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Unit 14: Solutions

Total questions: 79

Worksheet time: 2hrs 1mins

Name
Class
Date
1.

In the picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
2.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
3.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
4.

To make sugar solute dissolve more quickly in water, which would you do?

a)

Put it in cold water

b)

Put it in warm water

c)

Increase the pressure

d)

Decrease the pressure

5.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
6.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
c)

Supersaturated

d)

Concentrated

e)

Unsaturated

7.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
8.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
9.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
10.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
11.
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
12.

Which of the following actions will NOT increase the rate of dissolution?

(multiple answers)

a)

Stirring the solution

b)

Decreasing the temperature

c)

Increasing the surface area of the

solute

d)

Increasing the temperature

e)

Decreasing the surface area of the

solute

13.

You are given a small beaker of solution at room temp. You add a bit of solute to the solution and it dissolves. The solution was:

a)

saturated

b)

unsaturated

c)

concentrated

d)

warm

14.

How do you know when you have a saturated solution?

a)

Solute dissolves and you don't see anymore in the solution.

b)

Solute dissolves and you see some collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

The solution is clear and there is nothing at the bottom.

15.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

16.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

17.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
18.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
19.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
20.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
21.
A nonelectrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
22.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
23.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)

9000 moles NaCl

c)

.0002 moles NaCl

d)
4000  moles NaCl
24.
Solubility is defined as
a)
the ability to catch on fire
b)
the ability to be dissolved
c)
the ability to fly.
d)
the ability to get on Mrs. D's nerves.
25.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
26.

Identify the solute in Lemonade - it contains water, lemon juice, and sugar

a)

water

b)

lemon juice

c)

sugar and lemon juice

27.

If we heat a sample of water, then the amount of oxygen dissolved will increase.

a)

true

b)

false

28.

A common gas that we find dissolved in coca cola is

a)

krypton

b)

neon

c)

oxygen

d)

carbon dioxide

29.

If I want more sugar to dissolve in a saturated solution of water, I should heat the water

a)

true

b)

false

30.

If I want more salt to dissolve in a saturated solution of salt water, I should stir the water

a)

true

b)

false

31.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
32.

A sample of 0.0255 mol potassium hydroxide, KOH, was dissolved in water to yield 10.0 mL of solution.  Which amount would you need to change to solve for molarity?

a)
change .0255 moles to grams
b)
change 10 mL to L
c)
change both values to grams and L
d)
leave it as it is
33.

Which of the following would result in being able to dissolve a greater amount of gas in a solution?

a)
Heat the gas and solution
b)
Decrease the pressure of the solution
c)
Make the gas an electrolyte
d)
Cool the gas and solution
34.
90 grams of sodium nitrate (NaNO3) are put into 100 grams of water and stirred. The final
mixture has a temperature of 20°C. About how many grams of the sodium nitrate dissolved?
a)
23
b)
73
c)
80
d)
88
35.
Which of the following is the best way to determine if an aqueous solution  is supersaturated?
a)
add more solvent
b)
measure the temperature
c)
filter out excess solute
d)
add a seed crystal
e)

solid at the bottom of the solution

36.

State whether the following compound is soluble or insoluble in water:

calcium carbonate, CaCO3 

a)
soluble
b)
insoluble
37.

State whether the following compound is soluble or insoluble in water:

potassiun bromide, KBr

a)
Soluble
b)
Insoluble
38.

State whether the following compound is soluble or insoluble in water:

zinc hydroxide, Zn(OH)2

a)
Soluble 
b)
Insoluble
39.

State whether the following compound is soluble or insoluble in water:

iron(II) sulfide, FeS

a)
soluble
b)
insoluble
40.

State whether the following compound is soluble or insoluble in water:

silver iodide, AgI

a)
Soluble 
b)
Insoluble 
41.

State whether the following compound is soluble or insoluble in water:

zinc carbonate, ZnCO3 

a)
Soluble 
b)
Insoluble 
42.

State whether the following compound is soluble or insoluble in water:

barium sulfate, BaSO4

a)
soluble
b)
insoluble
43.

State whether the following compound is soluble or insoluble in water:

sodium nitrate, NaNO3

a)
soluble
b)
insoluble
44.

