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Chemistry II Unit 7 Review

Total questions: 111

Worksheet time: 6hrs 5mins

Name
Class
Date
1.

What is the definition of solubility?

a)
The ability of a substance to dissolve in another substance
b)
The ability of a substance to react with another substance
c)
The ability of a substance to change its state from solid to liquid
d)
The ability of a substance to change its color when heated
2.

What is a solute?

a)

A type of musical instrument

b)

A substance that is dissolved in a solution

c)
A mathematical solution
d)
A type of physical exercise
3.

What is a solvent?

a)

A substance that reacts with a solute

b)
A substance that cannot be dissolved
c)

A substance that it dissolves in usually water

d)
A substance that is insoluble in water
4.

If something is soluble in another substance it (a)   .

5.

If something is NOT soluble in a substance it does NOT (a)   .

6.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
7.

25 grams of NaCl are dissolved in 100 mL of water at 60 oC. How many more grams need to be dissolved for the solution to be saturated?

a)

13 grams

b)

25 grams

c)

6 grams

d)

38 grams

8.

How many grams of K2Cr2O7, are soluble in 100 g of water at 90 ºC?

a)

85 grams

b)

70 grams

c)

40 grams

d)

15 grams

9.

How many grams of K2Cr2O7, are soluble in 50 g of water at 90ºC?

a)

70 grams

b)

35 grams

c)

140 grams

d)

105 grams

10.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
11.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
12.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
13.
When 42 grams of potassium chloride, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
14.

How many grams of KClO3, are soluble in 200g of water at 30ºC?

a)

5 grams

b)

100 grams

c)

10 grams

d)

20 grams

15.

How much KNO3 solute is present in a saturated solution at 40 oC in 100 g of H2O?

a)

75

b)

55

c)

63

d)

85

16.

How much Ce2(SO4)3 solute is saturated at 40 oC in 100 g of H2O?

a)

240 g

b)

220 g

c)

230 g

d)

250 g

e)

3 g

17.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

18.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

19.
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 
20.
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)
21.
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) →
22.
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
23.
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
24.
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
25.
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)→
26.
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-
27.
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
28.
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)
29.

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

30.

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

31.

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

a)

CuI

b)

Zn(ClO4)2

c)

ZnClO4

d)

CuI2

32.

The concentration of OH– in a saturated solution of Mg(OH)2 is 3.6 x 10–4 M. The Ksp of Mg(OH)2 is

a)

1.3 x 10–7

b)

4.7 x 10–11

c)

3.6 x 10–4

d)

2.3 x 10–11

33.

The correct mathematical expression for finding the molar solubility (X) of Sn(OH)2 is:

a)

2(X)3 = Ksp

b)

108(X)5 = Ksp

c)

4(X)3 = Ksp

d)

8(X)3 = Ksp

34.

Barium carbonate has a measured solubility of 4.0 x 10–5 at 25°C. Determine the Ksp.

a)

5.3 x 10–10

b)

6.1 x 10–5

c)

9.1 x 10–7

d)

1.6 x 10–9

35.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 x 10-7, 1,6 x 10-10, and 2.0 x 10-13, respectively. Which compound will precipitate first?

a)

CuCl(s)

b)

AgCl(s)

c)

AuCl(s)

d)

All will precipitate at the same time.

36.

Calculate the solubility of Ca3(PO4)2(s) (Ksp = 1.3 x 10–32) in a 1.0 x 10–2 M Ca(NO3)2 solution.

a)

5.7 x 10–14 mol/L

b)

6.2 x 10–7 mol/L

c)

1.6 x 10–14 mol/L

d)

3.16 x 10–12 mol/L

37.

The [IO3–] in a saturated solution of Ce(IO3)3 is 5.55 x 10–3 M. Calculate the Ksp for Ce(IO3)3.

a)

3.16 x 10–10

b)

1.03 x 10–5

c)

2.56 x 10–8

d)

3.51 x 10–11

38.

What is the Ksp for silver phosphate (Ag3PO4) at 25°C? The solubility of silver phosphate at 25°C is 1.6 x 10–5 mol/L.

a)

7.7 x 10–10

b)

1.8 x 10–18

c)

8.6 x 10–13

d)

3.3 x 10–13

39.

