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Solutions Test Worksheets

Total questions: 71

Worksheet time: 2hrs 22mins

Name
Class
Date
1.

In a true solution, the dissolved particles

a)

are visible to the eye

b)

will settle out on standing

c)

are always solids

d)

cannot be removed by filtration

2.

Salt water is classified as a

a)

mixture, with fixed composition

b)

mixture, with variable composition

c)

compound, with fixed composition

d)

compound, with variable composition

3.

In an aqueous solution of potassium chloride,

the solute is

a)

Cl- only

b)

K+ only

c)

K+Cl-

d)

H2O

4.

Which sample of matter is a mixture?

a)

H2O (s)

b)

H2O (l)

c)

NaCl (l)

d)

NaCl (aq)

5.

Most ionic substances are soluble in water because water molecules are

a)

nonpolar

b)

inorganic

c)

ionic

d)

polar

6.

An aqueous solution of copper sulfate is poured into a filter paper cone. What passes through the filter paper?

a)

only the solvent

b)

only the solute

c)

both solvent and solute

d)

neither the solute nor solvent

7.

Nonpolar solvents will most easily dissolve solids that are

a)

ionic

b)

covalent

c)

metallic

d)

colored

8.

As the temperature rises, the solubility of all gases in water

a)

decreases

b)

increases

c)

remains the same

9.

A decrease in pressure has the greatest effector a solution that contains

a)

a gas in a liquid

b)

a liquid in a liquid

c)

a solid in a solid

d)

a solid in a liquid

10.

Which diagram best illustrates the ion-molecule attractions that occur when the ions of NaCI (s) are added to water?

a)
b)
c)
d)
11.

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

a)

Cl- ions are attracted to the oxygen atoms of the water.

b)

Cl- ions are attracted to the hydrogen atoms of the water.

c)

Na+ ions are attracted to the hydrogen atoms of the water.

d)

No attractions are involved; the crystal just falls apart.

12.

Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as

a)

an element

b)

a compound

c)

a homogeneous mixture

d)

a heterogeneous mixture

13.

According to Table F, which substance is most soluble in water?

a)

AgCl

b)

CaCO3

c)

Na2CO3

d)

SrSO4

14.

At standard pressure, which substance becomes less soluble in water as temperature increases form 10.°C to 80.°C?

a)

HCl

b)

KCl

c)

NaCl

d)

NH4Cl

15.

Which compound is insoluble in water?

a)

KOH

b)

NH4Cl

c)

Na3PO4

d)

PbSO4

16.

Which compound is least soluble in water at 60.°C?

a)

KClO3

b)

KNO3

c)

NaCl

d)

NH4Cl

17.

The solubility of KClO3 (s) in water increases as the

a)

temperature of the solution increases

b)

temperature of the solution decreases

c)

pressure on the solution increases

d)

pressure on the solution decreases

18.

According to Reference Table G, which of these substances is most soluble at 60°C?

a)

NaCl

b)

KCl

c)

KClO3

d)

NH4Cl

19.

Based on Reference Table G, what change will cause the solubility of KNO3(s) to increase?

a)

decreasing the pressure

b)

increasing the pressure

c)

decreasing the temperature

d)

increasing the temperature

20.

According to Reference Table G, how does a decrease in temperature from 40°C to 20°C affect the solubility of NH3 and KCl?

a)

The solubility of NH3 decreases, and the solubility of KCl decreases.

b)

The solubility of NH3 decreases, and the solubility of KCl increases.

c)

The solubility of NH3 increases, and the solubility of KCl decreases.

d)

The solubility of NH3 increases, and the solubility of KCl increases.

21.

Under which conditions of temperature and pressure is a gas most soluble in water?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and low pressure

d)

low temperature and high pressure

22.

An unsaturated solution is formed when 80. grams of a salt is dissolved in 100. grams of water at 40.°C. This salt could be

a)

KCl

b)

KNO3

c)

NaCl

d)

NaNO3

23.

Which salt has the greatest change in solubility between 30°C and 50°C?

a)

KNO3

b)

KCl

c)

NaNO3

d)

NaCl

24.

The graph below represents four solubility curves. Which curve best represents the solubility of a gas in water?

a)

A

b)

B

c)

C

d)

D

25.

According to Reference Table G, which solution is saturated at 30°C?

a)

12 grams of KClO3 in 100 grams of water

b)

12 grams of KClO3 in 200 grams of water

c)

30 grams of NaCl in 100 grams of water

d)

30 grams of NaCl in 200 grams of water

26.

Based on Reference Table G, a solution of NaNO3 that contains 120 grams of solute dissolved in 100 grams of H2O at 50°C is best described as

a)

saturated and dilute

b)

saturated and concentrated

c)

supersaturated and dilute

d)

supersaturated and concentrated

27.

