solute will dissolve in solution and has reached maximum. The rest settles to the bottom of container?

a)

Solubility

b)

Super Saturated

c)

Saturated

d)

Unsaturated

3.

Molarity is defined as ______ per _____.

a)

grams solvent, mols solute

b)

liters solution, mols solute

c)

mols of solvent, liters solute

d)

mols solute, liters solvent

4.

A solution not in equilibrium with a given dissolved substance in which more solute can be added.

a)

saturated

b)

unsaturated

c)

super saturated

d)

solvent

5.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility?

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

6.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

7.

True or False? The higher the concentration of a solution the less solutes it has in it.

a)

True

b)

False

8.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

55 g

d)

33 g

9.

Which solute does not increase in solubility as temperature rises?

a)

NH3

b)

NaNO3

c)

KNO3

d)

NaCl

10.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

11.

How many grams are soluble in 100 g of water at 100 ºC?

a)

300 grams

b)

250 grams

c)

100 grams

d)

50 grams

12.

What does it mean to dilute a solution?

a)

lower the concentration of solute per solvent

b)

increase the concentration of solute per solvent

13.

Which gas is the most soluble at 20 oC?

a)

Helium

b)

Nitrogen

c)

Carbon dioxide

d)

oxygen

e)

methane

14.

In the expression “like dissolves like,” the word “like” refers to similarity in what?

a)

size

b)

polarity

c)

energy

d)

mass

15.

As temperature increases, solubility of a solid in a liquid

a)

increases

b)

decreases

c)

stays the same

d)

can increase or decrease

16.

As temperature increases, solubility of a gas in a liquid

a)

increases

b)

decreases

c)

stays the same

d)

can increase or decrease

17.

Which gas is the least soluble at 20 oC?

a)

Helium

b)

Nitrogen

c)

Carbon dioxide

d)

oxygen

e)

methane

18.

The van't Hoff factor represents

a)

how much degrees C the temperature will be lowered from freezing

b)

how much degrees C the temperature will be raised from boiling

c)

how many atoms a compound has

d)

the amount of particles which dissociate in an ideal conditions

19.

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

a)

1

b)

2

c)

3

d)

4

e)

5

20.

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

a)

1

b)

3

c)

4

d)

5

e)

6

21.

Colligative properties depend on the _____ of solute particles in solution.

a)

type

b)

number

c)

pH

d)

nature

22.

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

23.

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

24.

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

a)

more than

b)

less than

c)

equal to

25.

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

26.

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

a)

1

b)

2

c)

3

d)

4

e)

5

27.

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

28.

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

29.

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

30.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

31.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

32.

a solution that holds more dissolved solute than is required to reach equilibrium at a given temperature

a)

supersaturated solution

b)

saturated solution

c)

unsaturated solution

d)

suspension

33.

Match the following

a)

dissolution

1.

solution that contains a mixture of a solute and solvent

b)

cohesion

2.

due to the strong bonds of water molecules

c)

adhesion

3.

surfaces of objects are attracted to water

d)

polar

4.

opposite charged ends of a molecule

e)

saturation

5.

amount of solute that can be dissolved in solution

34.

Which would NOT increase the rate at which a sugar cube dissolves?

a)

Reducing the amount of solvent

b)

Crushing the sugar cube

c)

Stirring the solution

d)

Heating the solvent

35.

Three 10 g samples of sugar are represented below.


Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

a)

It has the most volume.

b)

It has the smallest surface area.

c)

It has the largest number of sugar molecules.

d)

It has the fewest bonds between sugar modules.

36.

A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?

a)

As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.

b)

Water molecules, trapped with the KCl crystals, were released after heating.

c)

At lower temperatures the solubility of KCl decreased and recrystallization occurred.

d)

At increased temperatures the solubility of KCl increased and remained too high after cooling.

37.

Which would cause the vapor pressure of a solvent to decrease?

a)

heating

b)

Adding a more volatile solute

c)

Adding a less volatile solute

d)

reducing the volume of the solvent

38.

How do we define a solute?

a)

Usually a liquid, in which other materials dissolve to form a solution

b)

A substance that is dissolved in a solution

c)

A substance with sulfur in it

d)

When a solution contains a mixture of two substances

39.

amount of solute in a given amount of solvent

a)

concentration

b)

saturated

c)

solution

d)

suspension

40.