In a solution prepared by adding excess PbI2(s) [Ksp = 1.4 x 10–8] to water, the [I–] at equilibrium is:

a)

1.5 x 10–3 mol/L

b)

2.4 x 10–3 mol/L

c)

1.2 x 10–3 mol/L

d)

3.0 x 10–3 mol/L

40.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
41.

In a redox reaction, the species that is reduced will ___ electrons, becoming more _____ charged.

a)

lose; negatively

b)

lose; positively

c)

gain; positively

d)

gain; negatively

42.

A precipitation reaction must...

a)

Have a solid ionic product from aqueous reactants

b)

Have only gaseous products from gaseous reactants

c)

Have only aqueous products from aqueous reactants

43.

Which of the following represents the net ionic equation for the precipitation reaction between sodium carbonate and magnesium sulfate?

a)

Na2CO3 + MgSO4 --> MgCO3 + Na2SO4

b)

2Na+ + CO3-2 + Mg+2 + SO4-2 --> Mg+2 + CO3-2 + 2Na+ + SO4-2

c)

2Na+ + SO4-2 --> Na2SO4

d)

CO3-2 + Mg+2 --> MgCO3

44.

What is the oxidation number of N in NO21-?

a)

0

b)

-1

c)

2

d)

3

45.

The ______ the acid, the ______ its conjugate base.

a)

stronger, weaker

b)

stronger, stronger

46.

Spectator ions _____________________________.

a)

undergo chemical change during a chemical reaction.

b)

do not undergo chemical change during a chemical reaction.

c)

wear spectacles during a chemical reaction.

47.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
48.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

49.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
50.
What element is being Reduced?
a)
N
b)
H
c)
O
d)
S
51.
What are the coefficients when the equation is balanced?
a)
2 + 3 --> 2 + 3 + 4
b)
1 + 3 --> 1 + 3 + 2
c)
2 + 4 --> 2 + 3 + 2
d)
1 + 1 --> 1 + 1 + 1
52.
What element is being Oxidized?
a)
I
b)
H
c)
S
d)
O
53.
What are the coefficients when the equation is balanced?
a)
1 + 1 + 1 --> 2 + 1 + 3
b)
2 + 2 + 2 --> 4 + 2 + 3
c)
1 + 2 + 1 --> 2 + 2 + 3
d)
1 + 1 + 1 --> 1 + 1 + 1
54.
What element is being reduced?
a)
I
b)
H
H
c)
S
S
d)
O
O
55.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
56.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
57.
What is oxidation number of H in CaH2?
a)
+1
b)
-1
c)
0
d)
+2
58.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
59.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
60.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
61.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
62.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
63.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
64.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
65.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
66.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
67.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
68.
Oxygen always has an oxidation number of...
a)
-1
b)
1
c)
2
d)
-2
69.

Which of the following statements applies to the change in mass of the electrodes involved in this electrochemical cell?

a)

Electrode A is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

b)

Electrode B is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

c)

Electrode A is the cathode and it gains mass since metal ions are being converted to metal atoms which often adhere to the electrode.

d)

Electrode B is the cathode and it gains mass since metal ions are

being converted to metal atoms which often adhere to the electrode.

70.

Which statement best describes how a salt bridge maintains electrical neutrality in the half-cells of an electrochemical cell?

a)

It prevents the migration of electrons.

b)

It prevents the reaction from occurring spontaneously.

c)

It permits the migration of ions.

d)

It allows for the reaction from occurring spontaneously.

71.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
72.
Which change does nitrogen undergo oxidation?
a)
A
b)
B
c)
C
d)
D
73.
Which are examples of reduction?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
74.

What is oxidation number of Cr in Cr2O72-?

a)

-2

b)

+2

c)

+6

d)

+12

75.

When water is electrolyzed, gas collected at cathode, is

a)

sulphur

b)

oxygen

c)

hydrogen

d)

sulphur dioxide

76.

Galvanic cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

77.

In the following reaction


Sn+2 + 2Fe+3 → Sn+4 + 2Fe+2


the oxidizing agent is....

a)

Sn+4

b)

Sn+2

c)

Fe+3

d)

Fe+2

78.

