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Classwork Formation of Solution

Total questions: 97

Worksheet time: 4hrs 41mins

Name
Class
Date
1.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
2.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
3.
In the above 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
4.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
5.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
6.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
7.
When Koolaid mix is light colored and tastes watery it is a _______ solution.
a)
saturated 
b)
diluted
8.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
9.
To make a solute dissolve more quickly i n a solvent which would you do?
a)
Put it in cold water and stir it
b)
Put it in warm water and stir it
10.
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
11.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
12.
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
13.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
14.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
15.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
16.
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
17.
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
18.

Which of the following actions will NOT

increase the rate of dissolution

(dissolving)?

a)

Stirring the solution

b)

Decreasing the temperature

c)

Increasing the surface area of the

solute

d)

Increasing the temperature

19.

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

20.

How do you know when you have a saturated solution?

a)

You don't see anymore material in the solution. It has dissolved.

b)

The material dissolves and no more will dissolve because you see it collect at the bottom.

c)

The solution is bubbling and cloudy.

d)

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

21.

Which 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

22.

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.

23.

A solution that contains all of the solute it can hold at a given temperature is

a)

diluted.

b)

saturated.

c)

supersaturated.

d)

unsaturated.

24.

The amount of solute that can be dissolved in a specific amount of solvent at a given temperature is its

a)

concentration.

b)

density.

c)

dilution.

d)

solubility.

25.

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 number of sugar molecules.

d)

It has the fewest bonds between sugar modules.

26.

A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?

a)

As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.

b)

Water molecules, trapped with the KCl crystals, were released after heating.

c)

At lower temperatures the solubility of KCl decreased and recrystallization occurred.

d)

At increased temperatures the solubility of KCl increased and remained too high after cooling.

27.

A student pours mineral salts into a bottle of cold water. Which of the following best explains why shaking the bottle will affect the dissolving rate of the salt?

a)

Shaking exposes the salts to the solvent more quickly.

b)

Shaking helps more water evaporate.

c)

Shaking equalizes the water temperature.

d)

Shaking causes more ions to precipitate out of solution.

28.

Students in Ms. Alvarez’s science class are investigating how temperature, in degrees Celsius (C), affects the solubility of a compound in 100 milliliters (mL) of water. Ms. Alvarez provides the students with a graph that shows the solubility of a certain compound, as shown below.


She then tell the students that she will demonstrate how many grams (g) of the compound will dissolve in 100 mL of water at 40 C. Based on the information in the graph, which of the following is the best prediction of how many grams of the compound will dissolve at 40 C?

a)

40 g

b)

65 g

c)

85 g

d)

100 g

29.

The solubility graph below shows the amounts of four substances that will dissolve in 100 grams of water at various water temperatures.


Which substance has 80 grams of solute dissolved in 100 grams of water at 50 C?

a)

Potassium Bromide

b)

Ammonium Chloride

c)

Potassium Chloride

d)

Lithium Hydroxide

30.

A solution that is able to dissolve additional solute is best described as

a)

supersaturated.

b)

concentrated.

c)

saturated

d)

unsaturated.

