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FX chem 20 Final Review

Total questions: 162

Worksheet time: 4hrs 12mins

Name
Class
Date
1.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

2.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

3.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
4.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
5.

Chloroform was used as anesthesia and a sedative a long time ago. Which of these is the probable formula of the molecule shown?

a)

Cl2

b)

C6H12O6

c)

CHCl3

d)

CH4

e)

H2O

6.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

7.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free moving electrons.

8.
Choose the set that goes from lowest to highest electronegativity?
a)

Cu, Mg, Sr, Ca

b)

F, Cl, Br, Si

c)

Cs, Rb, Ca, Mg

d)

Zn, Cd, Ag, Cu

9.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
10.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

11.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
12.
What is the molecular shape of a silicon dioxide molecule?
a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

13.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
14.

3 atoms bonded and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

15.

Silicon and carbon react to form silicon carbide. The crystal structure of silicon carbide is similar to that of diamond. Silicon carbide is very hard because

a)

it has a high melting point.

b)

silicon atoms and carbon atoms form triple bonds.

c)

it has a giant network structure with strong covalent bonds.

d)

both silicon and carbon atoms have four outermost shell electrons.

16.

Which type of solid has mobile electrons in the crystal (sea of electrons)?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

17.
This type of solid will have the highest boiling point.
a)
ionic
b)
metallic
c)
network
d)
covalent
18.

Classify the following molecule.

a)

polar

b)

nonpolar

19.

Classify the following molecule as polar or nonpolar: HCl

a)

Polar

b)

Nonpolar

20.

Which of the following formulas represents a polar molecule?

a)

H2

b)

NI3

c)

CO2

d)

CCl4

21.

Which force is only found between polar covalent molecules?

a)

Ionic bond

b)

Dipole Dipole

c)

London Dispersion Force

d)

Covalent bond

22.

In this force, electron movement cause a slight charge at a single instant. This charge is temporary.

a)

Hydrogen bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

23.

Which is not a bond, but is an intermolecular force?

a)

Covalent Bond

b)

Ionic Bond

c)

Hydrogen Bond

d)

These are all bonds

24.

All polar covalent molecules contain:

(Check all that apply)

a)

Hydrogen bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

25.

H2O, NH3, and HF all contain:

(Check all that apply)

a)

Hydrogen Bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

26.

Nonpolar molecules all contain

(Check all that apply)

a)

Hydrogen Bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

27.

What could make London Dispersion Forces stronger?

a)

Heating up the molecules

b)

Heavier molecules

c)

Molecules with more electrons

28.

Which of these forces is always the strongest?

a)

Hydrogen bonds

b)

Dipole Dipole force

c)

London Dispersion force

d)

Ionic bonds

29.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

30.

Which of these is the weakest intermolecular force [IMF]?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

31.

Which intermolecular force [IMF] requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

32.

Which intermolecular force [IMF] is characterized by partial charges?

a)

Dipole-dipole forces

b)

Hydrogen bonding

c)

London dispersion forces

33.

Which intermolecular force [IMF] causes water to have an elevated boiling point?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

34.

Which type of intermolecular force [IMF] does this molecular drawing best represent?

a)

dipole-dipole forces

b)

hydrogen bonding

c)

London dispersion forces

35.

What explains the very high melting and boiling point of water?

a)

Strong dipole-dipole bonds between water molecules

b)

Strong hydrogen bonds between water molecules

c)

Dispersion forces which are present in all molecules

d)

Asymmetrical shape of the polar bonds.

36.

Which substance has the weakest intermolecular forces [IMF]?

a)

Substance A, boiling point of 75 °C

b)

Substance C, boiling point of 25 °C

c)

Substance B, boiling point of 105 °C

d)

Substance d, boiling point of 45 °C

37.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
38.

Which type of bond is being formed in this diagram?

a)

covalent bond

b)

energy bond

c)

ionic bond

39.

