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Worksheets

Sect 3&4

Total questions: 139

Worksheet time: 6hrs 8mins

Name
Class
Date
1.

Match the following

a)

Theoretical Yield

1.

the maximum amount of product that could be formed from given amounts of reactants

b)

Limiting Reagent

2.

the reactant that determines the amount of product that can be formed in a reaction

c)

Actual Yield

3.

the amount of product formed when a reaction is carried out in the laboratory

d)

Excess Reagent

4.

the reactant that is not completely used up in a reaction

e)

Percent Yield

5.

the ratio of the actual yield to the theoretical yield

2.

The mass % of C in octane (C8H18) is __________

a)

15.88%

b)

84.12%

c)

8%

d)

114.12%

e)

12.01 %

3.

What is the percentage composition of C12H22O11?

a)

12.0% C

22.2% H

16.0% O

b)

40.6% C

22.2% H

37.2% O

c)

42.1% C

6.5% H

51.4% O

d)

41.1% C

12.1% H

35.8% O

4.

How many molecules are there in 125.0 g of Magnesium Phosphate, Mg3(PO4)2?

a)

2.86 x 1023

molecules

b)

1.97 x 1029

molecules

c)

6.07 x 1039

molecules

d)

6.02 x 1023

molecules

5.

Solid potassium reacts violently with water, producing heat, hydrogen gas, and potassium hydroxide. How many molecules of hydrogen gas are formed when

8.7 g of potassium are added to water?

2K + 2H2O → 2KOH + H2

a)

6.7 x 1023

molecules H2

b)

1.4 x 1022

molecules H2

c)

6.7 x 1022

molecules H2

d)

1.4 x 1023

molecules H2

6.

A compound has a molar mass of 90 grams, which contains 79.9% C and 20.1% H by mass.  What is the molecular formula of the compound?

a)

CH4

b)

C4H12

c)

C5H15

d)

C6H18

7.

Balance the following equation:

_CH4 + _O2 → _CO2 + _H2O

a)

1 : 2 : 1 : 2

b)

2 : 3 : 2 : 4

c)

1 : 6 : 4 : 5

d)

2 : 12 : 8: 6

8.

When balancing a chemical equation, why must the subscripts remain unchanged?

a)

Law of Conservation of Mass

b)

Changing the subscript is allowed if you need to balance the reaction

c)

Law of Conservation of Energy

d)

Changing the subscript in a formula changes the chemical composition of the compound

9.

Write the correct formula and the formula weight for

Copper (II) Nitrate

a)

Cu2NO

157.11 g/mole

b)

CuNO2

109.56 g/mole

c)

Cu2(NO)3

217.13 g/mole

d)

Cu(NO3)2

187.57 g/mole

10.

Which of the following are a Hydrate?

a)

CaS (aq)

b)

CuSO4 * 5H2O

c)

H2O

d)

None of the following are hydrates

11.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
12.
What is the molar mass of table salt (NaCl)?
a)

116.89 g/mol

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

13.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
14.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

15.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

16.

Calculate the molar mass of NH4NO2

a)

50 g/mol

b)

60 g/mol

c)

64 g/mol

d)

78 g/mol

17.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
18.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
19.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
20.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
21.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
22.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
23.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.0829 moles

24.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

25.

What is the mass of 4.98 x 1024 atoms of Zn?

a)

541 g

b)

8.27 g

c)

.122 g

d)

4.59 x 1046 g

26.

How many moles of sodium chloride are in a 321.8 g sample?

a)

18810 moles

b)

3.315 x 1024 moles

c)

5.507 moles

d)

4.767 moles

27.

How many formula units of calcium chloride are in a 25.69 g sample?

a)

1.394 x 1023 F.U.'s

b)

2851 F.U.'s

c)

.2315 F.U.'s

d)

3.845 x 1025 F.U.'s

28.

What is the mass of one mole of silver?

a)

32.06 g

b)

107.87 g

c)

14.01 g

d)

22.99 g

29.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.0829 moles

30.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

31.

What would be the mass of 9.76 x 1022 formula units of SrCl2?

a)

.1622 g

b)

25.7 g

c)

20.0 g

d)

.3589 g

32.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
33.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
34.

