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Chemistry Final Review

Total questions: 160

Worksheet time: 9hrs 4mins

Name
Class
Date
1.
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
2.
2NaClO3 (s) → 2NaCl (s) + 3O2 (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
3.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
4.
Fe2O3 + 3H2 → 2Fe + 3H2O
About how many grams of H2O will be produced from 150 grams of Fe2O3? 
a)
50 grams H2O
b)
60 grams H2O
c)
5000 grams H2O
d)
6000 grams H2O
5.
Given the following reaction, 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
6.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
7.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
8.
Use the following equation:
2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide?
a)
150.22 g Na2SO4
b)
593.44 g Na2SO4
c)
330.04 g Na2SO4
d)
297.65 g Na2SO4
9.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
10.

151 grams of Al2O3 are produced. How many grams of Al was needed in the reaction? Al + O2 -------> Al2O3 balance first.

a)

79.91 g

b)

22.4 liters

c)

57.8 g

d)

142.8 g

11.

What is the mole-to-mole ratio for hydrogen and oxygen in the balanced equation: 2 H2 + O2 -> 2 H2O?

a)

1:2

b)

1:1

c)

3:1

d)

2:1

12.

How many moles of H2O are produced when 4 moles of O2 react? 2 H2 + O2 -> 2 H2O

a)

8 mol

b)

2 mol

c)

6 mol

d)

10 mol

13.

What is the mass of NaCl produced when 2.2 moles of Na react with excess Cl2?

2 Na + Cl2 →\rightarrow 2 NaCl

molar mass of NaCl = 58.44 g/mol

a)

128.57 g

b)

58.65 g

c)

117.3 g

d)

234.6 g

14.

How many moles of CO2 are produced when 5.6 grams of C6H12O6 react?

C6H12O6 + 6 O2 →\rightarrow 6 CO2 + 6 H2O

Molar mass C6H12O6 = 180.18 g/mol

a)

2.5 mol

b)

1.5 mol

c)

0.186 mol

d)

0.5 mol

15.

What is the Law of Conservation of Mass?

a)

It states that matter cannot be created or destroyed.

b)

It states that energy cannot be created or destroyed.

c)

It states that matter can be created or destroyed.

d)

It states that sound can be created or destroyed.

16.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number in front of a chemical formula.
c)
The number in between the chemical symbols.
d)
The number behind a chemical formula.
17.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
18.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
19.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
20.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
21.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
22.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
23.
Is the following equation balanced?
4Fe + 3O2 --> 2Fe2O3
a)
yes
b)
no
24.
Is the following reaction balanced?
NaHCO3 --> Na2CO3 + H2O + CO2
a)
yes
b)
no
25.
Is the following reaction balanced?
2CH3OH + 3O2 --> 2CO2 + 4H2O
a)
yes
b)
no
26.

The coefficient in 3H2O is

a)

6

b)

5

c)

2

d)

3

27.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
28.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
29.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
30.

What are the coefficients that would properly balance this equation?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)

2,1 --> 2,1

b)

1,2 --> 1,1

c)

1,2 --> 2,4

d)

1,2 --> 2,1

31.

What are the coefficients that would properly balance this equation?

__H2 + __S --> __H2S

a)

1,1 --> 1

b)

2,2 --> 2

c)

1,2 --> 1

d)

1,2 --> 2

32.
What is the total number of atoms present in 5Na3PO4
a)
5
b)
40
c)
55
d)
8
33.

Balance the the following equation.

__Zn+__HCl -->__ZnCl2 +__H2

a)

1,1,2,1

b)

1,1,1,2

c)

1,2,1,1

d)

2,1,1,1

34.
Which number should go in the blank?
Mn + _ HNO3 → Mn(NO3)2 + H2
a)
1
b)
2
c)
3
d)
0
35.

What creates pressure?

a)

gas molecules spinning

b)

gas molecules colliding with container walls

c)

potential energy

d)

electrons

36.

What is the mathematical expression for Boyle's Law?

a)

P1V1=P2V2P_1V_1=P_2V_2  

b)

P1V1=P2V2\frac{P_1}{V_1}=\frac{P_2}{V_2}  

c)

V2P2=V1P1\frac{V_2}{P_2}=\frac{V_1}{P_1}  

d)

P1V2=P2V1P_1V_2=P_2V_1  

37.