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

a)

increase

b)

decrease

c)

stay the same

41.

____________ is the process where particles of a solvent completely surround the particles of a solute.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

42.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

43.

A 'dilute' solution is a solution with a _____ concentration

a)

high or strong

b)

normal

c)

low or weak

44.

Solvation will happen if the attractive forces between the solute and solvent particles are stronger than the individual forces inside the solute and solvent themselves.

a)

True

b)

False

45.

Which of these would be most likely to decrease the rate of solvation?

a)

stirring or shaking

b)

breaking the solute into smaller pieces

c)

lowering the temperature

d)

increasing the temperature

46.

The overall energy change that occurs during the solution formation process is called the

a)

Endothermic change

b)

Exothermic change

c)

Heat of solution

d)

Attractive energy change

47.

What is the most common liquid solvent in Chemistry?

a)

Oil

b)

Water

c)

Hydrochloric Acid

d)

Sodium Chloride

48.

Chloroform (CHCl3) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

49.

Octane (C8H18) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

50.

Ethanol (CH3CH2OH) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

51.

Butanol (C4H9OH) in methanol (CH3OH)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

52.

Diethyl ether (CH3OCH3) in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

53.

Methanol (CH3COH) in pentane (C5H12)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

54.

Sodium chloride in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

55.

Sodium chloride in ethanol (CH3CH2OH)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

56.

Sodium chloride in acetone (CH3COCH3)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

57.

Sodium chloride in hexane (C6H14)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

58.

Toluene (C6H5CH3) in chloroform (CHCl3)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

59.

Toluene (C6H5CH3) in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

60.

Toluene (C6H5CH3) in hexane (C6H14)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

61.

Hydrogen peroxide (H2O2) in ethanol (CH3CH2OH)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

62.

Hydrogen peroxide (H2O2) in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

63.

Hydrogen peroxide (H2O2) in hexane (C6H14)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

64.

Napthalene (C10H8) in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

65.

Sodium hydroxide (NaOH) in water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

66.

Sodium hydroxide (NaOH) in chloroform (CHCl3)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

67.

Sodium hydroxide (NaOH) in methanol (CH3OH)

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

68.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

69.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

70.

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)

71.

How do the boiling point and freezing point of a solution of water and calcium chloride at standard pressure compare to the boiling point and freezing point of water at standard pressure?

a)

Both the freezing point and boiling point of the solution are higher.

b)

Both the freezing point and boiling point of the solution are lower.

c)

The freezing point of the solution is higher and the boiling point of the solution is lower.

d)

The freezing point of the solution is lower and the boiling point of the solution is higher.

72.

Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M aqueous solution of NaCl at 1 atmosphere has a

a)

lower boiling point and a higher freezing point

b)

lower boiling point and a lower freezing point

c)

higher boiling point and a higher freezing point

d)

higher boiling point and a lower freezing point

73.

At standard pressure when NaCl is added to water, the solution will have a

a)

higher freezing point and a lower boiling point than water

b)

higher freezing point and a higher boiling point than water

c)

lower freezing point and a higher boiling point than water

d)

lower freezing point and a lower boiling point than water

74.

Which solution will freeze at the lowest temperature?

a)

1 mole of sugar in 500 g of water

b)

1 mole of sugar in 1,000 g of water

c)

2 moles of sugar in 500 g of water

d)

2 moles of sugar in 1,000 g of water

75.

Colligative properties depend on the ​ (a)   of the solute but not the ​ (b)   of the solute.

Choose from the below words
concentration
identity
nature
reactivity
volume
mass
76.

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

77.

Match the following

a)

Solute

1.

The part of the solution that is being dissolved

b)

Solvent

2.

The part of the solution that is dissolving

c)

Dilute

3.

Contains more solvent than solute

d)

Concentrate

4.

Contains more solute than solvent

78.

What was one surprising experimental result of the photoelectric effect?

a)

The number of ejected electrons is independent of light intensity.

b)

The kinetic energy of ejected electrons is independent of light frequency.

c)

The photoelectric effect occurs only with visible light.

d)

The kinetic energy of ejected electrons is independent of light intensity.

79.