Which of the following is the correct Lewis dot between Rb and O?

a)
b)
c)
d)
40.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
41.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
42.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
43.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
44.

What is the formula for Boyle's Law?

a)

P1V1=P2V2

b)

P1V1/P2V2

c)

P1V2=P2V1

d)

P1/V1=P2/V2

45.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
46.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
47.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
48.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
49.

Which best explains why increasing the pressure on a gas decreases the volume of the gas sample?

a)

Increasing the pressure causes the gas particles to hit the container walls more often.

b)

Increasing the pressure on a gas sample moves the gas particles closer together.

c)

Increasing the pressure on a gas sample causes the kinetic energy to increase.

50.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
51.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
52.

There are 40 liters of helium in a balloon at a temperature of 100 K. If the temperature of the balloon is increased to 200 K, what will be the new volume of the balloon?

a)

80 L

b)

45 L

c)

54 L

d)

45.33 L

53.

If a beach ball has a volume of 261 L at a temperature of 502 K, what will be the new temperature of the balloon if the volume decreases to 176 L?

a)

744 K

b)

0.0030 K

c)

339 K

d)

512 K

54.

When the temperature of a gas decreases (with pressure and amount held constant), does the volume increase or decrease?

a)

Unaltered

b)

Remains constant

c)

Increase

d)

Decrease

55.

If the Kelvin temperature of a gas is doubled, the volume of the gas will increase by ____.

a)

A factor of 2

b)

A factor of 1

c)

A factor of 3

d)

A factor of 0.5

56.

If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)

1.29 L

b)

12.36 L

c)

1.29 atm

d)

12.36 atm

57.

Oxygen gas is at a temperature of 40oC when it occupies a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters?

a)

611.84oC

b)

611.84 K

c)

880.33 K

d)

880.33oC

58.

How do you convert Kelvin to Celsius?

a)

Add 273

b)

Subtract 273

c)

You can't convert those

d)

They are the same thing

59.

Which answer shows the correct Combined Gas Law

a)
b)
c)
d)
60.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
61.

A rigid plastic container holds 1.00 L methane gas at 0.9 atm pressure when the temperature is 22.0°C. How much more pressure will the gas exert if the temperature is raised to 44.6°C?

a)

0.97 atm

b)

1.82 atm

c)

0.97oC

d)

1.82oC

62.
Gases have...
a)
A definite shape and volume
b)
A definite shape but no definite volume
c)
No definite shape but a definite volume
d)
No definite shape or volume
63.
What is the variable for this number 122 K
a)
P
b)
T
c)
n
d)
V
64.
What is the variable for this number 1.5 mol
a)
P
b)
T
c)
n
d)
V
65.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
66.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
67.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

68.
What is the variable for this number 9.10 atm
a)
P
b)
T
c)
n
d)
V
69.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
70.

Under which conditions of temperature and pressure does carbon dioxide behave most like an ideal gas?

a)

A) Low temperature and low pressure

b)

B) Low temperature and high pressure

c)

C) High temperature and low pressure

d)

D) High temperature and high pressure

71.

A real gas differs from an ideal gas because the molecules of a real gas have

a)

A) Some volume and no attraction for each other

b)

B) Some volume and some attraction for each other

c)

C) No volume and no attraction for each other

d)

D) No volume and come attraction for each other

72.

One reason that a real gas deviates from an ideal gas is that the molecules of a real gas have

a)

A) a straight-line motion

b)

B) no net loss of energy on collision

c)

C) a negligible volume

d)

D) forces of attraction for each other

73.

According to the kinetic molecular theory, the molecules of an ideal gas

a)

A) have a strong attraction for each other

b)

B) have significant volume

c)

C) move in random, constant, straight-line motion

d)

D) are closely packed in a regular repeating pattern

74.