When using Charles' Law if you double volume, what happens to temperature?

a)

it remains constant

b)

it triples

c)

it is divided by 2

d)

it is doubled also

38.

What temperature scale must we use in the Gas Laws?

a)

Rankine

b)

Fahrenheit

c)

Kelvin

d)

Celsius

39.

How many kpa are in 1.01 bar?

a)

760

b)

101.3

c)

14.7

d)

1

40.

How do we measure an increase in kinetic energy?

a)

volume

b)

temperature

c)

Liters

d)

none of the above

41.

What happens to pressure as we in crease kinetic energy?

a)

it decreases

b)

it remains constant

c)

it increases

d)

none of the above

42.

If you place a balloon in a refrigerator what will happen to the volume?

a)

it will decrease

b)

it will increase

c)

it will remain constant

d)

none of the above

43.

Why does the volume decrease in the previous question?

a)

because the molecules slow down their spinning

b)

because temperature and pressure decrease with a decrease in kinetic energy and collisions

c)

because of a decrease in potential energy

d)

none of the above

44.

What gas law should you use to describe the balloon in the last two questions

a)

Charles' Law

b)

Boyles Law

c)

Dalton's Law

d)

Combined Gas Law

45.

How many (partial pressures) gasses can we have in Dalton's Law?

a)

5

b)

10

c)

100

d)

an infinite number of (partial pressures) gases

46.

What happens to pressure at higher elevations?

a)

it increases

b)

it decreases

47.

Why does the pressure decrease as we reach higher elevations?

a)

the air molecules have more kinetic energy

b)

there are less air molecules

c)

the air molecules have less kinetic energy

d)

there are more air molecules

48.

In the picture when the pistons rise the volume of the cylinder decreases. What happens to the pressure and temperature?

a)

The temperature will decrease and, therefore, the pressure will decrease.

b)

The collisions between molecules and the container walls will increase causing an increase in pressure. The temperature will decrease because the kinetic energy decreases.

c)

The collisions between molecules and the container walls will increase causing an increase in pressure. The temperature will because the kinetic energy will increase.

d)

The temperature and pressure are not related.

49.

What causes a hot air balloon to rise?

a)

An increase in temperature causes an increase in pressure that causes an increase in volume which causes the air in the balloon to be more dense than the air around it.

b)

An increase in temperature causes an increase in pressure that causes an increase in volume which causes the air in the balloon to be less dense than the air around it.

c)

As the temperature of the gas increases it escapes the balloon similarly to the gas leaving a rocket. This forces the balloon into the air.

d)

The increase in kinetic energy due to a temperature increase causes the atoms to lose protons and become helium. Helium is lighter than the air surrounding the balloon and this causes it to rise.

50.

A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atmosphere. When the volume increases to 4.0 liters at constant temperature, what will be the resulting pressure of the sample?

a)

0.25 atm

b)

0.50 atm

c)

1.0 atm

d)

2.0 atm

51.

A rigid cylinder contains a sample of gas at STP. What is the pressure of this gas after the sample is heated to 410 K?

a)

0.50 atm

b)

0.67 atm

c)

1.0 atm

d)

1.5 atm

52.

Every time matter changes from a liquid to a gas, the matter also experiences a change in the

a)

molecular motion

b)

total molecular mass

c)

size of the molecules

d)

total number of molecules

53.

The Kinetic Molecular Theory of Matter states that the higher the temperature, the faster the ____.

a)

Particles that make up a substance move.

b)

Bonds between atoms break down.

c)

Molecules of gas rush together.

d)

Lighter molecules within a substance clump together.

54.

As the temperature of a fixed volume of a gas increases, the pressure will ____.

a)

varies inversely

b)

decrease

c)

not change

d)

increase

55.

At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?

a)

447 K

b)

50.3 K

c)

412 K

d)

36.7 K

56.

Find the final temperature of a sample of nitrogen gas at constant pressure if it starts at 27 °C and changes volume from 600 mL to 700 mL.

a)

350 K

b)

257 K

c)

315 K

d)

1400 K

57.

