Free Printable Lesson 46

Free Printable Worksheets

Worksheets

Lesson 46

Total questions: 86

Worksheet time: 43mins

Name

Class

Date

1.

is this compound soluble or insoluble : BaSO₄

a)

soluble

b)

insoluble

2.

is this compound soluble or insoluble : CaCl2

a)

soluble

b)

insoluble

3.

is this compound soluble or insoluble : Pb(NO₃)₂

a)

soluble

b)

insoluble

4.

is this compound soluble or insoluble : Ag₂SO₄

a)

soluble

b)

insoluble

5.

is this compound soluble or insoluble : Li₂SO₄

a)

soluble

b)

insoluble

6.

is this compound soluble or insoluble : PbBr₂

a)

soluble

b)

insoluble

7.

is this compound soluble or insoluble : Na₂SO₄

a)

soluble

b)

insoluble

8.

is this compound soluble or insoluble : AgCl

a)

soluble

b)

insoluble

9.

is this compound soluble or insoluble : CsI

a)

soluble

b)

insoluble

10.

is this compound soluble or insoluble : NH₄OH

a)

soluble

b)

insoluble

11.

is this compound soluble or insoluble : K₃PO₄

a)

soluble

b)

insoluble

12.

is this compound soluble or insoluble : MgCl₂

a)

soluble

b)

insoluble

13.

is this compound soluble or insoluble : Hg₂Cl₂

a)

soluble

b)

insoluble

14.

is this compound soluble or insoluble : Pb(C₂H₃O₂)₂

a)

soluble

b)

insoluble

15.

is this compound soluble or insoluble : CaCO₃

a)

soluble

b)

insoluble

16.

is this compound soluble or insoluble : BaCl₂

a)

soluble

b)

insoluble

17.

is this compound soluble or insoluble : Ca(NO₃)₂

a)

soluble

b)

insoluble

18.

is this compound soluble or insoluble : CuS

a)

soluble

b)

insoluble

19.

Which product is the precipitate (use solubility rules):

FeI₂+ 2NaOH → 2NaI + Fe(OH)₂

a)

FeI₂

b)

NaOH

c)

NaI

d)

Fe(OH)₂

20.

Which product is the precipitate (use solubility rules):

3BaCl₂+ 2Li₃PO₄ → 6LiCl + Ba₃(PO₄)₂

a)

LiCl

b)

Ba₃(PO₄)₂

c)

Li₃PO₄

d)

BaCl₂

21.

Which product is the precipitate (use solubility rules):

MgI₂+ K₂CrO₄ → MgCrO₄ + 2KI

a)

KI

b)

MgCrO₄

c)

K₂CrO₄

d)

MgI₂

22.

Which product is the precipitate (use solubility rules):

CaSO₄+ Pb(NO₃)₂ → PbSO₄ + Ca(NO₃)₂

a)

Ca(NO₃)₂

b)

CaSO₄

c)

PbSO₄

d)

Pb(NO₃)₂

23.

Which product is the precipitate (use solubility rules):

2LiCl+ Pb(C₂H₃O₂)₂ → 2LiC₂H₃O₂ + PbCl₂

a)

Pb(C₂H₃O₂)₂

b)

PbCl₂

c)

LiC₂H₃O₂

d)

LiCl

24.

Which product is the precipitate (use solubility rules):

Mg(CN)₂+Ca(OH)₂ →Ca(CN)₂ + Mg(OH)₂

a)

Mg(OH)₂

b)

Ca(OH)₂

c)

Mg(CN)₂

d)

Ca(CN)₂

25.

Use graph 1 on the solubility reference sheet to answer:

At what temperature will 100g of KBr dissolve in 100 ml of water

a)

18°C

b)

93°C

c)

53°C

26.

Use graph 1 on the solubility reference sheet to answer:

At what temperature will NaCl and KNO₃ have the same solubility?

a)

27°C

b)

58°C

c)

48°C

27.

Use graph 1 on the solubility reference sheet to answer:

How many grams of KNO₃ would dissolve in 100ml of water at 80°C?

a)

170 g

b)

40 g

c)

95 g

28.

