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Unit 4 Exam Review

Total questions: 43

Worksheet time: 3hrs 29mins

Name
Class
Date
1.

A solution that has water as the solvent is called a(n).....

a)

Aqueous Solution

b)

Water-Based Solution

c)

Organic Solution

d)

Dilute Solution

2.

What is the molarity of a solution containing 400 g of CuSO4 (FM: 159.6 g/mol) in 4.0 L of solution?

a)

100 M

b)

1.6 M

c)

0.63 M

d)

0.010 M

3.

How many moles of solute are present in 0.050 L of 0.20M KNO3?

a)

10 moles solute

b)

0.050 moles solute

c)

1.0 moles solute

d)

0.010 moles solute

4.

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

5.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
6.

Which of these has ONLY London forces?

a)

I2

b)

NH3

c)

OCl2

d)

SH2

7.

What is the strongest type of Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

8.

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

a)

higher

b)

lower

9.

What is the strongest type of Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

10.

What is the strongest type of forces the following molecule have?

a)

dispersion forces

b)

dipoles

c)

hydrogen bonding

11.

Which of the following has the lowest boiling point?

a)

H2

b)

F2

c)

Cl2

d)

O2

12.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
13.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
14.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
15.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

16.

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

1.95 °C

d)

5128 °C

17.

There are four main processes in changing of phase, and they are

a)

Melting

b)

Boiling

c)

Condensation

d)

All the above

e)

Freezing

18.

Calculate the energy (in kJ) needed to completely boil away 30 g of water at 100 ⁰C .

a)

67.8 kJ

b)

2.26 kJ

c)

226 kJ

d)

0.100 kJ

19.

Temperature when a substance changes from a liquid to a gas

a)

Heat of Vaporization

b)

Boiling point

c)

Heat Energy

d)

Phase change

20.

Calculate the energy (in kJ) emitted when 100 grams of ice at 0 οC completely freezes.

a)

33.4 kJ

b)

0.400 kJ

c)

-33.4 kJ

d)

-2000 kJ

21.
On the pH scale what numbers are bases?
a)
8-14
b)
0-7
c)
7
d)
1
22.
On the pH scale what numbers are acids?
a)
8-14
b)
0-7
c)
7
d)
1
23.
On the pH scale what numbers are neutrals?
a)
8-14
b)
0-7
c)
7
d)
1
24.
The pH scale measures...
a)
...the strength of an acid.
b)
...the strength of hydrogen ions.
c)
...the concentration of hydrogen ions.
d)
...the concentration of an acid
25.

Is the following substance an acid or a base? Ca(OH)2

a)

Acid

b)

Base

26.

Is the following substance an acid or a base? HCl

a)

Acid

b)

Base

27.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
28.

Which compound is the conjugate acid? (Hint: Determine the base)

PO43- + HNO3 ==> NO3- + HPO42-

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

29.

In the reaction below, H2O is a(n):

H2SO3 + H2O --> H3O+ + HSO3-

a)

base

b)

acid

c)

conjugate acid

d)

conjugate base

30.
HSO4- + H2O → H3O++ SO42-
Identify the Acid in the above reaction.
a)
HSO4-
b)
H2O
c)
H3O+
d)
SO42-
31.
CO32-(aq)+H2O(l)      →              HCO3-(aq)+OH-(aq)
Using the above reaction, which compound is the conjugate base?
a)
CO32-
b)
H2O
c)
HCO3-
d)
OH-
32.

What is the pH of a 1.5 x 10-6 M solution of HCl?

a)

5.82

b)

8.18

c)

6.99

d)

4.15

33.

The pH of a solution where [H3O+] = 0.001 M is:

a)

11

b)

3

c)

-3

d)

-11

34.

The reaction of hydrochloric acid (HCl) with ammonia (NH3) is described by the equation:

HCl + NH3 → NH4Cl

A student is titrating 100.0 mL of 0.100 M NH3 with 0.500 M HCl. How much hydrochloric acid must be added to react completely with the ammonia?

a)

20.0 mL

b)

500 mL

c)

100 mL

d)

5.00 mL

35.

A 0.025L solution of HCl is neutralized by 0.018L of a 1.0 M NaOH solution. What is the concentration of the HCl solution? (predict the chemical equation first then)

Use the steps in your notes to help you set up this problem!

a)

1.4 M

b)

4.0 M

c)

0.72 M

d)

None of the above

36.

A 0.050L solution of Ba(OH)2 is neutralized by 0.072L of a 0.55 M HNO3 solution. What is the concentration of the Ba(OH)2 solution?

Ba(OH)2 + 2 HNO3 --> 2 H2O + Ba(NO3)2

a)

2 M

b)

0.40 M

c)

1.2 M

d)

None of the above

37.

Calculate the volume of a 0.15 M Ba(OH)2 solution required to completely neutralize 45 mL of a 0.29 M HNO3 solution.

a)

0.044 L

b)

0.087 L

c)

0.023 L

d)

0.051 L

38.

What is the mass percent of a solution that has 14.4 g of solute and 75.8 g of solvent?

(a)  

39.

Draw the full energetics / phase change diagram

40.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
41.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
42.
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
43.

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 %

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