Which postulate of KMT explains why the scent of fresh coffee in the morning fills up every room in the house?

a)

All particles are infinitely small and the size of a particle is negligible compared to the container that it holds.

b)

The particles of gas are in constant motion and move in straight lines.

c)

The particles of gas do not exert any force of attraction or repulsion on each other. There is no energy loss during a collision.

d)

The mean kinetic energy of the particles is directly proportional to their absolute temperature.

58.

A sample of a pure substance in the form of a liquid is heated until it changes into a gas. Which of the following statements best describes the difference between the molecules of the pure sample in the liquid state and the molecules of the pure sample in the gas state?

a)

The molecules in the gas state will have more kinetic energy and be closer together than the molecules in the liquid state.

b)

The molecules in the gas state will have more kinetic energy and be farther apart than the molecules in the liquid state.

c)

The molecules in the gas state will have less kinetic energy and be closer together than the molecules in the liquid state.

d)

The molecules in the gas state will have less kinetic energy and be farther apart than the molecules in the liquid state.

59.

What is the molar volume of any gas at STP?

a)

22.4 L

b)

2.24 L

c)

224 L

d)

6.02 x 10^23 L

60.

According to the KMT, increasing the temperature of particles will

a)

give off energy

b)

increase motion

c)

decrease volume

d)

increase pressure

61.

According to the KMT, the particles of the different states of matter differ in what two key aspects?

a)

volume and mass

b)

density and extention of interactions

c)

temperature and freedom of motion

d)

freedom of motion and extent of interactions

62.

How doe the particles in a gas behave?

a)

Neatly organized without any movement.

b)

Move around trapped in a small volume and with the same surrounding particles.

c)

Move fast enough to break attractions and pushing other particles out of the way.

d)

Move freely in a straight line until they collide with another particle.

63.

In which state of matter are the particles the farthest apart?

a)

gas

b)

liquid

c)

solid

64.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

65.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

66.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
67.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
68.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
69.
According to Boyle's law of PV, at constant temperature, as the pressure of a given sample of gas is increased, the volume will –
a)
Increase
b)
Decrease
c)
Remains the same
70.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
71.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
72.
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)
73.
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) →
74.
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
75.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
76.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
77.
Which of these results in formation of a precipitate?
a)
BaNO3(aq)  +  NaCl(aq)→
b)
KNO3(aq)  +  LiOH(aq)→
c)
Zn(NO3)2(aq)  +  NaOH(aq)→
d)
NaNO3(aq)  +  Ba(OH)2(aq)→
78.
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-
79.
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
80.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
81.
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)
82.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl1- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl1- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
83.

Which of the following reactions does NOT have a net ionic equation?

a)

C9H20 + O2 --> CO2 + H2O

b)

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

c)

NH4I + PbOH --> NH4OH + PbI2

d)

Fe(NO3)2 + KOH --> KNO3 + FeOH

84.

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

85.

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

86.

What is the precipitate in the net ionic equation of CuClO4 + ZnI2

a)

CuI

b)

Zn(ClO4)2

c)

ZnClO4

d)

CuI2

87.

In this equation,

CuCl2+ NaOH → Cu(OH)2 + NaCl

Which product is insoluble?

a)

copper(II) hydroxide

b)

sodium chloride

c)

sodium hydroxide

d)

copper(I) hydroxide

88.
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
89.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
90.

What do we call the substance that is being dissolved?

a)

Solute

b)

Solvent

c)

Concentration

d)

Electrolyte

91.

What do we call the substance that is doing the dissolving?

a)

Solute

b)

Solvent

c)

Concentration

d)

Electrolyte

92.

Kool aid is the perfect refreshment on a hot summer day. What is the solvent in this delicious mixture?

a)

Kool aid

b)

Water

93.

Kool aid is the perfect refreshment on a hot summer day. What is the solute in this delicious mixture?

a)

Kool aid

b)

Water

94.

What is the universal solvent?

a)

Water

b)

Milk

c)

Salt

d)

Sugar

95.

What can be found on the y-axis of this solubility graph?

a)

grams of solute

b)

Temperature

c)

moles of solute

d)

mL of solute

96.

What can be found on the x-axis of this solubility graph?

a)

grams of solute

b)

Temperature

c)

moles of solute

d)

mL of solute

97.

Which of the following can increase the solubility of a solution?

a)

Stirring

b)

Decreasing temperature

c)

Adding more solute

d)

Evaporation

98.