Which property of light affects the kinetic energy of ejected electrons in the photoelectric effect?

a)

Intensity

b)

Wavelength

c)

Frequency

d)

Amplitude

80.

How quickly does the photoelectric effect occur when light is shone on a metal?

a)

Delayed by seconds

b)

Delayed by minutes

c)

Instantaneous

d)

Delayed by hours

81.

What happens when the frequency of light is increased in the photoelectric effect?

a)

The number of ejected electrons increases.

b)

The intensity of light increases.

c)

The wavelength of light increases.

d)

The kinetic energy of ejected electrons increases.

82.

What was the classical theory of light before the discovery of the photoelectric effect?

a)

Light is a stream of particles.

b)

Light is a sound wave.

c)

Light is a gravitational wave.

d)

Light is an electromagnetic wave.

83.

What concept did the photoelectric effect help to establish?

a)

Classical wave theory

b)

Newtonian mechanics

c)

Quantum nature of light

d)

General relativity

84.

What happens if the frequency of light is below the threshold frequency in the photoelectric effect?

a)

No photoelectric effect occurs below the threshold intensity.

b)

No photoelectric effect occurs below the threshold frequency.

c)

The photoelectric effect occurs with reduced intensity.

d)

The photoelectric effect occurs with increased intensity.

85.

What is a historical fact about the discovery of the photoelectric effect?

a)

The photoelectric effect was discovered before electrons were discovered.

b)

The photoelectric effect was discovered after electrons were discovered.

c)

The photoelectric effect was discovered at the same time as electrons.

d)

The photoelectric effect was discovered by the same person who discovered electrons.

86.

A particle of light is called a...

a)

Photoelectron

b)

Photon

c)

Proton

d)

Electron

87.

The only way to increase the number of photoelectrons emitted is by increasing the _________ of the light

a)

Intensity

b)

Wavelength

c)

Frequency

d)

Energy

88.

What color of light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

89.
This image is an illustration of
a)
photoelectric effect
b)
Dalton's atomic theory
c)
Bohr model
d)
Quantum mechanical model
90.
Which of the following type of electromagnetic radiation has the most energy
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
91.

The energy in joules of a photon of wavelength 355 nm is

a)

5.596 x 1019 J

b)

5.596 x 1028 J

92.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
93.
Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 × 10 10 1/s.
a)
6.63 x 10-34 J
b)
5.25 x 1014 J
c)
5.24 x 10-23 J
d)
1.19 x 1044 J
94.
Light has characteristics of both a wave and a ____________.
a)
amplitude
b)
freqency
c)
joule
d)
photon
95.

A beam of light has a wavelength of 600 nm in air. What is the frequency of the light (c = 3x108 m/s)?

a)

5 x 1014 Hz

b)

2 x 1014 Hz

c)

3 x 1014 Hz

d)

6 x 1014 Hz

96.
Solve this problems using the equation: 
C = λν
If an AM radio station broadcasts at
9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
302 m
97.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
98.

Which of the following is the relationship between Absorbance and the Transmission of light?

a)

A= antilog of - %T

b)

A= - log T

c)

A= log 100/ T

d)

A= -log 1/ T

99.

A student finds the percent transmittance and the absorbance of the 0.10 M solution at different wavelengths. She creates the two graphs below. What is the optimum wavelength for analysis?

a)

600 nm

b)

400 nm

c)

510 nm

d)

440 nm

100.

What is the unit of absorbance which can be derived from Beer Lambert’s law?

a)

L mol-1 cm-1

b)

L gm-1 cm-1

c)

Cm

d)

No unit

101.

How do we make a dilution?

a)

Add more solute

b)

Remove solute

c)

Remove solvent

d)

Add more solvent

102.

Which of the following statements is correct??

a)

Spectrophotometry allows for a correlation to be made between samples

b)

Spectrophotometry allows for a correlation to be made between patient absorbance

c)

Spectrophotometry allows for a correlation to be made between absorbance and concentration

d)

Spectrophotometry allows for a correlation to be made between the concentration of each sample

103.

What passes through your sample to give you an absorbance reading?

a)

Water

b)

Blank solution

c)

Biuret

d)

Light

104.

