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Review for Quarterly exam

Total questions: 40

Worksheet time: 1hrs 1mins

Name
Class
Date
1.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
2.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
3.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
4.
A saturated 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.
5.
A supersaturated 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.
6.
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.
7.
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.
8.
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.
9.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
10.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
11.
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
12.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)
9000
c)
9
d)
4000  moles NaCl
13.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

14.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

15.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

16.
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
17.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
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.
Which substance is SOLUBLE in water?
a)
sand
b)
oil
c)
salt (sodium chloride)
d)
sulfur
20.
Which substance is INSOLUBLE in water?
a)
salt (sodium chloride)
b)
sugar (sucrose)
c)
oil
d)
copper sulfate
21.
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.
22.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
23.
What is the molarity of 4 grams of sodium chloride (NaCl) in 3,800 mL of solution?
a)
0.018 M
b)
0.018 m
c)
1.052 M
d)
1.052 m
24.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.074 mol
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
25.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

26.

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

27.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

28.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

8.47 %

e)

11.8 %

29.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
30.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 liters of water?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.02 ppm

31.

Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following has hydrogen bonding?

a)

CBr4

b)

H2S

c)

NO2

d)

NH3

32.

Does HCl have hydrogen bonding?

a)

yes

b)

no

33.

Which is the second strongest intermolecular force, after hydrogen bonding?

a)

ion - dipole

b)

dipole - dipole

c)

Hydrogen bonding

d)

dispersion forces

34.

All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London forces?

a)

I2

b)

OCl2

c)

NH3

d)

SH2

35.

Which substance would have the weakest intermolecular forces of attraction?

a)

MgF2

b)

NaCl

c)

CH4

d)

H2O

36.

________________________ have the strongest intermolecular forces of attraction.

a)

Ion - dipole

b)

Dipole - dipole

c)

London dispersion

d)

Hydrogen bonding

37.

Intermolecular forces for: NH3

a)

ion - dipole

b)

hydrogen bonding

c)

dipole - dipole

d)

London dipersion

38.

Intermolecular forces for: CO2

a)

ion - dipole

b)

hydrogen bonding

c)

dipole - dipole

d)

London dispersion

39.

Crystalline solids contain particles that are arranged and organized in a specific location.

a)

Trot

b)

Charot

40.

The particle in amorphous solids are put together in random and they form in a short span of time

a)

Trot

b)

Charot

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