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CHEM: Solubility

Total questions: 133

Worksheet time: 4hrs 36mins

Name
Class
Date
1.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a solvent in it. 
2.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Mixture
d)
Homogeneous solution
3.
Describe a solute.
a)
part of solution present in largest amount
b)
gets dissolved
c)
water
d)
surrounds and breaks apart
4.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
5.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
6.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
7.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
8.
What is able to dissolve other substances?
a)
Solute
b)
Salt
c)
Suspension
d)
Solvent
9.

What is a solvent

a)

A liquid that will dissolve a solid solute

b)

Another word for solution

c)

A thing that make drinks change colour

d)

Usually the solid about to be dissolved

10.

What is Solubility?

a)

If something dissolves in water

b)

If something sinks in water

c)

If something floats in water

d)

None of the above

11.

Salt has Solubility because it dissolves in water.

a)

True

b)

False

12.

Which answer does NOT have solubility?

a)

sugar

b)

salt

c)

oil

13.

Which answer is Soluble in water?

a)

rocks

b)

honey

c)

pepper

d)

marbles

14.

A homogeneous mixture is the same thing as...

a)

a solution

b)

a heterogeneous mixture

c)

a compound

d)

an element

15.

The prefix hetero means...

a)

same

b)

different

c)

together

d)

awesome

16.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
17.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

18.

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

a)

300 grams

b)

250 grams

c)

100 grams

d)

50 grams

19.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

20.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
21.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
22.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
23.
A solution of potassium chlorate, KClO3, has 20 grams of the salt dissolved in 100 grams of water at 70 ºC. Approximately how many more grams of the salt can be added to the solution before reaching the saturation point?
a)
10 grams
b)
30 grams
c)
80 grams
d)
60 grams 
24.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

55 g

d)

33 g

25.
What will allow more solute to be dissolved in a solvent.
a)
adding more solute
b)
stiring
c)
cooling solution
d)
heat
26.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

27.

At 80'C, KBr's solubility is:

a)

100

b)

90

c)

80

d)

0

28.

Determine the solubility for the substances at 55'C and arrange them in order from lowest to highest solubility.

a)

NaCl, NH4Cl, KBr, NaNO3

b)

NaCl, NH4Cl, NaNO3, KBr

c)

NH4Cl, NaCl, NaNO3, KBr

d)

NaNO3, KBr, NH4Cl, NaCl

29.

At 10'C, NaNO3's solubility is 80 g/100 g of H2O. Based on this information, what would the solubility be in 50 g of H2O.

a)

40

b)

80

c)

160

d)

16

30.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

31.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

60 g

d)

33 g

32.

Water becomes __________ changing from a solid to a liquid

a)

more dense & more kinetically chaged

b)

less dense & less kinetically charged

c)

more dense & less kinetically charged

d)

less dense & more kinetically charged

33.

Identify a method to decrease the dissolving rate of a solution:

a)

decrease the temperature

b)

add KE

c)

stir the solution

d)

increase the temperature

34.
Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.
a)
Volume
b)
Proportion
c)
Mass
d)
Particles
35.
An ______ is a compound that breaks apart in water, forming charged particles (ions) that can conduct electricity.
a)
electrolyte
b)
nonelectrolyte
c)
polar molecule
d)
non polar molecule
36.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
37.

Which of the following would NOT increase the rate at which a sugar cube dissolves?

a)

Reducing the amount of solvent

b)

Crushing the sugar cube

c)

Stirring the solution

d)

Heating the solvent

38.

You can make a solute dissolve more quickly in a solvent by

a)

adding more solute.

b)

adding ice.

c)

heating the solvent.

d)

removing some solvent.

39.

When you measure how fast a solute dissolves, you are measuring the

a)

amount of dissolving

b)

rate of particle movement

c)

amount of particle movement

d)

rate of solubility

40.