What is the molar mass of fluorine gas F2?

a)
18.998 g/mol
b)
38 g/mol
c)
9 g/mol
d)
18 g/mol
35.

What is the molar mass of NaCl?

a)

58.45g/mol

b)

28g/mol

c)

12g/mol

d)

6.02 x 1023

36.

Calculate the % composition by mass of oxygen present in H2SO4.

a)

16.3%

b)

65.25%

c)

32.6%

d)

57.14%

37.
How many moles are 98.3 grams of aluminum hydroxide, Al(OH)3?
a)
1.26 moles
b)
0.8 moles
c)
7,673.4 moles
d)
150 moles
38.

Convert 25 g of NaBr to molecules

a)

102.96 molecules

b)

0.24 molecules

c)

1.45x1023 molecules

d)

2.34 x 1020molecules

39.

Calculate the percentage of composition by mass of oxygen in Al(HCO3)3.

a)

22.86 %

b)

68.57 %

c)

78.26 %

d)

40.50 %

40.

Which of the following statement are true about the formula of dinitrogen monoxide, N2O?

a)

The relative molecular mass is 28.

b)

One molecule of N2O consists of one nitrogen atom and one oxygen atom.

c)

One mole of N2O contains 6.02 x 1023 atoms of nitrogen.

d)

One mole of N2O consists of two mole of nitrogen atom and one mole of oxygen atom.

41.

The mass of 4.50 x 1022 Cu atoms is ___________

a)

4.75 g

b)

63.55 amu

c)

7.47 x 10-2 g

d)

7.47 x 10-2 amu

42.

How many particles are found in a mole?

a)

6.022 x 10236.022\ x\ 10^{23}  

b)

6.022 x 10236.022\ x\ 1023  

c)

6022 x 10236022\ x\ 10^{23}  

d)

6022 x 10236022\ x\ 1023  

43.

What are the units used for Molar Mass

a)

grams

b)

mols

c)

g/mol

d)

mol/g

44.

How many grams are in 3 mol of carbon?

a)

6 grams

b)

12 grams

c)

18 grams

d)

36 grams

45.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
46.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
47.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
48.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
c)
C = 92.2%
H = 7.8%
d)
C = 71.9%
H = 28.1%
49.

Which of the following is a molar volume conversion factor?

a)

22.4 L/mole

b)

6.02 x 1023 atoms/mole

c)

(Atomic Mass) g/mol

d)

Mole to Mole Ratio

50.

Which of the following is a molar particle conversion factor?

a)

22.4 L/mole

b)

6.02 x 1023 atoms/mole

c)

(Atomic Mass) g/mol

d)

Mole to Mole Ratio

51.

Which of the following is a molar mass conversion factor?

a)

22.4 L/mole

b)

6.02 x 1023 atoms/mole

c)

(Atomic Mass) g/mol

d)

Mole to Mole Ratio

52.

Which of the following equals one mole?

a)

22.4 L/mole

b)

6.02 x 1023 atoms/mole

c)

(Atomic Mass) g/mol

d)

All are equal to one mole

53.

What is the name of the following conversion factor?

1 mole = 22.4 L

a)

Molar Mass

b)

Molar Particle

c)

Molar Volume

d)

All are correct

54.

What is the name of the following conversion factor?

1 mole = 6.02 x 1023

a)

Molar Mass

b)

Molar Particle

c)

Molar Volume

d)

All are correct

55.

What is the name of the following conversion factor?

1 mole = Atomic Mass (g)

a)

Molar Mass

b)

Molar Particle

c)

Molar Volume

d)

All are correct

56.

Balance the following equation:  _ Mg +  _H3PO4  -->_ Mg3(PO4 ) 2 + _H2

a)

3:2:1:3

b)

1:1:1:3

c)

3:2:2:2

d)

3:2:1:2

57.

For the reaction represented by the equation

CH4 + 2O2 → CO2+ 2H2O

how many moles of carbon dioxide can be produced from 8.0 mol of oxygen and an excess of hydrogen?

a)

1 mole

b)

2 moles

c)

4 moles

d)

8 moles

58.

If 3 cups of flour and 2/3 cup of shortening are needed for a recipe that makes 7 dozen cookies, how many dozen can you make if you used up all 6 cups of flour and 3 cups of shortening?