Use graph 1 on the solubility reference sheet to answer:

At what temperature will KNO₃ and NaClO₃ have the same solubility?

a)

27°C

b)

48°C

c)

95°C

29.

Use graph 1 on the solubility reference sheet to answer:

How many grams of NaClO₃ would dissolve in 100ml of water at 65°C?

a)

120 g

b)

163 g

c)

89 g

30.

Use graph 1 on the solubility reference sheet to answer:

How many grams of KBr would dissolve in 100ml of water at 100°C?

a)

104 g

b)

230 g

c)

89 g

31.

Use graph 1 on the solubility reference sheet to answer:

At what temperature will 120 g of KNO₃ dissolve in 100ml of water?

a)

104 °C

b)

35°C

c)

64 °C

32.

How would raising air pressure effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

33.

How would Agitating the solution effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

34.

How would Decreasing air pressure effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

35.

How would Increasing temperature effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

36.

How would Increasing surface area effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

37.

How would Lowering temperature effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

38.

How would Decreasing surface area effect the rate of dissolution of a solid?

a)

Dissolve faster

b)

Dissolve more slowly

c)

No effect

39.

A student wants to dissolve some sugar into a batch of tea. The student is impatient and wants this to happen as quickly as possible. What is the best way to achieve this in the shortest amount of time?

a)

lower temperature of tea and stir like crazy using cubed sugar

b)

heat the tea and let sit to dissolve granulated sugar

c)

heat the tea and stir granulated sugar like crazy

d)

put the cubed sugar in and wait

40.

Which is the definition of a Saturated solution?

a)

maximum solute dissolved in solvent at a certain amount of water and a certain temperature

b)

less than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

c)

more than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

41.

Which is the definition of a Supersaturated solution?

a)

maximum solute dissolved in solvent at a certain amount of water and a certain temperature

b)

less than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

c)

more than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

42.

Which is the definition of an Unsaturated solution?

a)

maximum solute dissolved in solvent at a certain amount of water and a certain temperature

b)

less than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

c)

more than maximum solute dissolved in solvent at a certain amount of water and a certain temperature

43.

Used Graph #1 to determine proper saturation of the following:

100 g of water conains 100g of NaClO₃ at 20°C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

44.

Used Graph #1 to determine proper saturation of the following:

100 g of KBr are dissolved in 100g of water at 20°C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

45.

Used Graph #1 to determine proper saturation of the following:

A solution contains 20 g of NaCl in 100g of water at 10°C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

46.

Used Graph #1 to determine proper saturation of the following:

At 50°C, 100g of KNO₃ is dissolved in 100g of water.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

47.

Used Graph #1 to determine proper saturation of the following:

109g of NaClO₃ is dissolved in 100g of water at 20°C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

48.

Used Graph #1 to determine proper saturation of the following:

At 65°C, 90g of KBr is dissolved in 100g of water.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

49.

Used Graph #1 to determine proper saturation of the following:

A solution contains 170g of KNO₃ in 100 g of water at 65°C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

50.

What are the two characteristics of an electrolyte?

a)

covalent, insoluble

b)

ionic, soluble

c)

ionic,insoluble

d)

covalent, soluble

51.

Is SiBr₄an electrolyte?

a)

yes

b)

no

52.

Is PbI₂an electrolyte?

a)

yes

b)

no

53.

Is SrCl₂an electrolyte?

a)

yes

b)

no

54.

Is Na₂SO₄an electrolyte?

a)

yes

b)

no

55.

Is K₂CO₃an electrolyte?

a)

yes

b)

no

56.

Is PBr₅an electrolyte?

a)

yes

b)

no

57.

Is AgNO₃an electrolyte?

a)

yes

b)

no

58.

Is Mg(NO₃)₂an electrolyte?

a)

yes

b)

no

59.

Is NaOHan electrolyte?

a)

yes

b)

no

60.

Is Hg₂Br₂an electrolyte?

a)

yes

b)

no

61.

Is N₂O₅an electrolyte?

a)

yes

b)

no

62.

Is IF₇an electrolyte?

a)

yes

b)

no

63.

What is the effect on solubility when you Decrease air pressure on a solid solute?

a)

More soluble

b)

Less soluble

c)

No effect

64.

