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AP Chem Unit 4 Review

Total questions: 77

Worksheet time: 2hrs 54mins

Name
Class
Date
1.

A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms.

Which of the following is the balanced net ionic equation for the formation of the precipitate?

a)

Ag+(aq)+Cl−(aq)→AgCl(s)

b)

Na+(aq)+NO3−(aq)→NaNO3(s)

c)

NaCl(aq)+AgNO3(aq)→NaNO3(s)+AgCl(aq)

d)

NaCl(aq)+AgNO3(aq)→NaNO3(aq)+AgCl(s)

2.

A chemistry teacher carried out several demonstrations, and students recorded their observations. For one of the demonstrations, a student concluded that a physical change took place, but not a chemical change. Which of the following observations could the student have made of the results of the demonstration?

a)

Two colorless solutions were combined, and the resulting solution was pink.

b)

When a solid was added to a liquid, sparks were produced.

c)

One piece of solid substance was changed into small pieces.

d)

When two solutions were combined, a precipitate formed.

3.

Which of the following is the correct net ionic equation of the reaction that occurs when aqueous solutions of ammonia and hydrochloric acid are combined?

a)

NH3(aq)+HCl(aq)→NH4Cl(aq)

b)

NH3(aq)+H+(aq)→NH4+(aq)

c)

NH3(aq)+HCl(aq)→NH4+(aq)+Cl−(aq)

d)

NH3(aq)+H+(aq)+Cl−(aq)→NH4+(aq)+Cl−(aq)

4.

Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)

When the reaction represented above proceeds, heat is produced. Which of the following best describes the reaction?

a)

It is a combustion reaction because heat is produced by the reaction.

b)

It is a double replacement reaction because 2Cl atoms are added to Zn.

c)

It is an acid-base reaction because HCl is an acid that is capable of exchanging H+.

d)

It is an oxidation-reduction reaction because zinc is oxidized and hydrogen is reduced.

5.

In the reaction between C5H5N(aq) and HHCl(aq) represented above, C5H5N acts as

a)

a Brønsted-Lowry base

b)

a Brønsted-Lowry acid

c)

the conjugate base of HCl

d)

the conjugate acid of [C5H5NH]+

6.

A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms.

Which of the following is evidence that ionic bonds formed during the precipitation?

a)

The resulting solution is colorless.

b)

The resulting solution conducts electricity.

c)

The precipitate has a high melting point.

d)

The temperature of the solution did not change significantly during the precipitation.

7.

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

When a zinc plate is placed in an aqueous solution of copper sulfate, elemental copper forms, as represented by the equation above. Which of the following represents the reduction half-reaction of the reaction? (Sulfate, SO4, has a -2 charge)

a)

Cu+2+(aq)+2e →Cu(s)Cu^{+2}+(aq)+2e\ →Cu(s)  

b)

Cu(s) → Cu+2(aq) + 2eCu\left(s\right)\ \rightarrow\ Cu^{+2}\left(aq\right)\ +\ 2e  

c)

Zn(s) + 2e → Zn−2(aq)Zn\left(s\right)\ +\ 2e\ \rightarrow\ Zn^{-2}\left(aq\right)  

d)

Zn(s) → Zn+2(aq) +2eZn\left(s\right)\ \rightarrow\ Zn^{+2}\left(aq\right)\ +2e  

8.

What is a titration?

a)

when the moles of hydrogen ions is equal to the moles of hydroxide ions

b)

adding a known amount of solution of known concentration to determine the concentration of an unknown

c)

reaction in which an acid and a base react in an aqueous solution to produce a salt and water

d)

the extent of ionization of an acid or base

9.
In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
10.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
11.
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-
12.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
13.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

14.
Neutralization reactions
a)
formed from joining positive and negative ions 
b)
increases OH ions
c)
froms a salt and water
d)
increases H2O ions
15.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
16.
Is calcium oxidized or reduced in the following reaction? 
2 CaO--> 2 Ca + O2
a)
Oxidized
b)
Reduced
17.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
18.
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
19.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

20.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
21.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
22.