State whether the following compound is soluble or insoluble in water:

lead (II) nitrate, PbNO3

a)
soluble
b)
insoluble
45.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

46.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

47.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

48.

What type of a solution is 55g KCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

49.

What type of a solution is 25g NaCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

50.
Which of the following is an electrolyte?
a)

ammonium hydroxide

b)
sugar
c)

acetone

d)

ammonia

51.

What is the molarity of 4 g of NaCl in 3,800 mL of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

52.

You have been asked to prepare 500 mL of a 2.5 M solution of NaOH. How much NaOH should you measure out before adding water?

a)

10g

b)

100g

c)

50g

d)

80g

53.

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

a)

electrolytes; ionic

b)

nonelectrolytes; ionic

c)

electrolytes; molecular

d)

electrolytes; covalent

54.
Oil molecules are nonpolar. What kind of solvent is required to remove an oil stain?
a)
saturated
b)
unsaturated
c)
polar
d)
nonpolar
55.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
56.

You and your friend have a contest to see who can make sweet iced tea the fastest. Which of the following would NOT help you win?

a)

Cooling the water

b)

Using smaller sugar crystals

c)

Heating the water

d)

Stirring quickly

57.

The amount of solute that can dissolve in a given amount of solvent at a given temperature is...

a)
saturated solution
b)
solubility
c)

homogeneous

d)

heterogeneous

58.
What is the most common solvent in everyday life?
a)
Ethanol
b)
Tuluene
c)
Water
d)
Oils
59.
A dissolved solute that does not form ions is:
a)

a nonelectrolyte and is covalent

b)

a weak electrolyte and is covalent

c)

a strong electrolyte and is ionic

d)

a nonelectrolyte and is ionic

60.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
61.

Which solution of sodium hydroxide (NaOH) is the least concentrated?

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

62.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
63.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
64.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
65.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

66.

The vapor pressure of a pure solvent is ___________ that of a solution

a)

more than

b)

less than

c)

equal to

67.

Which one of the following diagrams has the lowest vapor pressure?

a)

1

b)

2

c)

3

d)

4

e)

5

68.

Compared to the freezing point and boiling point of water at 1 atmosphere, a solution of a salt and water at 1 atmosphere has a

a)

lower freezing point and a lower boiling point

b)

lower freezing point and a higher boiling point

c)

higher freezing point and a lower boiling point

d)

higher freezing point and a higher boiling point

69.

Which one of the following diagrams has the highest boiling point?

a)

1

b)

2

c)

3

d)

4

e)

5

70.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

71.

Three 10 g samples of sugar are represented below.


Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

a)

It has the most volume.

b)

It has the smallest surface area.

c)

It has the largest surface area.

d)

It has the fewest bonds between sugar modules.

72.
The "like dissolves like" rule is the reason why water cannot dissolve
a)
salt
b)
sugar
c)
vinegar
d)
oil
73.

Based on the solubility curve, how many grams of sugar will dissolve in a 100 mL of water at 20°C?

a)

100 g

b)

150 g

c)

200 g

d)

250 g

74.

Which substance is MOST soluble at 90 ºC?

a)

Solid A

b)

Solid B

c)

Solid C

75.

How many moles of HNO3 would be needed to react with 85 mL of 0.75 M KOH?

a)

110 mol

b)

1.1 mol

c)

.11mol

d)

0.064 mol

e)

64 mol

76.

What is the theoretical yield of lead(II) chloride, in grams, if 250.0 mL of 1.75 M sodium chloride reacts with excess lead(II) nitrate?

2 NaCl (aq) + Pb(NO3)2 (aq) --> PbCl2 (s) + 2 NaNO3 (aq)

a)

78.5 g

b)

93.1 g

c)

45.5 g

d)

60.8 g

e)

59.4 g

77.

How many milliliters of 2.4 M H3PO4 solution are needed to react with 45 g Zn?

(2 H3PO4 + 3 Zn --> Zn3(PO4)2 + 3 H2)

a)

2400 mL

b)

190 mL

c)

290 mL

d)

1700 mL

78.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
79.

A dilution is when

a)

solute is added to the volume of stock solution

b)

water is added to the volume of stock solution

c)

solute is removed from the volume of stock solution

d)

water is removed from the volume of stock solution

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