*HINT: You are trying to calculate the theoretical yield

a)

14 cookies

b)

24 cookies

c)

14 dozen

d)

24 dozen

59.

How many liters of H2 are needed to react completely with 20.0 L of Cl2 (at STP)?

H2 + Cl2 --> 2HCl

a)

10 L

b)

20 L

c)

40 L

d)

22.4 L

60.

Balance the following equation:

_C2H6 + _O2 → _CO2 + _H2O

a)

1 : 2 : 1 : 2

b)

2 : 3 : 4 : 4

c)

1 : 6 : 4 : 5

d)

2 : 7 : 4: 6

61.

Match the following

a)

Theoretical Yield

1.

the calculated amount of product that will form during a reaction is called

b)

Limiting Reagent

2.

when two substances react to form products, this reactant gets completely used up

c)

Actual Yield

3.

the measured amount of product obtained during a chemical reaction

d)

Excess Reagent

4.

when two substances react to form products, there will be left over or unused of this reactant

e)

Stoichiometry

5.

The calculation of quantities in chemical equations is called

62.

Match the following

a)

Limiting reagent

1.

The amount of the product is determined by the ____

b)

Excess reagent

2.

Some of the ___ is left over after the reaction is complete

c)

Coefficients

3.

___ are changed to balance a chemical reaction

d)

Subscripts

4.

___ are never changed when balancing reactions because it changes the chemical composition

e)

Not true

5.

The reactant that has the smallest given mass is always the limiting reactant

63.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40.0 g
b)
80.0 g
c)
16.0 g
d)
32.0 g
64.
Fluorine is diatomic.  What is the molar mass of fluorine gas?
a)
18.998 g/mol
b)
37.996 g/mol
c)
9 g/mol
d)
18 g/mol
65.
How many grams are in 3.3 mol of Potassium Sulfide?
a)

363 g

b)
454 g
c)
238 g
d)
132 g
66.

How many moles is 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

67.

Find the molar masses of the following compounds:

(NH4)2CO3

a)

303.3 g/mole

b)

102.9 g/mole

c)

74.1 g/mole

d)

160.0 g/mole

e)

96.0 g/mole

68.

Find the molar masses of the following compound

C6H12O6

a)

303.3 g/mole

b)

102.9 g/mole

c)

180.0 g/mol

d)

160.0 g/mole

e)

96.0 g/mole

69.

Calculate the formula mass of Ba(BrO4)2

4 lines
70.

How many particles are in 45.6 grams of Aluminum bromide?

4 lines
71.

Calculate the formula mass of (NH3)2O.

4 lines
72.

Convert 35.5 grams cobalt (III) chloride to moles

4 lines
73.

Calculate the formula mass of Aluminum chloride

4 lines
74.

2.0 moles of AuCl3 is equal to how many grams?

a)

152 g

b)

607 g

c)

464 g

d)

0.007 g

75.

85.0 g of NaOH is equal to how many moles?

a)

3400 moles

b)

45 moles

c)

0.47 moles

d)

2.1 moles

76.

36.0 g of Be contains how many moles?

a)

0.25 moles

b)

27 moles

c)

4.0 mole

d)

324 moles

77.

4.0 moles of H2O would have a mass of ___________?

a)

72.0 g

b)

68.0 g

c)

0.22 g

d)

4.5 g

78.

6.0 g of Carbon is equal to how many moles?

a)

1.0 moles

b)

0.5 moles

c)

2.0 moles

d)

72.0 moles

79.

 How many moles are in 220.0 g of Ar?

a)

0.18 moles

b)

180 moles

c)

8800 moles

d)

5.5 moles

80.

 How many grams are in 0.2 moles of BeI2 ?

a)

52.6 g

b)

1315 g

c)

27.2 g

d)

0.002 g

81.

How many moles are present in a 32.5 sample of aluminum chloride AlCl3?

a)

720 moles

b)

1.2 moles

c)

0.24 moles

d)

4.1 moles

82.
What is a reactant?
a)
a volatile chemical
b)
a dangerous substance
c)
the substances you start with in a chemical reaction
d)
the substances that are formed by a chemical reaction 
83.
What is a product?
a)
a fancy word for make-up
b)
a volatile chemical
c)
the substances you start with in a chemical reaction
d)
the substances that are formed by a chemical reaction
84.
The number of atoms you begin with in a chemical reaction ...
a)
must be the same as the number of  atoms you end with
b)
must be an even number
c)
can be different to the number you finish with
d)
changes depending on how much energy is formed
85.
What mathematical function do coefficients perform in a balanced equation?
a)
addition
b)
subtraction
c)
multiplication
d)
division
86.