If 60 g of KCl were placed in 100 g of water at 60° C, what kind of solution would be formed?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

99.

If 30 g of K2Cr2O7  were placed in 100 g of water at 50° C, what kind of solution would be formed?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

100.

If 20 g of KClO3  were placed in 100 g of water at 80° C, what kind of solution would be formed?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

101.

At what temperature do NaCl and KCl have the same solubility?

a)

10°C10\degree C  

b)

30°C30\degree C  

c)

50°C50\degree C  

d)

70°C70\degree C  

102.

A solution that contains more of the dissolved material than could be dissolved under normal circumstances.

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

103.

The amount of solute added is below what the substance can dissolve.

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

104.

Which statement is true of the three solutions?

a)

Solution C is more soluble in water when compared to Solution A.

b)

Solution C is less soluble in water when compared to Solution B.

c)

Solution C is the least soluble in water when compared to Solutions A and B.

d)

Solution B is the least soluble in water when compared to Solutions A and C.

105.

If 20 g of KNO3 were placed in 100 g of water at 10° C, what kind of solution would be formed?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

106.

If 60 g of Pb(NO3)2 were placed in 100 g of water at 60° C, what kind of solution would be formed?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

107.

Hot chocolate is a great treat on a cold and dreary day. What is the solvent in this delicious mixture?

a)

Hot Cocoa Mix

b)

Milk

108.

Hot chocolate is a great treat on a cold and dreary day. What is the solute in this delicious mixture?

a)

Hot Cocoa Mix

b)

Milk

109.

A solute is added to water and a portion of the solute remains undissolved. When equilibrium between the dissolved and undissolved solute is reached, what type of solution is present?

a)

Saturated

b)

Supersaturated

c)

Unsaturated

d)

Nonsaturated

110.

What is the main purpose of acid-base titrations?

a)

To test if reactants react.

b)

To calculate the concentration of unknown analyte.

c)

To calculate the concentration of known analyte.

d)

To test quality of reactants.

111.

What is the role of an indicator in a reaction?

a)

To help reactants react successfully.

b)

To bind to the analyte to form a products.

c)

To show when the reaction has reached or past the equivalence point.

d)

To provide a surface for the reaction to occur.

112.

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.

113.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
114.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
115.

Ascorbic acid, H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10–5 and K2 = 1.6 × 10–12. In a 0.005 M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration?

a)

H3O+(aq)

b)

H2C6H6O6(aq)

c)

HC6H6O6-(aq)

d)

C6H6O62-(aq)

116.

In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment?

a)

The [H+] at the equivalence point equals the ionization constant of the acid.

b)

The pH at the equivalence point depends on the indicator used.

c)

The graph of pH versus volume of base added rises gradually at first and then much more rapidly.

d)

The graph of pH versus volume of base added shows no sharp rise.

117.

Which of the following best approximates the Ka value for this weak acid?

a)

1 x 10–4

b)

1 x 10–5

c)

5x 10–6

d)

5 x 10–7

118.

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

119.

At point P in the titration, which of the following species has the highest concentration?

a)

HA

b)

A–

c)

H3O+

d)

OH–

120.

Which of the following best represents a 0.100-molar solution of H2SO4 in water?

a)
b)
c)
d)
121.

Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest?

a)

Beaker 1

b)

Beaker 2

c)

Beaker 3

d)

Beaker 4

122.

Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion in solution in largest concentration, other than the K+ ion, is

a)

H2PO4 –

b)

HPO4 2–

c)

PO4 3–

d)

OH-

123.

What part of the curve corresponds to the optimum buffer action for the acetic acid/acetate ion pair?

a)

Point V

b)

Point Z

c)

Along all of section WY

d)

Along all of section YZ

124.

Which of the following indicators is the best choice for this titration?

a)

Methyl orange (pH range of color change is 3.2 - 4.4)

b)

Methyl red (pH range of color change is 4.8 - 6.0)

c)

Bromothymol blue (pH range of color change is 6.1 - 7.6)

d)

Phenolphthalein (pH range of color change is 8.2 - 10.0)

125.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
126.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

vinegar

b)

milk

c)

water

d)

bleach

127.

Zn(OH)2 is an example of a...

a)

acid

b)

base

c)

salt

d)

water

128.