A sample of chlorine gas is at 300K and 1.00 atmosphere. At which temperature and pressure would the sample behave more like an ideal gas?

a)

A) 0 K and 1.0 atm

b)

B) 150 K and 0.50 atm

c)

C) 273 K and 1.00 atm

d)

D) 600 K and 0.50 atm

75.
Dependent variable means
a)
the scientist controls what to test
b)
educated guess
c)
ask a question
d)
what is being measured
76.

Identify the manipulated variable :

a)

Total weight before the glass rod is broken

b)

Length of copper wire

c)

Type of glass rod

d)

Size of glass rod

77.

Identify the manipulated variable :

a)

Volume of distilled water

b)

Steel nail and iron nail

c)

Type of nail

d)

Resistance towards rusting

78.

Identify the constant variable :

a)

Volume of distilled water

b)

Condition of nail

c)

Type of nail

d)

Size of nail

79.

What is the INDEPENDENT variable (cause)in this experiment?

"Which type of metal, copper or aluminum, conducts heat faster?"

a)

size of metal

b)

types of metal

c)

time it takes to heat up

d)

shape of the metal

80.

Thomas tests different types of liquids to see which will grow his plants the most. He has water, soda, milk, and no liquid at all. What is the control group?

a)

Water

b)

Soda

c)

Milk

d)

No liquid

81.
Measuring the number of times a person breathes after exercise involves ____ data. 
a)
quantitative
b)
qualitative
82.

Copper(II) sulphate solution

a)

Electrolyte

b)

Non-electrolyte

83.

Solid copper(II) chloride

a)

Electrolyte

b)

Non-electrolyte

84.

What state of matter is an electrolyte?

a)

solid

b)

gas

c)

plasma

d)

aqueous

85.

What is required for a liquid to conduct an electric current?

a)

ions that are mobile

b)

ions in a strong bond

c)

covalent bonds

d)

shared protons

86.

Why are all ionic compounds electrolytes?

a)

because they are non-metals

b)

because they share electrons when they bond

c)

because they are electrically neutral

d)

because they dissociate into ions

87.

Why are molecular compounds nonelectrolytes?

a)

they do not have kinetic energy

b)

they do not contain atoms

c)

they do not have chemical bonds

d)

they are not composed of ions

88.
Which solution would be least likely to carry an electric current?
a)
NaCl
b)
HCl
c)
C6H12O6
d)
CsI
89.
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
90.

Which of the following containers most likely contains sugar?


A B

a)

Container A because it forms ions.

b)

Container B because it forms ions.

c)

Container A because it does not form ions.

d)

Container B because it does not form ions.

91.

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

92.

A solution has an [OH] of 1.0x10-8. What is the pOH? Give your answer to 1 significant figure.

(a)  

93.

A solution has a pH of 6.72. What is the pOH? Give your answer to two decimal places

(a)  

94.

What is the concentration of hidroxide ions in a solution with a pH = 7.65?

a)

2.24x10-8

b)

2.5x10-7

c)

4.47x10-7

d)

1.8x10-8

95.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

96.

If a solution has a pH of 1 what is the pOH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

15

e)

neutral

97.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
98.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
99.

If we have a solution of NaCl at of 6.6 mol/L at 60°C, what will happen?

a)

More NaCl can be dissolved.

b)

NaCl will precipitate out.

c)

The solution is saturated.

100.

If we have a solution of NaCl at of 6.5 mol/L at 90°C, what will happen?

a)

More NaCl can be dissolved.

b)

NaCl will precipitate out.

c)

The solution is saturated.

101.

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

102.
When a solution is saturated:
a)
No additional material will dissolve in it
b)
You need to stir it more 
c)
Two materials have combined to create a clear liquid
d)
Crystals form 
103.

What is this image representing?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Insoluble

104.

What is this image representing?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Insoluble

105.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
106.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
107.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
108.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
109.
If 4 grams of HCl are dissolved to make 4,000 grams of solution, how many parts per million of HCl are there? 
a)
100 ppm
b)
999 ppm
c)
1,000,000,000 ppm
d)
1,000 ppm
110.