In the following reaction

Sn+2 + 2Fe+3 --> Sn+4 + 2Fe+2,

the reducing agent is...

a)

Fe+3

b)

Sn+2

c)

Sn+4

d)

Fe+2

79.

An oxidizing agent will

a)

increase in mass

b)

lose electrons

c)

be reduced

d)

increase in oxidation number

80.

What occurs to the mass of copper electrode in the following reaction?

Zn/Zn2+ // Cu2+/Cu

a)

increases

b)

decreases

c)

remains the same

81.

Electrons always flow from

a)

cathode to anode

b)

anode to cathode

82.

In a Galvanic Cell, the anode is...

a)

positive

b)

negative

83.

In a Galvanic Cell, the cathode is...

a)

positive

b)

negative

84.

Oxidation occurs at the...

a)

anode

b)

cathode

85.

Reduction occurs at the...

a)

anode

b)

cathode

86.

In a redox reaction, the oxidising agent... (choose two options)

a)

is oxidised

b)

is reduced

c)

increases its oxidation number

d)

decreases its oxidation number

87.

In a redox reaction, the reducing agent... (choose two options)

a)

is oxidised

b)

is reduced

c)

increases its oxidation number

d)

decreases its oxidation number

88.

In a Galvanic cell, the cations in the salt bridge...

a)

flow the same way as the electrons flow in the wire

b)

flow the opposite way to the electron flow in the wire

c)

stay in the salt bridge

89.

In a Galvanic Cell, the salt bridge...

a)

completes the circuit so that electrons can flow through the wire

b)

maintains charge balance

c)

is soaked in an unreactive electrolyte such as KNO3

d)

all of the above

90.
What occurs during electrolysis of a molten salt?
a)
Electricity is produced by a spontaneous redox reaction
b)
Electricity cause a non-spontaneous redox reaction to occur
c)
Electrons flow through the molten salt
d)
Electrons are removed from both ions of the molten salt
91.

What is the name of the negative electrode in an electrolytic cell ?

a)

cathode

b)

anode

92.

What is the name of the positive electrode in an electrolytic cell?

a)

cathode

b)

anode

93.
Anion loses electrons at the
a)
cathode
b)
anode
94.
Reduction occurs at the 
a)
anode
b)
cathode
95.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
96.

According to Brønsted-Lowry acid base theory, an acid ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces H+ when added to water

d)

turns phenolphthalein pink

97.

According to Arrhenius acid-base theory, an acid ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

98.

Which reactant in the following equation is acting as a Brønsted-Lowry acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

99.

CO32-(aq) + H2O(l) → HCO3-(aq) + OH-(aq)

Using the above reaction, which species is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

100.

A substance that remains when a base has accepted an H+ ion is a(n)


(a)  
Choose from the below words
conjugate acid
acid
base
conjugate base
101.

True or False: All Arrhenius acids are also Brønsted-Lowry acids.

a)

True

b)

False

102.

According to Arrhenius acid-base theory, a base ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces OH- in water

d)

turns litmus paper red

103.

Match the following

a)

higher than 7

1.

base

b)

lower than 7

2.

acid

c)

7

3.

neutral

104.

What does pH measure?

a)

strength of an acid

b)

strength of a base

c)

strength of both acids and bases

d)

concentration of H+ ions

105.

What is the name of this ion: H3O+?

a)

Helium ion.

b)

Hydrogen ion.

c)

Hepatic ion.

d)

Hydronium ion.

106.

Choose the conjugate acid of OH-

a)

HCO3-

b)

OH-

c)

CO32-

d)

H2O

107.

Choose the conjugate base of HNO3

a)

HNO3

b)

H2O

c)

H3O+

d)

NO3-

108.

According to Brønsted-Lowry acid base theory, an acid ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces H+ when added to water

d)

turns phenolphthalein pink

109.

According to Arrhenius acid-base theory, an acid ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

110.

According to Arrhenius acid-base theory, a base ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces OH- in water

d)

turns litmus paper red

111.

According to Brønsted-Lowry acid base theory, a base ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces OH- when added to water

d)

has a bitter taste

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