H3PO4 is an example of a ...

a)

acid

b)

base

c)

salt

d)

non-electrolyte

129.

Four substances were tested for pH, lemon juice (pH 2), baking soda (pH 9), bleach (pH 12), and milk (pH 6). Which of the following correctly lists the substances from most basic to acidic?

a)

lemon juice, milk, baking soda, bleach

b)

bleach, baking soda, milk, lemon juice

c)

milk, lemon juice, baking soda, bleach

d)

baking soda, bleach, lemon juice, milk

130.

At what pH would all three indicators appear as yellow?

a)

1.7

b)

2.7

c)

4.7

d)

8.7

131.

Phenolphthalein is pink in an aqueous solution having a pH of

a)

2

b)

7

c)

5

d)

12

132.

Based on the results of testing colorless solutions with indicators, which solution is MOST acidic?

a)

a solution in which bromthymol blue is blue

b)

a solution in which bromcresol green is blue

c)

a solution in which phenolphthalein is pink

d)

a solution in which methyl orange is red

133.

If a solution has a pH of 1.5, then litmus would turn

a)

red

b)

purple

c)

blue

d)

yellow

134.

If a solution has a pH of 10, then methyl orange would turn

a)

red

b)

yellow

c)

orange

d)

blue

135.

According to the diagram, what is the color of bromcresol green at the pH of the mouth?

a)

Yellow

b)

Blue

c)

Green

d)

Red

136.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
137.

According to the diagram, which part of the digestive system has the most basic enviroment?

a)

Mouth

b)

Stomach

c)

Pancreas

d)

Small intestine

138.

Which pair of compounds represents one Arrhenius acid and one Arrhenius base?

a)

CH3OH and NaOH

b)

CH3OH and HCl

c)

HNO3 and NaOH

d)

HNO3 and HCl

139.

A solution with a pH of 7.8 is first tested with bromthymol blue and then with phenolphthalein. What is the color

of each indicator in this solution?

a)

Bromthymol blue is yellow and phenolphthalein is colorless.

b)

Bromthymol blue is blue and phenolphthalein is colorless.

c)

Bromthymol blue is yellow and phenolphthalein is pink.

d)

Bromthymol blue is blue and phenolphthalein is pink.

140.

The compound KOH can be described as an

a)

Arrhenius acid and an electrolyte

b)

Arrhenius base and an electrolyte

c)

Arrhenius acid and a nonelectrolyte

d)

Arrhenius base and a nonelectrolyte

141.

What is the color of the indicator thymol blue after it is added to an aqueous solution of vitamin C, also known ascorbic acid?

a)

Yellow

b)

Blue

c)

Red

d)

Pink

142.

Which indicator, when added to a solution, changes color from yellow to blue as the pH of the

solution is changed from 5.5 to 8.0?

a)

bromcresol green

b)

bromthymol blue

c)

litmus

d)

methyl orange

143.

According to the diagram, which indicator would turn yellow at the pH of the pancreas?

a)

methyl orange

b)

bromthymol blue

c)

bromcresol green

d)

litmus

144.

Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an

Arrhenius base in an aqueous solution?

a)

HBr

b)

KBr

c)

H2O

d)

KOH

145.

What type of reaction is Fe + Cl2 → FeCl3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

146.

What type of reaction is C2H2 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

147.

What type of reaction is BF3 + Li2SO3 → B2(SO3)3 + LiF

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

148.

What type of reaction is Ag2O → Ag + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

149.

What type of reaction is C5H10 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

150.

What type of reaction is Zn + HCl → H2 + ZnCl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

151.

What type of reaction is H2 + N2 → NH3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

152.

What type of reaction is (NH2)3PO4 + Pb(NO3)4 → NH4NO3 + Pb3(PO4)4

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

153.

What type of reaction is FeBr3 + H2SO4 → HBr + Fe2(SO4)3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

154.

What type of reaction is Fe + H2SO4 → H2 + FeSO4

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

155.

What type of reaction is Mg + Br2 → MgBr2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

156.

What type of reaction is KClO3 → KCl + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

157.

What type of reaction is K2CO3 → K2O + CO2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

158.

What type of reaction is CH4 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

159.

What type of reaction is NaOH + HCl → H2O + NaCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

160.

What type of reaction is SeCl6 + O2 → SeO2 + Cl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

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