Which of the following does not affect the solubility of a solute in a solvent?

a)

The rate of stirring

b)

The size of the solute

c)

The temperature of the solvent

d)

The amount of the colloid added

41.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
42.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
43.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
44.
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
45.
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
46.
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
47.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
48.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
49.
State whether the following compound is soluble or insoluble.  calcium carbonate CaCO3 
a)
soluble
b)
insoluble
50.
State whether the following compound is soluble or insoluble. potassiun bromide KBr
a)
Soluble
b)
Insoluble
51.
State whether the following compound is soluble or insoluble. Zinc hydroxide Zn(OH)2
a)
Soluble 
b)
Insoluble
52.
State whether the following compound is soluble or insoluble. Silver iodide AgI
a)
Soluble 
b)
Insoluble 
53.
State whether the following compound is soluble or insoluble.Potassium hydroxide KOH
a)
Soluble 
b)
Insoluble
54.
State whether the following compound is soluble or insoluble.Silver acetate AgC2H3O2
a)
Soluble 
b)
Insoluble
55.
State whether the following compound is soluble or insoluble.nickel chloride NiCl2
a)
Soluble 
b)
Insoluble
56.
State whether the following compound is soluble or insoluble.Lead iodide PbI2
a)
Soluble
b)
Insoluble
57.
State whether the following compound is soluble or insoluble.Barium chloride BaCl2
a)
soluble
b)
insoluble
58.
State whether the following compound is soluble or insoluble.Ammonium nitrate NH4NO3
a)
soluble
b)
insoluble
59.
State whether the following compound is soluble or insoluble.sodium nitrate NaNO3
a)
soluble
b)
insoluble
60.
State whether the following compound is soluble or insoluble. barium sulfate BaSO4
a)
soluble
b)
insoluble
61.
State whether the following compound is soluble or insoluble.lead nitrate PbNO3
a)
soluble
b)
insoluble
62.

Which of the following describes: Dissolved particles are distributed evenly and you can no longer see them.

a)

conductivity

b)

solution

c)

mixture

63.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
64.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

65.

What type of a solution is 260g sugar at 50ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

66.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
67.

When a substance partially dissolves in a liquid, but some particles remain, which type of solubility is that known as?

a)

High Solubility

b)

Low Solubility

c)

No Solubility

68.

When the volume of solvent increases, the solubility of a solute at a given temperature...

a)

increases

b)

decreases

c)

stays the same

69.

When the volume of solvent increases, the mass of solute that can dissolve in a saturated solution...

a)

increases

b)

decreases

c)

stays the same

70.

In general as temperature decreases, the solubility...

a)

increases

b)

decreases

c)

stays the same

71.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
72.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
73.

Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.5 L of solution

a)

1.5

b)

0.33 M

c)

30 M

d)

3 M

74.

Water is called the ___________ _____________

a)

universal solute

b)

universal solvent

c)

universal solution

75.

Substances that dissolve in water are _____________, which means " water loving"

a)

hydrophobic

b)

hydrophilic

c)

hyperactive

76.

Substances that do not dissolve in water are called ________, which means " water fearing"

a)

hydrophilic

b)

hydrofearic

c)

hydrophobic

77.

Concentration of a solution can be expressed as a ratio :

a)

C = M / M

b)

C = V / M

c)

C = M / V

78.

Mass of a solute is measured in ________

a)

liters

b)

mL

c)

grams

79.

Volume of a liquid solution can be measured in ________

a)

grams

b)

moles

c)

liters

80.

A containers holds 2 grams of solute and 4 mL of solvent. What is the concentration of the solution ?

a)

.125 g/mL

b)

.25 g/mL

c)

.50 g m/L

81.

What is the concentration of a solution that has 4 g of sugar and 2 mL of water ?

a)

2 g/L

b)

4 g/L

c)

8 g/ L

82.

Solution A has a concentration of .4 g / L and solution B has a concentration of .9 g/L . Which solution has a higher concentration?

a)

solution A

b)

solution B

83.

__________ is a measure of how easy a substance dissolves into another substance.

a)

evaporation

b)

concentration

c)

solubility

84.

Solubility is measured in _____ of solute per ________ mL of water

a)

liters, 100

b)

grams, 100

c)

grams, 1

85.

A substance with _______ solubility will dissolve ________ solute in 100 mL of water than a substance with _______ solubility

a)

low, more, high

b)

high, less, more

c)

high, more, less

86.