Balance the following:

____ Fe + ____ Cl2 → ____ FeCl3

a)
1,1,2
b)
1,3,1
c)
2,2,3
d)
2,3,2
87.

Balance the following:

____ Al + ____ O2 → ____ Al2O3

a)
2,3,4
b)
4,3,2
c)
1,1,2
d)
2,1,1
88.

Balancing the following:

____ Al + ____ HCl → ____ AlCl3 + ____ H2

a)
1,3,1,2
b)
2,3,2,3
c)
2,6,2,3
d)
3,2,6,2
89.

Balancing the following:

____ Al + ____ HCl → ____ AlCl3 + ____ H2

a)
1,3,1,2
b)
2,3,2,3
c)
2,6,2,3
d)
3,2,6,2
90.

Balance the following:

____ H2SO4 + ____ NaNO2 → ____ HNO2 + ____ Na2SO4

a)
1,1,2,1
b)
1,2,2,1
c)
2,3,3,2
d)
4,3,2,1
91.

Balance the following:

____ H2SO4 + ____ NaNO2 → ____ HNO2 + ____ Na2SO4

a)
1,1,2,1
b)
1,2,2,1
c)
2,3,3,2
d)
4,3,2,1
92.
Balance the following: Fluorine and Aluminum oxide react to produce Aluminum fluoride and Oxygen
a)
6,2,4,3
b)
3,4,2,6
c)
5,1,3,2
d)
3,2,4,3
93.

Balance the following:

Dicarbon hexahydride and Oxygen react to produce

Carbon dioxide and Dihydrogen monoxide

C2H6 + O2 --> CO2 + H2O

a)

1,6,2,3

b)

1,6,3,2

c)

2,7,4,6

d)

6,4,7,2

94.

Balance the following:

Aluminum nitrate and Carbonic acid react to form

Aluminum carbonate and Nitric acid

Al(NO3)3 + H2CO3 --> Al2(CO3)3 + HNO3

a)

4,1,2,5

b)

1,3,6,2

c)

2,1,3,6

d)

2,3,1,6

95.

Which type of reaction is:

2 NaBr + Ca(OH)2 → CaBr2 + 2 NaOH

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
96.
Which type of reaction is: C2H4 + 3 O2 → 2 CO2 + 2 H2O
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
97.
Which type of reaction is: C2H4 + 3 O2 → 2 CO2 + 2 H2O
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
98.

Which type of reaction is:

2 H3AsO4 → As2O5 + 3 H2O

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
99.

Which type of reaction is:

2 NH3 + H2SO4 → (NH4)2SO4

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
100.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
101.

Which type of reaction is:

C7H16 + 10 O2 → 7 CO2 + 8 H2O

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
102.

Which type of reaction is:

8 Ag2S → 8 S + 16 Ag

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
103.

Which type of reaction is:

4 (NH4)3PO4 + 3 Pb(NO3)4 → 12 NH4NO3 + Pb3(PO4)4

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
104.

Which type of reaction is:

2 K + MgBr2 → 2 KBr + Mg

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
105.

Reaction type?

____ Fe + ____ Cl2 → ____ FeCl3

a)

Decomposition

b)

Single Replacement

c)

Double Repleacment

d)

Synthesis

106.

Reaction type?

____ Fe + ____ Cl2 → ____ FeCl3

a)

Decomposition

b)

Single Replacement

c)

Double Repleacment

d)

Synthesis

107.

What is the name of this compound MgSO4?

a)

magnesium sulfur

b)

magnesium sulfate

c)

magnesium sulfide

108.

Potassium hydroxide, KOH

a)

Soluble

b)

Insoluble

109.

Ammonium carbonate

a)

Soluble

b)

Insoluble

110.

Calcium carbonate

a)

Soluble

b)

Insoluble

111.

Lead(II) nitrate, PbNO3

a)

Soluble

b)

Insoluble

112.