A spectrophotometer uses _______________ of a certain wavelength to determine the ________________ of a solution.

a)

water, color

b)

air, width

c)

compounds, density

d)

light, concentration

105.

The equation for Beer's law is ......

a)

M1V1 = M2V2

b)

A = bcd

c)

E = mc2

d)

A = Ebc

106.

The relationship between concentration and absorbance in Beer's law is .......

a)

direct

b)

inverse

c)

exponential

d)

unknown

107.

Which of the following is not in the Beer's Law equation?

a)

molar absorptivity

b)

cell path length

c)

light wavelength

d)

concentration

108.

What would happen if we use the wrong wavelength?

a)

there will be little to no absorbance

b)

there will be little to medium absorbance

c)

there will be medium to high absorbance

d)

None of the Above

109.
a)

A

b)

B

c)

A&B

d)

None of the above

110.

Which of the options represent complementary colors?

a)

Blue and Orange

b)

Yellow and Green

c)

Purple and Orange

d)

Yellow and Red

111.

A an outlier is found below the straight line graph of absorbance vs. concentration data. What could have caused this outlier?

a)

a fingerprint on cuvette

b)

drops water not removed from cuvette before adding new solution

c)

excess of compounds is used to solution

112.

Why is it generally preferable to use absorbance as a measure of absorption rather than % Transmittance?

a)

Because %T cannot be measured as accurately as absorbance

b)

Because %T is dependant on the power of the incident radiation

c)

Because absorbance is proportional to the concentration of the analyte, whereas %T is not.

113.

If light passes through water, what will be the %T?

a)

50%

b)

20%

c)

100%

d)

0%

114.

The higher the % Transmittance (%T) the lower the Absorbance (A) of the sample

a)

True

b)

False

115.
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)
116.
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
117.
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-
118.

Which of the following shows the correct net ionic equation for the reaction of Ba(MnO4)2(aq) + (NH4)2SO4?

a)

Ba2+ + SO42- --> BaSO4

b)

2NH4+ + 2MnO4- --> 2NH4MnO4

c)

Ba + MnO4- --> Ba(MnO4)2

d)

2MnO4- + SO42- --> BaSO4

119.

Which of the following shows the correct net ionic equation for Fe(NO3)2 + KOH

a)

Fe3+ + OH- --> Fe(OH)3

b)

Fe2+ + OH- --> Fe(OH)2

c)

2NO3- + 2K+ --> 2KNO3

d)

Fe2+ + 2OH- --> Fe(OH)2

120.

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

121.

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

122.

A substance that conducts an electrical current when dissolved in water is called

a)

catalyst

b)

metalloid

c)

electrolyte

d)

nonelectrolyte

123.

What happens when C12H22O11(s) is dissolved in water?

a)

O-2 ions are attracted to the oxygen atoms of the water

b)

O-2 ions are attracted to the hydrogen atoms of the water

c)

H+ ions are attracted to the hydrogen atoms of the water

d)

No attractions are involved, the crystal just falls apart

124.

Which of the following is not an electrolyte?

a)

KBr

b)

LiOH

c)

RbNO3

d)

CH4

125.
Which pair could be spectator ions?
a)
NH4+ and Cl-
b)
Ca+2 and OH-
c)
Ag+ and Br-
d)
Sr+2 and CO3 -2
126.

What is a Net Ionic Equation?

a)

a balanced chemical equation in which all the reactants and products are given by their chemical formulae.

b)

a chemical equation that shows all soluble species broken into their respective ions.

c)

a chemical equation showing only the species which are actively involved in the reaction.

127.

Which term refers this chemical equation describing potassium chloride in water?

KCl(s) → K+(aq) + Cl-(aq)

a)

dissociation

b)

precipitation

c)

displacement

d)

synthesis

128.

Solid copper(II) chloride

a)

Electrolyte

b)

Non-electrolyte

129.

Copper(II) sulphate solution

a)

Electrolyte

b)

Non-electrolyte

130.

Hydrochloric acid

a)

Electrolyte

b)

Non-electrolyte

131.