Molarity is measured in _____.

a)

mol/g

b)

mol/L

c)

mol

d)

mol/mL

111.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
112.

What is the molarity in 650 mL of solution containing 63 grams of sodium chloride (NaCl)?

a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
113.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 grams of water?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

114.
Determine the molarity of 2.25 mole of sulfuric acid, H2SO4, dissolved in 725 mL of solution.
a)
322.2 M
b)
3.1 M
c)
0.32 M
d)
2.25 M
115.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
116.

In general as temperature decreases, the solubility...

a)

increases

b)

decreases

c)

stays the same

117.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
118.

How do you increase the concentration of a solution?

a)

Add more solute

b)

Reduce the amount of solute

c)

Add more solvent

d)

Reduce the amount of solvent

119.

A student prepares a solution by dissolving 60.00 g of glucose (molar mass 180.2 g mol-1) in enough distilled water to make 250.0 mL of solution. The molarity of the solution should be reported as

a)

12.01 M

b)

12.0 M

c)

1.332 M

d)

1.33 M

e)

1.3 M

120.
How many grams of solute are dissolved in 125.0 mL 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
121.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
122.

What mass of NaCl is needed to make 10 mL of 50 mg/mL NaCl solution? *Give final answer!

a)

500 mg NaCl

b)

0.5 g NaCl

c)

500,000 g NaCl

d)

50 mg NaCl

123.

What mass of CaCl2 is needed to make 100 mL of 1.2 g/mL CaCl2 solution? *Give final answer!

a)

0.12 g CaCl2

b)

120 mg CaCl2

c)

0.12 mg CaCl2

d)

120 g CaCl2

e)

120,000 g CaCl2

124.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

125.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

126.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

127.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

128.

To prepare a solution of accurately known volume, use a

a)

measuring cylinder

b)

beaker

c)

concial flask

d)

volumetric flask

129.

To deliver a fixed accurate volume of a solution, use a

a)

pipette

b)

burette

c)

dropper

d)

beaker

130.

What is the reading on this burette?

a)

24.2 mL

b)

24.0 mL

c)

25.8 mL

d)

23.9 mL

131.

25.0 cm3 of sodium hydroxide solution is tritrated against 0.200 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.

Which of the following pieces of apparatus should be used to transfer 25.0 cm3 of the sodium hydroxide solution?

a)

Burette

b)

Measuring cyclinder

c)

Pipette

d)

Volumetric flask

132.

You need to make 200 mL of a 0.20 M aqueous solution of sodium chloride. The only available solution is 1.0 M. Determine how to make the needed dilution.

a)

Add 160 mL to the initial volume

b)

Add 160 grams to the initial volume

c)

Evaporate 160 mL from the initial volume

d)

the experiment cannot be conducted with the materials provided

133.

In an aqueous solution of 0.12M calcium phosphate, what is [Ca2+]?

a)

0.12 M

b)

0.06 M

c)

0.24 M

d)

0.36 M

134.

In the reaction of aqueous MgCl2 and aqueous NaOH, a spectator ion would be:

a)

Na+

b)

OH-

c)

Mg2+

d)

H+

135.

Standard temperature and pressure (STP) mean

a)

A temperature of 0°C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

b)

A temperature of 100°C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

c)

A temperature of 0°K and a pressure of 10 atmosphere (atm).

136.
What is the volume of 0.881 mole of a gas at standard temperature and pressure?
a)
0.0401 L
b)
19.7 L
c)
22.4 L
d)
39.4 L
137.

What is the molar mass of C2H4O2?

a)

40 g/mol

b)

50 g/mol

c)

60 g/mol

d)

68 g/mol

138.
What is the volume of 2 moles of gas at STP?
a)
22.4 L
b)
44.8 L
c)
11.2 L
d)
2 L
139.

At STP, 1 mol, or representative particles, of any gas occupies a volume of......................

a)

24.4 L

b)

44.2 L

c)

22.4 L.

140.