What is the effect on solubility when you Decrease air pressure on a gas solute?

a)

More soluble

b)

Less soluble

c)

No effect

65.

What is the effect on solubility when you Increase air pressure on a solid solute?

a)

More soluble

b)

Less soluble

c)

No effect

66.

What is the effect on solubility when you Increase air pressure on a gas solute?

a)

More soluble

b)

Less soluble

c)

No effect

67.

What is the effect on solubility when you Decrease temperature on a solid solute?

a)

More soluble

b)

Less soluble

c)

No effect

68.

What is the effect on solubility when you Decrease temperature on a gas solute?

a)

More soluble

b)

Less soluble

c)

No effect

69.

What is the effect on solubility when you Increase temperature on a solid solute?

a)

More soluble

b)

Less soluble

c)

No effect

70.

What is the effect on solubility when you Increase temperature on a gas solute?

a)

More soluble

b)

Less soluble

c)

No effect

71.

Which of the following would keep solids and gases from being considered complete opposites in regards to solubility?

a)

Increasing temperature has the same effect on the solubility of solids and gases.

b)

Decreasing air pressure has the same effect on the solubility of solids and gases.

c)

Changing the temperature has no effect on the solubility of gases.

d)

Changing the air pressure has no effect on the solubility of solids.

72.

Which beaker shown above would be able to dissolve the greatest amount of gases?

a)

Q

b)

R

c)

S

d)

T

73.

which beaker would dissolve the greatest amount of gases?

a)

average temp, high pressure

b)

high temp, high pressure

c)

lower temp, low pressure

d)

lowest temp, high pressure

74.

which beaker would dissolve the greatest amount of solids?

a)

average temp, high pressure

b)

high temp, pressure no count

c)

lower temp, low pressure

d)

lowest temp,pressure no count

75.

Which beaker shown above would be able to dissolve the greatest amount of solids?

a)

Q

b)

R

c)

S

d)

T

76.

Using graph #2 on the solubility reference sheet:

At what temperature will 80 g of KNO₃ dissolve in 100mL of water?

a)

79°C

b)

35°C

c)

45°C

77.

Using graph #2 on the solubility reference sheet:

How many grams of KNO₃would dissolve in 100mL of water at 60°C

a)

110 g

b)

42 g

c)

53g

78.

Using graph #2 on the solubility reference sheet:

How many grams of KClwould dissolve in 100mL of water at 40°C

a)

69 g

b)

38 g

c)

59g

79.

Using graph #3 on the solubility reference sheet:

At what pressure of O₂ is hemoglobin 70% saturated?

a)

5.4 kPa

b)

3.4 kPa

c)

7.2 kPa

80.

Using graph #3 on the solubility reference sheet:

What percentage of hemoglobin will be saturated at 8 kPa O₂?

a)

25%

b)

94%

c)

68%

81.

Using graph #3 on the solubility reference sheet:

At what pressure of O₂ is hemoglobin 40% saturated?

a)

6.9 kPa

b)

3.4 kPa

c)

1.2 kPa

82.

Using the solubility reference sheet: If 0.250 moles of Na₂SO₄ are dissolved in 450 mL, what is the molarity of the solution?

a)

1.8 M

b)

0.11 M

c)

0.56 M

83.

Using the solubility reference sheet: What is the molarity of a solution made by dissolving 50.0 g of CaCl₂ in enough water to make 0.800 L of solution

a)

1.8 M

b)

0.36 M

c)

0.56 M

84.

Using the solubility reference sheet: If 0.500 liters of solution contains 0.050 moles of KNO₃ , what is the molarity of the solution?

a)

0.025M

b)

10 M

c)

0.1 M

85.

Using the solubility reference sheet: A teacher starts with 0.750 L of a 0.100M KOH solution and dilutes it to 1.25L. What is the concentration of KOH in the new solution?

a)

0.06M

b)

9.4 M

c)

0.17 M

86.

Using the solubility reference sheet: A student wants to make 0.125 L of 2.0 M LiCl by diluting a 3.0 M LiCl solution. How much of that solution should be used?

a)

0.08 L

b)

48 L

c)

0.18 L

100 %

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