Identify the complete ionic reaction for products of this reaction: (final answer is not balanced)

HCl + Mg(OH)2 →

a)

→ MgCl2 + H2O(l)

b)

→ Mg2+ + Cl-1 + H2O(l)

c)

→ Mg2+ + Cl-1 + H+1 + O2-

d)

→ MgCl2 + H2O(l) + CO2(g)

132.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
KMnO4
a)
KMnO4(s) --> K+(aq)+ Mn4+(aq) + O4 -(aq)
b)
KMnO4 --> K++ MnO4 - 
c)
KMnO4(s) --> K+(aq) + MnO4 -(aq)  
d)
KMnO4 --> K++ Mn4+ + O4 -
133.

This beaker represents

a)

complete dissociation

b)

incomplete dissociation

c)

no dissociation

d)

A pure substance

134.

This beaker represents a __________ electrolyte.

a)

strong

b)

weak

c)

non-

135.

This beaker represents a __________ electrolyte.

a)

strong

b)

weak

c)

non-

136.

This beaker represents

a)

complete dissociation

b)

incomplete dissociation

c)

no

137.

The H3O+, OH-, and 3 HOH represent

a)

Water's autoionization

b)

an insoluble solution

c)

a solute

138.

This beaker represents

a)

complete dissociation

b)

incomplete dissociation

c)

no

139.

This beaker shows a __________ electrolyte

a)

strong

b)

weak

c)

non-

140.

What determines whether a polar molecule will be ionized in a polar solvent?

a)

the attraction of the polar solvent is stronger than the covalent bond in the solute

b)

the attraction of the polar solvent is weaker than the covalent bond in the solute

c)

only non-polar molecules are ionized

d)

molecular compounds are never ionized

141.

If an electrical current can run through a solution, it is said to contain

a)

magic

b)

spectator ions

c)

electricity

d)

electrolytes

142.

How many moles of ions are produced when 1 mol of magnesium chlorate are dissolved in water?

a)

1 moles of ions

b)

2 moles of ions

c)

3 moles of ions

d)

4 moles of ions

143.

What makes a solution a WEAK electrolyte?

a)

When the solute completely ionizes in water.

b)

When the solute doesn't dissolve in water.

c)

When the solute partially ionizes in water.

d)

When the solute is not added to the water.

144.

What is a nonelectrolyte?

a)

A substance that dissolves in water and produces ions.

b)

A substance that dissolves in water but doesn't produce ions.

c)

A substance that doesn't dissolve in water.

d)

A substance that vaporizes at room temperature.

145.
Which solution would be least likely to carry an electric current?
a)
NaCl
b)
HCl
c)
C6H12O6
d)
CsI
146.

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

147.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

148.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

149.

Why do we perform a titration?

a)

To determine the concentration of an unknown solution

b)

To see if a reaction will occur between an acid and base

c)

To find the mass of an unknown acid

d)

To find the molar mass of an unknown solution

e)

To calculate the viscosity of the solution

150.

What are some things we will need for a titration?

a)

A solution of known concnetration

b)

A burette

c)

indicator

d)

mass balance

e)

a bunsen burner

151.

If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? (record you answer with the correct unit)

a)

0.043 M

b)

0.034 M

c)

0.065 M

d)

0.77 M

152.

A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 M NaOH. What is the molarity of HCl?

a)

1.6 M HCl

b)

0.03 M HCl

c)

0.6 M HCl

d)

1.2 M HCl

153.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
154.
What is the endpoint of a titration
a)
Where the amount of acid and base are balanced according to the equation
b)
Where there is no base
c)
At the end
155.

A(n) (a)   is a procedure in which a solution of known concentration is used to determine the concentration of an unknown solution.

Choose from the below words
calibration
titration
neutralization
reaction
polymerization
156.

Buret 1: What is the volume in mL of this buret?

(a)  

157.

A 0.125L solution of NaOH is neutralized by 0.0425L of a 0.65 M H2SO4 solution. What is the concentration of the NaOH solution?

a)

0.1 M

b)

1.6 M

c)

0.44 M

d)

None of the above

158.

What is an equivalence point?

a)

It is the point when enough analyte has been added.

b)

It is the point when the amount of added titrant is equal to the amount of analyte in the solution.

c)

It is the point when the volume of titrant is equivalent the volume of analyte.

d)

It is the point when the concentration of titrant added is equivalent to the volume of analyte.

159.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
160.

Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

a)

Q

b)

R

c)

S

d)

T

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