31.
The _____is the part that gets dissolved. 
a)
solute 
b)
solvent 
c)
solution 
d)
Sacajawea 
32.
A solution is a kind of ________. 
a)
mixture 
b)
compound 
c)
element 
d)
stuff 
33.
A solution is a ________ mixture. 
a)
heterogeneous 
b)
homogeneous 
c)
dumb 
d)
mixed 
34.
The universal solvent is ______. 
a)
sodium 
b)
acid 
c)
water 
d)
wind 
35.
This is the part of the solution that does the dissolving. 
a)
solute
b)
solvent 
c)
salt water 
d)
First Continental Congress 
36.
Solubility is a ________ property. 
a)
neat 
b)
chemical 
c)
physical 
d)
an organic 
37.
Which of the following is a heterogeneous mixture
a)
water
b)
Salt dissolved in water
c)
chex mix
d)
air
38.
Which of the following does not increase the rate of dissolving a solid in a liquid?
a)
stirring the solution
b)
crushing up the solute
c)
raising the temperature of the water
d)
lowering the temperature of the water
39.
Why will sugar dissolve in water?
a)
sugar is ionic
b)
sugar has a similar polarity to water
c)
sugar will not dissolve in water
d)
sugar has similar energy to water
40.
Calculate the molarity of a solution prepared by dissolving 78.2 grams of CaCl2 in 500.0mls of water
a)
0.156 M
b)
0.709 M
c)
0.353 M
d)
1.41 M
41.
How many grams of ammonium chloride are needed to make a saturated solution at 80o C?
a)
50 grams
b)
80 grams
c)
65 grams
d)
75 grams
42.
At 40oC which salt is least soluble?
a)
KClO3
b)
NaCl
c)
KI
d)
KNO3
43.
What kind of solution is made from 50 grams of KNO3 at 40oC?
a)
saturated
b)
unsaturated
c)
supersaturated
44.
Which will dissolve the slowest
a)
powdered sugar in hot water
b)
Powdered sugar in cold water
c)
sugar cubes in hot water
d)
sugar cubes in cold water
45.
Which of the following solutions made from one mole of the following solutes in 100.0 mls of water has the lowest freezing point?
a)
MgBr2
b)
Al2(CO3)3
c)
NH4C2H3O2
d)
N2O4
46.
A metal solution is a(n)
a)
colloid
b)
suspension
c)
alloy
d)
heterogeneous mixture
47.
As the pressure decreases the solubility of a gas in a liquid
a)
increases
b)
decreases
48.
What mass of NaCl is needed to prepare 850 mls of 6.0 M NaCl solution?
a)
5.1 grams
b)
0.087 grams
c)
87 grams
d)
298 grams
49.
Which of the following has components in a uniform arrangement?
a)
Heterogeneous mixture
b)
Colloids
c)
Suspensions
d)
Solutions
50.
What is the molarity of  420 mls of a KCl solution that contains 16.0 grams of KCl
a)
625 M
b)
0.51 M
c)
3.19 M
d)
0.00563 M
51.
How much of the 12.0 M stock solution do you need to prepare 250 mls of .20M HCl?
a)
15,000 mls
b)
4.17 mls
c)
9.6 mls
d)
0.0096 mls
52.
Which of these is a colloid?
a)
paint
b)
salt water
c)
air
d)
gasoline
53.
If the amount of solute present in a solution is more than the maximum than can be dissolved, the solution is
a)
saturated
b)
unsaturated
c)
supersaturated
d)
colloidal
54.
The Tyndall effect is used to distinguish between 
a)
gases and solids
b)
solutions and colloids
c)
solvent and suspensions
d)
all of these 
55.
Which of the following will produce crystals if disturbed?
a)
 saturated solutions
b)
colloids
c)
supersaturated solutions
d)
unsaturated solutions
56.

Carbonated water is a mixture of carbon dioxide gas and water. Identify the solute.

a)

water

b)

carbon dioxide

c)

there is no solute in carbonated water

57.

Air is a mixture composed of about 78% nitrogen, 21% oxygen less than 1% argon and many trace gases. Identify the solvent in air.

a)

argon

b)

oxygen

c)

nitrogen

d)

trace gases

58.

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

a)

electrolytes; ionic

b)

nonelectrolytes; ionic

c)

electrolytes; molecular

d)

electrolytes; covalent

59.
Oil molecules are nonpolar. What kind of solvent is required to remove an oil stain?
a)
saturated
b)
unsaturated
c)
polar
d)
nonpolar
60.

Which of the following has the MOST surface area?

a)

A single 5 gram ice cube

b)

5 grams of crushed ice

c)

5 grams of shaved ice

61.

You begin with a solution of 400 grams of potassium chloride dissolved in 1250 mL of water. If the volume of water is increased by 33%, what is the final molarity of the solution?

a)

3.2 M

b)

4.3 M

c)

5400 M

d)

5.4 M

62.

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

63.
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.
64.

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

65.
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
66.
A dissolved solute that does not form ions is:
a)
a nonelectrolyte
b)
a weak electrolyte
c)
a strong electrolyte
d)
insoluble
67.
How does temperature affect solubility?
a)
Solubility is not affected by temperature.
b)
Solubility decreases with an increase in temperature.
c)
Solubility increases with an increase in temperature.
68.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
69.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
70.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
71.
Which of the following is an electrolyte?
a)
sodium chloride
b)
sugar
c)
water
72.
Solutions in which electric currents cannot run through are said to be
a)
noncolloidal
b)
electrolytes
c)
nonelectrolytes
d)
conductors
73.
An example of a nonelectrolyte is
a)
sugar water
b)
salt water
c)
sodium chloride
d)
hydrogen chloride
74.