In the equation below, what is the Bronsted Lowry base (accepts H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

23.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
24.

30mL of NaOH is neutralised by 12.3mL of 0.2mol/l HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

25.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
26.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
27.
If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of sulfuric acid, what is the concentration of the acid?
a)
0.2 M
b)
5 M
c)
0.5 M
28.

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

29.

Which of the following represents the net ionic equation for the precipitation reaction between sodium phosphate and lead (II) acetate?

a)

2Na3PO4+ 3Pb(C2H3O2)2 --> Pb3(PO4)2 + 6NaC2H3O2

b)

6Na+ + 2PO4-3 + 3Pb+2 + 3C2H3O2-1 --> Pb3(PO4)2 + 6NaC2H3O2

c)

2PO4-3 + 3Pb+2 --> Pb3(PO4)2

d)

Na+ + C2H3O2-1 --> NaC2H3O2

30.

Chemical or physical change? 2 H2O(l) + O2(g) → 2 H2O2(l)

a)

Chemical

b)

Physical

31.

Chemical or physical change? H2O(l) → H2O(g)

a)

Chemical

b)

Physical

32.

Physical changes occur when...

a)

bonds are broken and formed

b)

a different phase appears in the product side

33.

Chemical changes occur when...

a)

bonds are broken and formed

b)

a different phase appears in the product side

34.

Which observation suggests a chemical change occurred?

a)

Change in total volume

b)

Change in temperature

c)

Change in total pressure

35.

Which observation suggests a chemical change occurred?

a)

The mass stays constant

b)

The solution stays colorless

c)

A precipitate forms

36.

Which observation suggests a physical change occurred?

a)

The shape of an object changed

b)

Color change

c)

Clear solutions turn cloudy

37.

Boiling is an example of a __________

a)

Physical change because bonds are broken

b)

Physical change because IMFs are overcome

c)

Chemical change because bonds are broken

d)

Chemical change because IMFs are overcome

38.

What represents the net ionic equation for the reaction that occurs when the solutions of sodium carbonate and calcium nitrate are combined?

a)

Na2CO3 + Ca(NO3)2 --> 2NaNO3 + CaCO3

b)

2Na+ + CO3-2 + Ca+2 + 2NO3-1 --> 2NaNO3 + CaCO3

c)

Na+ + NO3-1 --> NaNO3

d)

CO3-2 + Ca+2 --> CaCO3

39.

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

40.

In order to be considered an oxidation-reduction reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

the pH must change

41.

In order to be considered an acid-base reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

one or more protons must be transfered

42.

In a combustion reaction,

a)

oxygen must be a reactant and carbon dioxide and water are products

b)

carbon dioxide and water are reactants and oxygen must be a product

43.

In a redox reaction, electrons are

a)

transferred from the species that's reduced to the species that's oxidized

b)

transferred from the species that's oxidized to the species that's reduced

44.

An acid is defined as a...

a)

proton donor

b)

proton acceptor

45.

An base is defined as a...

a)

proton donor

b)

proton acceptor

46.

In this example, H+ + H2O -> H3O+ the water acts as a(n)

a)

acid donating a proton

b)

acid accepting a proton

c)

base donating a proton

d)

base accepting a proton

47.

In the following example, CH3CH2COOH(aq) + H2O(l) ⇄ CH3CH2COO-(aq) + H3O+(aq) what would be considered a conjugate acid-base pair?

a)

CH3CH2COOH(aq) and H2O(l)

b)

CH3CH2COO-(aq) and H3O+(aq)

c)

CH3CH2COO-(aq) and CH3CH2COOH(aq)

d)

CH3CH2COOH(aq) and H3O+(aq)

48.

Which of the following represent a Brønsted-Lowry conjugate acid-base pair?

a)

HF and H2O

b)

NaOH and H2O

c)

HF and NaOH

d)

HF and F-

49.

Which of the following represent a Brønsted-Lowry conjugate acid-base pair

a)

HCN and H2O

b)

H3O+ and CN-

c)

CN- and H+

d)

HCN and CN-

50.

