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Solutions

Total questions: 48

Worksheet time: 2hrs 52mins

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.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
4.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
5.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
6.

Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.

a)

Mean

b)

Range

c)

Amount

d)

Mode

7.
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
8.
What is the correct formula to solve for the Molarity of a solution that has .4 moles of HCl in 9.5 L of solution?
a)
M = 9.5 L / .4 mol
b)
M1V1=M2V2
c)
M = .4 mol / 9.5 L
d)
none of the other choices
9.
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
10.
A questions asks, "what volume of 0.125 M KMnO4 is required to yield 0.180 mol of potassium permanganate,
KMnO4?"  What is the correct formula set up to solve for this problem?
a)
.125 M = .180 mol / L
b)
M1 V1 = M2 V2
c)
.125 M = L / .180 mol
d)
none of the choices listed
11.
Which formula should you use to convert 2.00 L of 0.300 M sulfuric acid, how many mL of a 1.00 M stock solution should be
used?
a)
molarity formula
b)
dilution formula
c)
both will work
d)
neither will work
12.
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
13.
Which of the following would decrease the rate of solution when dissolving a solid in water?
a)
Raise the temperature of the solution
b)
Crush the solid before mixing
c)
Stir the solution after mixing
d)
Use a single cube of solid
14.

NaNO3 soluble (aq) or insoluble (s)?

a)

Soluble (aq)

b)

Insoluble (s)

15.

MgF2 soluble (aq) or insoluble (s)?

a)

Soluble (aq)

b)

Insoluble (s)

16.

PbF2 soluble (aq) or insoluble (s)?

a)

Soluble (aq)

b)

Insoluble (s)

17.

CuCl2 soluble (aq) or insoluble (s)?

a)

Soluble (aq)

b)

Insoluble (s)

18.

* What is the precipitate (solid) of this reaction?

MgCl2 + 2 NaOH --> Mg(OH)2 + 2 NaCl

a)

MgCl2

b)

NaOH

c)

Mg(OH)2

d)

NaCl

19.

* What is the precipitate (solid) of this reaction?

Na2O + NiF2 --> 2 NaF + NiO

a)

Na2O

b)

NiF2

c)

NaF

d)

NiO

20.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
21.
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. 
22.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
23.

When the solution equilibrium point is reached and no more solute will dissolve, the solution is said to be _________.

a)

unsaturated

b)

saturated

c)

supersaturated

24.

Which of the following statements is true?

a)

B is a saturated solution

b)

A is a supersaturated solution

c)

C is an unsaturated solution

d)

None of the above

25.

What do you call a solution that contains less than the maximum amount of solute that is capable of being dissolved?

a)

unsaturated solution

b)

saturated solution

c)

supersaturated solution

d)

insoluble solution

26.
What does "polar" mean?
a)
A molecule is cold
b)
A molecule has ionic bonds
c)
A molecule has covalent bonds
d)
A molecule has areas of positive and negative charge
27.
This atom in a water molecule has more of a negative charge
a)
Oxygen
b)
Hydrogen
28.
Salt dissolves in water because
a)
The water molecules wiggle between the Na and Cl atoms
b)
Water gets warm and moves around too much
c)
The polar areas of water molecules stick to the Na and CL ions
29.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

a)

50 ml

b)

1.3 ml

c)

30 ml

d)

130 ml

30.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
31.

The term molar which is used to describe a solution's concentration, is written as?

a)

M

b)

mol

c)

g

d)

g/L

32.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
33.

If you have 34 mL of a 0.5 M NaBr solution, what will the concentration be if 56 mL of water is added to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

34.

The units "M" can also be written as:

a)

mol/L

b)

moles

c)

g/L

d)

g/mol

35.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

36.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

37.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

38.

Phase change going from Liquid to Solid...

a)

Melting

b)

Freezing

c)

Condensation

d)

Sublimation

39.

Phase change going from a Solid to a Liquid...

a)

Freezing

b)

Condensation

c)

Melting

d)

Sublimation

40.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
41.
7. All phase changes (changing states) requires energy to be added or taken away.
a)
True
b)
False
42.
What happens to particles when they are heated?
a)
They speed up and spread out
b)
They slow down and compress
c)
They stop moving
d)
They move closer together and speed up
43.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
44.
How are solids different from liquids?
a)
particles in solids are moving freely around each other.
b)
particles in solids have no motion.
c)
particles in solids are vibrating in place.
d)
particles in solids have more motion than in liquids
45.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
46.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
47.
Which state of matter has molecules that slide past each other but stay close together? They do not form a regular pattern.
a)
solid
b)
liquid
c)
gas
48.
Molecules are closest together in a 
a)
Solid
b)
Liquid
c)
Gas

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