Silver chloride, AgCl

a)

Soluble

b)

Insoluble

113.

Zinc hydroxide, Zn(OH)2

a)

Soluble

b)

Insoluble

114.

Which is the correct net ionic equation for this reaction?

AgNO3 + CaCl2 → AgCl + Ca(NO3)2

a)

Ca2+ (aq) + 2Cl- (aq) → CaCl2 (s)

b)

Ag+(aq) + Cl- (aq) → AgCl(s)

c)

Ag + Cl → AgCl

d)

Ag+ + Ca2+ → Ag2Ca (s)

115.

Which of the following reactions does NOT form a precipitate?

a)

Pb(NO3)2 (aq) + 2KI (aq) → PbI2 + 2KNO3

b)

Pb(NO3)2 (aq) + K2SO4 (aq) → PbSO4 + KNO3

c)

AgNO3 (aq) + Na2S (aq) → Ag2S + NaNO3

d)

KCl (aq) + NaNO3 (aq) → NaCl + KNO3

116.

What are the spectator ions in this reaction?

NaCl + AgNO3 → AgCl + NaNO3

a)

Ag+ and NO3-

b)

Na+ and Cl-

c)

Na+ and NO3-

d)

Ag+ and Cl-

117.

Which is the correct net ionic equation for this reaction?

3KOH + FeCl3 → 3KCl + Fe(OH)3

a)

3K+ (aq) + 3Cl- (aq) → 3KCl (s)

b)

Fe3+ (aq) + 3OH- (aq) → Fe(OH)3 (s)

c)

Fe3+ (aq) + Cl- (aq) → Fe(OH)3 (s)

d)

3K+ (aq) + 3OH- (aq) + Fe3+ (aq) + 3Cl- (aq) → Fe(OH)3 (s)

118.

What are the spectator ions in this reaction?

CuCl2 + 2NaOH → Cu(OH)2 + 2NaCl

a)

Cu2+ and OH-

b)

Cu2+ and Cl-

c)

Na+ and Cl-

d)

Na+ and OH-

119.

What is the precipitate formed in this reaction?

3CaS + 2Al(NO3)3 → Al2S3 + 3Ca(NO3)2

a)

CaS

b)

Al(NO3)3

c)

Al2S3

d)

Ca(NO3)2

120.

What are the spectator ions in this reaction?

3Pb(NO3)2 + 2AlCl3 → 3PbCl2 + 2Al(NO3)3

a)

Pb2+ and Cl-

b)

Cl- and Al3+

c)

Al3+ and NO3-

d)

NO3- + Pb2+

121.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

122.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

123.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

124.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

125.
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)
126.
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
127.
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-
128.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)?

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

3Cu2+(aq) + 2 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

129.

Copper(II) sulphate solution

a)

Electrolyte

b)

Non-electrolyte

130.

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

131.

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

a)

catalyst

b)

metalloid

c)

electrolyte

d)

nonelectrolyte

132.

What happens when BaF2(s) is dissolved in water?

a)

F- ions are attracted to the oxygen atoms of the water

b)

F- ions are attracted to the hydrogen atoms of the water

c)

Ba2+ ions are attracted to the hydrogen atoms of the water

d)

No attractions are involved, the crystal just falls apart

133.

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

134.

Which of the following is not an electrolyte?

a)

KBr

b)

LiOH

c)

RbNO3

d)

CH4

135.

Solutions that conduct a current are called ____________ and are made from ___________ compounds.

a)

electrolytes; ionic

b)

nonelectrolytes; ionic

c)

electrolytes; molecular

d)

electrolytes; covalent

136.

If 400 mL of a 8.0 M solution is diluted to a molarity of 5.3M, about how much solvent volume was added?

a)

200 mL

b)

600 mL

c)

400 mL

d)

180 mL

137.
what is the molarity of a solution that contains 125 g NaCl in 4.00 L of solution?
a)
0.535 M NaCl
b)
2.14 M NaCl
c)
8.56 M NaCl
d)
31.3 M NaCl
138.
A dissolved solute that does not form ions is:
a)
a nonelectrolyte
b)
a weak electrolyte
c)
a strong electrolyte
d)
insoluble
139.
What is the most common solvent in everyday life?
a)
Ethanol
b)
Tuluene
c)
Water
d)
Oils

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