A solution contains 14 grams of KCl in 100. grams of water at 40°C. What is the minimum amount of KCl that must be added to make this a saturated solution?

a)

14g

b)

19g

c)

25g

d)

44g

28.

Which compound is insoluble in water?

a)

BaSO4

b)

CaCrO4

c)

KClO3

d)

Na2S

29.

The attraction between water molecules and an Na+ ion or a Cl- ion occurs because water molecules are

a)

linear

b)

symmetrical

c)

polar

d)

nonpolar

30.

According to your Reference Tables, which substance forms an unsaturated solution when 80 grams of the substance is dissolved in 100 grams of H2O at 10°C?

a)

KI

b)

KNO3

c)

NaNO3

d)

NaCl

31.

A mixture consists of sand an an aqueous salt solution. Which procedure can be used to separate the sand, salt, and water from each other?

a)

Evaporate the water, then filter out the salt.

b)

Evaporate the water, the filter out the sand.

c)

Filter out the salt, then evaporate the water.

d)

FIlter out the sand, then evaporate the water.

32.

As the temperature increases from 0°C to 25°C, the amount of NH3 that can be dissolved in 100 grams of water

a)

decreases by 10 grams

b)

decreases by 40 grams

c)

increases by 10 grams

d)

increases by 40 grams

33.

Base your answer to the question on the diagram below which represents the solubility curve of salt X. The four points on the diagram represent four solutions of salt X.


Which point represents the most concentrated solution of salt X?

a)

A

b)

B

c)

C

d)

D

34.

Base your answer to the question on the diagram below which represents the solubility curve of salt X. The four points on the diagram represent four solutions of salt X.


Which point represents a supersaturated solution of salt X?

a)

A

b)

B

c)

C

d)

D

35.

Which compound is insoluble in water?

a)

calcium bromide

b)

potassium bromide

c)

silver bromide

d)

sodium bromide

36.

Based on Reference Table F, which of these saturated solutions has the lowest concentration of dissolved ions?

a)

NaCl (aq)

b)

MgCl2 (aq)

c)

NiCl2 (aq)

d)

AgCl (aq)

37.

According to Reference Table F, which substance is most soluble?

a)

AgI

b)

CaSO4

c)

PbCl2

d)

(NH4)2CO3

38.

According to Reference Table G, how many grams of KNO3 would be needed to saturate 200 grams of water at 70°C?

a)

43g

b)

86g

c)

134g

d)

268g

39.

Which compound is least soluble in 100 grams of water at 40°C?

a)

SO2

b)

NaCl

c)

KClO3

d)

NH4Cl

40.

According to Reference Table G, a temperature change from 10°C to 30°C would have the least effect on the solubility of

a)

NaCl

b)

KClO3

c)

NH3

d)

SO2

41.

As the pressure on a gas confined above a liquid increases, the solubility of the gas in the liquid

a)

decreases

b)

increases

c)

remains the same

42.

What is the total mass of KNO3, that must be dissolved in 50. grams of H2O at 60.°C to make a saturated solution?

a)

32g

b)

53g

c)

64g

d)

106g

43.

A solution contains 100 grams of a nitrate salt dissolved in 100 grams of water at 50°C. The solution could be a

a)

supersaturated solution of NaNO3

b)

saturated solution of NaNO3

c)

supersaturated solution of KNO3

d)

saturated solution of KNO3

44.

The molarity of an aqueous solution of NaCl is defined as the

a)

grams of NaCl per liter of water

b)

grams of NaCl per liter of solution

c)

moles of NaCl per liter of water

d)

moles of NaCl per liter of solution

45.

What is the the total number of moles of NaCl (s) needed to make 3.0 liters of a 2.0 M NaCl solution?

a)

6.0 mol

b)

8.0 mol

c)

1.0 mol

d)

0.70 mol

46.

What is the total number of moles of solute in 250 milliliters of a 1.0 M solution of NaCl?

a)

1.0 mole

b)

0.25 mole

c)

0.50 mole

d)

42 moles

47.

A student obtained the following data in determining the solubility of a substance. Which graph best represents the solubility curve drawn from the results obtained by the student?

a)
b)
c)
d)
48.

What is the molarity of a solution that contains 20. grams of CaBr2 in 0.50 liter of solution?

a)

0.50 M

b)

0.20 M

c)

5.0 M

d)

10. M

49.

Which solution is the most concentrated?

a)

1 mole of solute dissolved in 1 liter of solution

b)

2 moles of solute dissolved in 3 liters of solution

c)

6 moles of solute dissolved in 4 liters of solution

d)

4 moles of solute dissolved in 8 liters of solution

50.