When mixing substances with different densities , substances with _________densities sink to the bottom .

a)

higher

b)

lower

c)

neither they will be equal

87.

Container A has 20 grams of sugar and 100 mL of water. Container B has 30 grams of sugar and 200 mL of water. What is Concentration of both containers?

a)

A= .8 g/mL , B= .9 g/mL

b)

A= .4 g/mL , B=8 g/mL

c)

A= .2 g/mL , B= .15 g/mL

88.

The X axis of this solubility graph shows what variable ?

a)

saturation

b)

grams

c)

temperature

89.

The Y axis of this graph shows what variable ?

a)

temperature

b)

celcius

c)

solubility rate

90.

What compound's solubility rate shows to be constant as temperature increases?

a)

BaNo32

b)

Na2So4

c)

NaCL

91.

What compound's solubility rate shows to be constant as temperature increases?

a)

BaNo32

b)

Na2So4

c)

NaCL

92.

How many grams of NaCl are required for the solution to become saturated at 10°C?

a)

37 g

b)

70 g

c)

50 g

d)

25 g

93.

How many grams of ammonium chloride (NH4Cl) will dissolve at 90°C?

a)

38 g

b)

70 g

c)

100 g

d)

15 g

94.

Which factor affecting solubility is shown in the picture?

a)

temperature

b)

height

c)

stirring

d)

particle size

95.

Which factor is shown in the picture?

a)

temperature

b)

particle size

c)

stirring

d)

use of spoon

96.

Why do sugar particles dissolve faster in hot water?

a)

water particles move slow

b)

water particles move fast

c)

water particles settle down

d)

water particles stay on top

97.

What are the factors that affect solubility?

a)

rate of stirring

b)

particle size

c)

temperature

d)

all of these

98.

Which of the following does not affect solubility of solutes?

a)

Tempearture

b)

Color

c)

Size particles

d)

Kind of solute

99.

Which will dissolve faster crushed table salt or crystal of table salt?

a)

crushed table salt

b)

crystal of table salt

100.

What would dissolve most slowly?

a)

Large crystals in stirred water

b)

Large crystals in unstirred water

c)

Small crystals in stirred water

d)

Small crystals in unstirred water

101.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

102.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

103.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
104.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

105.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
106.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
107.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

108.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

109.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

110.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

111.

What are the units of molality?

a)

M

b)

m

c)

Ml

d)

Mr

112.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

113.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

114.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

115.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

116.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

117.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
118.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
119.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
120.

suppose a hydrochloric acid solution contains 36 g of HCl and 64 g of H2O.what is the mole fraction of HCl?

a)

0.78

b)

0.99

c)

0.22

d)

3.6

121.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

122.

What is the mass of 0.75 moles of (NH4)3PO4? (Ar: N=14, H=1,P=31, 0=16)

a)

101.75 g

b)

121.75 g

c)

111.75 g

d)

131.75 g

123.

What is the molarity in 650. ml of solution containing 63 grams of sodium chloride, NaCl?

a)

2.4 M

b)

0.86 M

c)

1.657 M

d)

0.541 M

124.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
125.

What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?

a)

a. 2.4 M

b)

b. 0.54 M

c)

c. 0.86 M

d)

d. 1.7 M

126.

A beaker contain 795 mL of 0.35M of Na2SO4 solution. Calculate the mass of Na2SO4.

a)

39.55 g

b)

40.00 g

c)

39.05 g

d)

39.5 g

127.

A 40mL, 0.25 mol L−1 HCl solution is mixed with 15mL, 0.6 mol L−1 H2SO4 solution. Calculate the concentration of H+ ion in the combined solution.

a)

0.49 M

b)

0.50 M

c)

0.60 M

d)

0.51 M

128.

The density of aqueous solution containing 10% of ethanol, C2H5OH by mass is 0.984 gmL-1. Calculate its molality.

a)

2.314m

b)

2.251m

c)

2.415m

d)

2.154m

129.

Calculate the molality of 3.0 mol dm-3 sucrose, C12H22O11 if the density of the solution is 1.35 g cm-3.

a)

9.26 m

b)

9.20 m

c)

9.19 m

d)

9.23 m

130.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
131.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
132.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
133.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL

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