Tastes bitter

a)

acid

b)

base

c)

both an acid and a base

141.

Which is the correct set of acid properties:

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

142.

Reacts with metals

a)

acid

b)

base

c)

both acid and base

143.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

144.

Your teacher tells you that a substance is acidic. This means the pH will be...

a)

More than 7

b)

7 exactly

c)

Less than 7

d)

Higher than 14

145.

Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.

The substance in the beaker

a)

is a base

b)

is an acid

c)

have neutral pH

d)

doesn't have pH

146.
The Acid-Base classification system that defined acids as those that release H+ and bases as release OH- is known as ________.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
147.

An acid that has more than one ionizable hydrogen is a ____.

a)

binary acid

b)

polyprotic acid

c)

strong acid

d)

weak acid

148.

Which of the following is a polyprotic acid?

a)

HCl

b)

HF

c)

HBr

d)

H2SO4

149.

HCl is a strong acid because ____.

a)

it ionizes completely into H+ and Cl- ions

b)

it is very concentrated

c)

it ionizes incompletely into H+ and Cl- ions and some stays as HCl

d)

it will react with bases

150.

Household vinegar has a pH of approximately 3.0. Which would appear yellow when added to a vinegar solution?

a)

Methyl orange

b)

Bromcresol green

c)

Phenophthalein

d)

Litmus

151.

Phenolphthalein has a pink color in a solution that has a pH of

a)

5

b)

11

c)

1

d)

7

152.

Which indicators would cause a solution with a pH of 2 to turn red?

a)

Bromthymol blue and thymol blue

b)

Bromcresol green and litmus

c)

Litmus and methyl orange

d)

Methyl orange and phenolphthalein

153.

An indicator was used to test a water solution with a pH of 3. Which indicator color would be observed?

a)

Yellow with methyl orange

b)

Pink with phenolphthalein

c)

Blue with litmus

d)

Yellow with bromcresol green

154.

At what pH will bromthymol blue, thymol blue, and bromcresol all be yellow?

a)

4

b)

2

c)

7

d)

5

155.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
NaCl
a)
NaCl  --> Na+ + Cl-
b)
NaCl(s)  --> Na+(aq) + Cl-(aq)
c)
NaCl  --> Na + Cl
d)
NaCl(s) --> Na(aq) + Cl(aq)
156.
Write dissociation equations for the following electrolytes. Show physical states of all species involved!
Ca(NO3)2
a)
Ca(NO3)2(s) -->Ca+(aq) + 2NO3- (aq) 
b)
Ca(NO3)2(s) -->Ca2+(aq) + 2NO3- (aq) 
c)
Ca(NO3)2(s) -->Ca2+(aq) + NO3- (aq) 
d)
Ca(NO3)2 -->Ca+ + 2NO3- 
157.
what is the net ionic equation for the reaction 
2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s)
a)
2OH–(aq) + Cu2+(aq)  →  Cu(OH)2(s)
b)
2OH–(aq) + Na+(aq) → NaOH(s)
c)
2Cl–(aq) + Cu2+(aq) → CuCl2(s)
d)
Cl–(aq) + Na+(aq) → NaCl(s)
158.
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
159.

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

a)

ionization

b)

dissociation

c)

electronegativity

d)

spectation

160.
What is the coefficient of AgNO3 in this reaction?
_AgNO3 + _H2S →_Ag2S+_HNO3
a)
1
b)
2
c)
3
d)
4
161.

Balance this equation, AlCl3 + NaOH → Al(OH)3 + NaCl

a)

3,1,3,1

b)

1,3,3,1

c)

1,1,1,3

d)

1,3,1,3

162.
Given the equation representing a system at equilibrium:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Which statement describes this system? 
a)
The concentration of PCl5(g) is increasing. 
b)
The concentration of PCl5(g) is decreasing. 
c)
The concentrations of PCl5(g) and PCl3(g) are equal. 
d)
The concentrations of PCl5(g) and PCl3(g) are constant. 

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