If 0.025 gram of Pb(NO3)2 is dissolved in 100. grams of H2O, what is the concentration of the resulting solution, in parts per million?

a)

2.5 x 10-4 ppm

b)

2.5 ppm

c)

250 ppm

d)

4.0 x 103 ppm

51.

Which statement describes the components of a mixture?

a)

Each component gains new properties.

b)

Each component loses its original properties.

c)

The proportions of components can vary.

d)

The proportion of components cannot vary.

52.

Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as

a)

an element

b)

a compound

c)

a homogeneous mixture

d)

a heterogeneous mixture

53.

Which formula represents a mixture?

a)

C6H12O6 (l)

b)

C6H12O6 (s)

c)

LiCl (aq)

d)

LiCl (s)

54.

Bronze contains 90 to 95 percent copper and 5 to 10 percent tin. Because these percentages can vary, bronze is classified as

a)

a compound

b)

an element

c)

a mixture

d)

a substance

55.

A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describe the resulting mixture?

a)

The mixture is homogeneous and can be separated by filtration.

b)

The mixture is homogeneous and cannot be separated by filtration.

c)

The mixture is heterogeneous and can be separated by filtration.

d)

The mixture is heterogeneous and cannot be separated by filtration.

56.

If a student pours a mixture of sand and salt water through a filter paper into a beaker, what will be found in the beaker after filtering?

a)

salt, only

b)

sand, only

c)

salt and water

d)

salt and sand

57.

Which solution has the highest boiling point at standard pressure?

a)

0.10 M KCl (aq)

b)

0.10 M K2SO4 (aq)

c)

0.10 M K3PO4 (aq)

d)

0.10 M KNO3 (aq)

58.

How do the boiling point and freezing point of a solution of water and calcium chloride at standard pressure compare to the boiling point and freezing point of water at standard pressure?

a)

Both the freezing point and boiling point of the solution are higher.

b)

Both the freezing point and boiling point of the solution are lower.

c)

The freezing point of the solution is higher and the boiling point of the solution is lower.

d)

The freezing point of the solution is lower and the boiling point of the solution is higher.

59.

Which concentration of a solution of CH3OH in water has the lowest freezing point?

a)

0.1 M

b)

0.01 M

c)

0.001 M

d)

0.0001 M

60.

What is the concentration of an aqueous solution that contains 1.5 moles of NaCl in 500 milliliters of this solution?

a)

0.30 M

b)

0.75 M

c)

3.0 M

d)

7.5 M

61.

What is the molarity of a solution that contains 0.500 mole of KNO3 dissolved in 0.500-liter of solution?

a)

1.00 M

b)

2.00 M

c)

0.500 M

d)

4.00 M

62.

Which expression could represent the concentration of a solution?

a)

3.5g

b)

3.5 M

c)

3.5 mL

d)

3.5 mol

63.

What is the molarity of 1.5 liters of an aqueous solution that

contains 52 grams of lithium fluoride, LiF, (gram-formula mass = 26 grams/mole)?

a)

1.3 M

b)

2.0 M

c)

3.0 M

d)

0.75 M

64.

How many total moles of KNO3 must be dissolved in water to make 1.5 liters of a 2.0 M solution?

a)

0.50 mol

b)

2.0 mol

c)

3.0 mol

d)

1.3 mol

65.

What is the molarity of a solution containing 20 grams of NaOH in 500 milliliters of solution?

a)

1 M

b)

2 M

c)

0.04 M

d)

0.5 M

66.

How many milliliters of 12.0 M HCl(aq) must be diluted with water to make exactly 500. mL of 3.00 M hydrochloric acid?

a)

100. mL

b)

125. mL

c)

200 mL

d)

250 mL

67.

A 20.-milliliter sample of 0.60 M HCl is diluted with water to a volume of 40. milliliters. What is the new concentration of the solution?

a)

0.15 M

b)

0.60 M

c)

0.30 M

d)

1.2 M

68.

A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million?

a)

5.0 ppm

b)

15 ppm

c)

20. ppm

d)

50. ppm

69.

Which unit can be used to express the concentration of a solution?

a)

L/s

b)

J/g

c)

ppm

d)

kPa

70.

What is the concentration of O2(g), in parts per million, in a solution that contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)?

a)

0.8 ppm

b)

8 ppm

c)

80 ppm

d)

800 ppm

71.

What is the concentration of a solution, in parts per million, if 0.02 gram of Na3PO4 is dissolved in 1000 grams of water?

a)

20 ppm

b)

2 ppm

c)

0.2 ppm

d)

0.02 ppm

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