Given this general acid-base reaction HA + B- --> A- + HB, if K>0, which acid is stronger?

a)

HA

b)

HB

51.

Given this general acid-base reaction HA + B- --> A- + HB, if K<0, which base is stronger?

a)

A-

b)

B-

52.

Given the following: NH3(aq) + HCl(aq) ⇄ NH4+(aq) + Cl-(aq)

The Brønsted-Lowry acids in the reaction represented above are

a)

NH3(aq) and NH4+(aq)

b)

HCl(aq) and NH4+(aq)

c)

HCl(aq) and Cl-(aq)

d)

NH3(aq) and HCl(aq)

53.

Is this a chemical or physical process? CO2(g) → C(s) + O2(g)

a)

chemical

b)

physical

c)

both chemical and physical

54.

Is this a chemical or physical process? H2O(s) → H2O(l)

a)

chemical

b)

physical

c)

both chemical and physical

55.

Is this a chemical or physical process? MgCl2(s) → Mg+2(aq) + 2Cl-1(aq)

a)

chemical

b)

physical

c)

both chemical and physical

56.

What coefficients balance this equation? ___Na + ___ZnI2 → ____NaI + ___Zn

a)

1,2,1,2

b)

2,1,2,1

c)

2,2,2,1

d)

1,1,2,1

57.

What coefficients balance this equation? ___N2 + ___H2 → ____NH3

a)

1,3,2

b)

2,1,2

c)

2,3,1

d)

1,2,3

58.

Which substance is the precipitate in this reaction? FeCl3(aq) + NaOH(aq) → Fe(OH)3(s) + NaCl(aq)

a)

FeCl3

b)

NaOH

c)

Fe(OH)3

d)

NaCl

59.

What are the spectator ions in this reaction? Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-1(aq)

a)

Fe+3 and Cl-1

b)

Na+1 and Cl-1

c)

Fe+3 and Na+

d)

Na+1 and OH-1

60.

What is the net ionic equation for this reaction? Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-1(aq)

a)

Fe+3 (aq) + OH-1(aq) → Fe(OH)3(s) 

b)

Na+1(aq) + Cl-1(aq) → NaCl(aq)

c)

Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-

61.

Precipitates are ____________________________ in solution.

a)

miscible

b)

soluble

c)

insoluble

62.

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.

63.
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 
64.
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)
65.
In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
66.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
67.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound
68.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
69.

Which of the following is an Arrhenius Acid?

a)

LiOH

b)

CO32-

c)

OH-

d)

H3PO4

70.

In this reaction...

CH3NH2 + H2O ↔ CH3NH3+ + OH-

CH3NH2 can be classified as which of the following? (HINT...follow the H+!!!)

a)

A Brønsted-Lowry base

b)

A Brønsted-Lowry acid

c)

An Arrhenius acid

d)

An Arrhenius base

71.

The conjugate base of H2SO4 is ___.

a)

H2SO3

b)

HSO4-1

c)

H3SO4+1

d)

SO4-2

72.

NH3 + H2O ↔ NH4+ + OH-

What is H2O in this reaction?

a)

acid

b)

base

c)

conjugate acid

d)

conjugate base

73.

Balance this equation:


____ Zn + _____HCl → _____ ZnCl2 + _______H2

a)

1,2,1,2

b)

2,1,1,2

c)

1,2,1,1

d)

1,3,1,2

74.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If 70.50 g of Zn and 71.65 g of HCl are combined, what is the limiting reactant?

a)

Zn limits

b)

HCl limits

c)

ZnCl2 limits

d)

H2 limits

75.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If 70.50 g of Zn and 71.65 g of HCl are combined, what is the maximum mass of zinc chloride that can be produced?

a)

133.9 g ZnCl2

b)

131.8 g ZnCl2

c)

146.9 g ZnCl2

d)

267.83 g ZnCl2

76.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If the reaction is done in a lab and 125.6 g of zinc chloride are produced, what is the percent yield?

a)

85.50%

b)

93.80%

c)

95.29%

d)

46.90%

77.

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

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