The drawings below represent beakers of aqueous solutions. Each o represents a dissolved solute particles.Which solution is most concentrated?

a)

A

b)

B

c)

C

d)

D

e)

E

75.

The drawings below represent beakers of aqueous solutions. Each o represents a dissolved solute particle.Which solution is least concentrated?

a)

A

b)

B

c)

C

d)

E

e)

F

76.

Which two solutions have the same concentration?

a)

A & D

b)

A & E

c)

C & E

d)

F & C

e)

B & E

77.

When Solutions E and F are combined, the resulting solution has the same concentration as Solution _____.

a)

A

b)

B

c)

C

d)

D

e)

F

78.

When Solutions B and E are combined, the resulting solution has the same concentration as Solution _____.

a)

A

b)

B

c)

C

d)

D

e)

E

79.

If you evaporate off half of the water in Solution B, the resulting solution has the same concentration as Solution _____.

a)

A

b)

B

c)

C

d)

D

e)

F

80.

In a chromatography experiment using water as the solvent, the solute that would have the highest Rf value would be:

a)

polar

b)

nonpolar

81.
When no more sugar will dissolve in a glass of water, the solution is...
a)
unsaturated
b)
saturated
c)
supersaturated
82.
According to the table which solute is nonpolar.
a)
ammonium chloride
b)
naphthalene
c)
ethanol
d)
urea
83.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH - molar mass 40 g/mol)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

84.

You place electrodes in a solution and this happens! This solution must be:

a)

electrolyte & ionic bond

b)

electrolyte & covalent bond

c)

nonelectrolyte & ionic bond

d)

nonelectrolyte & ionic bond

85.
If the saturated solution of K2Cr2O7 was cooled from 80 to 60 oC, how much solute would fall out? 
a)
20 g
b)
40 g
c)
15 g 
d)
30 g
86.
Which of the following bonds are soluble in water?
a)
polar & nonpolar covalent
b)
polar covalent & ionic
c)
nonpolar covalent & ionic
d)
Only ionic
87.

Calculate the molarity of 25.0 grams of KBr dissolved in 0.75 L (hint: find moles: convert grams to mol)

a)

0.280 M

b)

0.210 M

c)

33.3 M

88.
How many moles of solution will result when 15.0 L of H2SO4 is used to make a 0.20 M solution?
a)
75 moles
b)
7 moles
c)
3 moles
d)
0.013 moles
89.
Convert 3000 mL into L.
a)
3000 L
b)
300 L
c)
30 L
d)
3 L
90.
 In a Hydrogen bond the slightly positive hydrogen in water is attracted to:
a)
positive ions
b)
negative ions
91.
What is the molarity of a solution containing 8.0 moles of solute in 500 mL of solution?
a)
0.016 M
b)
16 M
c)
62.5 M
d)
0.063 M
92.
You place electrodes in a solution and this happens! The solution must be:
a)
nonelectrolyte & covalent bond
b)
nonelectrolyte & ionic bond
c)
electrolyte & covalent bond
d)
electrolyte & ionic bond
93.
Which solution is more concentrated?
a)
1 mole of solute in 1 liter of solvent
b)
3 moles of solute in 6 liters of solvent
c)
4 moles of solute in 2 liters of solvent
94.

What is molarity?

a)

a concentration unit, defined to be number of atoms per moles of water

b)

a concentration unit, defined to be the number of moles of solute divided by the number of liters of solution.

c)

a conversion factor, used to change moles to grams

d)

a conversion factor, used to change milliliters to liters

95.
What volume of 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
96.

125.0 mL of 2.00 M calcium hydroxide solution is diluted to a concentration of 1.50 M. How many mL of water was added to the original volume?

a)

167 mL

b)

42.0 mL

c)

93.8 mL

d)

0.0240 mL

97.

How many liters 0.110 M nitric acid can be prepared by diluting 5.00 mL of 15.3 M stock solution?

a)

1530 mL

b)

1.53 L

c)

0.0654L

d)

0.153 L

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