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Test 7 Review (Honors)

Total questions: 146

Worksheet time: 5hrs 30mins

Name
Class
Date
1.
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. 
2.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Mixture
d)
Homogeneous solution
3.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
4.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
5.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

6.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

7.

The solubility of Yb2(SO4)3 ________________ with added temperature.

a)

increases

b)

decreases

c)

remains the same

8.

Determine the solubility for the substances at 55'C and arrange them in order from lowest to highest solubility.

a)

NaCl, NH4Cl, KBr, NaNO3

b)

NaCl, NH4Cl, NaNO3, KBr

c)

NH4Cl, NaCl, NaNO3, KBr

d)

NaNO3, KBr, NH4Cl, NaCl

9.

At 10'C, NaNO3's solubility is 80 g/100 g of H2O. Based on this information, what would the solubility be in 50 g of H2O.

a)

40

b)

80

c)

160

d)

16

10.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

11.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

60 g

d)

33 g

12.

How could you change a saturated solution to an unsaturated solution?

a)

Add solvent

b)

Add solute

13.

Identify the saturation associated with the product of this experiment.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

14.

Identify a method to decrease the dissolving rate of a solution:

a)

decrease the temperature

b)

add KE

c)

stir the solution

d)

increase the temperature

15.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
16.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
17.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
18.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
19.
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
20.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
21.
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
22.
An ______ is a compound that breaks apart in water, forming charged particles (ions) that can conduct electricity.
a)
electrolyte
b)
nonelectrolyte
c)
polar molecule
d)
non polar molecule
23.
How many more grams of KNO3 dissolve at 50 ⁰C compared to 0 ⁰C?
a)
85 g
b)
15 g
c)
70 g
d)
100 g
24.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
25.
When two liquids mix, they are said to be....
a)
insoluble
b)
miscible
c)
soluble
d)
immiscible
26.
Which of the following usually makes a substance dissolve faster in a solvent?
a)
agitating the solution
b)
increasing the particle size of the solute
c)
lowering the temperature
d)
decreasing the number of particles
27.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
28.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
29.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
30.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
31.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

32.

Stirring the solution increases the rate of dissolution (rate of dissolving).

a)

True

b)

False

33.

The smaller the particle size the faster the rate of dissolution (rate of dissolving).

a)

True

b)

False

34.
Which of the following statements is true about how using smaller salt crystals would affect the rate of making a salt solution in water?
a)
Smaller crystals increase the surface area and slow down dissolving.
b)
Smaller crystals decrease the surface area and speed up dissolving.
c)
Smaller crystals increase the surface area and speed up dissolving.
d)
Smaller crystals decrease the surface area and slow down dissolving.
35.

Which will dissolve faster? Crushed table salt or a cube of table salt. Assume they have an equal mass.

a)

crushed table salt

b)

crystal of table salt

36.

What combination would dissolve a solid solute the fastest?

a)

high temperature, no stirring

b)

no heat, no stirring

c)

sugar cube, no heat

d)

high temperature, stirring

37.

Which of the following actions will NOT

increase the rate of dissolution

(dissolving) for solids?

a)

Stirring the solution

b)

Decreasing the temperature

c)

Increasing the surface area of the

solute

d)

Increasing the temperature

38.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

39.

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

40.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

41.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

42.

What are the units of molality?

a)

M

b)

m

c)

Ml

d)

Mr

43.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

44.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

45.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
46.
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
47.

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

48.

The units "M" can also be written as:

a)

mol/L

b)

moles

c)

g/L

d)

g/mol

49.

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

50.

How many moles are present when there is 200 g solvent in a 2.0 m solution?

a)

0.01 moles

b)

400 moles

c)

10 moles

d)

0.4 moles

51.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

52.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

53.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

54.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
55.
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
56.
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
57.

The van't Hoff factor measures the number of particles formed in solution. What is the van't Hoff factor for the compound Na2SO4?

a)

1

b)

3

c)

5

d)

7

58.

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

a)

are volatile

b)

have higher boiling points

c)

produce fewer moles of solute particles per mole of solvent

d)

produce more moles of solute particles per mole of solvent

59.

When 11.0 g of CaCl2 dissolves in 45.0 g of water, what is the boiling point of the solution? (Kb = 0.512 oC/m)

a)

3.4

b)

103.4

c)

101.1

d)

1.1

e)

101.4

60.

Find the boiling point of a solution containing 15.0 g sucrose (molar mass = 342.3g/mol), in 100g of water. (Kb = 0.512 oC/m)

a)

100.2

b)

99.8

c)

0.2

d)

-0.2

61.

When 26.0 g of NaCl, are dissolved in 0.5 kg of water, what is the freezing point of this solution? (Kf = 1.86 oC/m)

a)

-3.3

b)

103.3

c)

-1.7

d)

-0.8

62.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

63.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

64.

True or false: a neutral solution has equal amounts of H+ and OH-.

a)

True

b)

False

65.

NaOH may be found in drain cleaners and as a component of soaps. Is NaOH an acid or a base?

a)

Acid

b)

Base

c)

Neither (Neutral)

66.

in aqueous solution, H+ ions exist as

a)

H30+

b)

H9O4+

c)

Neither of these

d)

either H30+ or H9O4+

67.
Which describes a base?
a)
Turns blue litmus red
b)
Turns red litmus blue
c)
pH of 7
d)
pH of 3
68.
Which is an acid?
a)
Turns blue litmus red
b)
Turns red litmus blue
c)
Has a pH of 11
d)
Has a pH of 7
69.
When found in food, acids are ________
a)
Sour
b)
Bitter
c)
Salty
d)
Slippery
70.
When found in food, bases are _______.
a)
Sour
b)
Bitter
c)
Salty
d)
Soggy
71.
What are properties of acids?
a)
Bitter, slippery, ph above 7
b)
Sour, reacts with metals, ph below 7
c)
Sour, reacts with metals, ph above 7
d)
Bitter, ph of 7, does not react with metals
72.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

73.
A neutralization reaction will always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
74.
If the [H+] of a solution is 1 x 10-2 mol/L the pH is
a)
2
b)
12
c)
-2
d)
1
75.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105  M
b)
1.0 x 109  M
c)
5.0 x 101  M
d)
1.0 x 10-5  M
76.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
77.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
78.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
79.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
negative number, no solution.
80.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
81.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
82.
if a solution has a pOH of 5.2 the [OH-] of the solution is
a)
6 x 10 -6 M
b)
6.3 x 10 -6 M
c)
1.58 x 10-5 M
d)
2 x 10-5 M
83.

What characterizes a strong acid or strong base?

a)

polar covalent bonding

b)

complete ionization in water

c)

ionic bonding

d)

a hydrogen ion or hydroxide ion

84.

Which of the following is an example of a weak base?

a)

NaOH

b)

KOH

c)

Ca(OH)2

d)

NH4OH

85.

Which compound can act as both an acid and a base?

a)

water

b)

ammonia

c)

sodium hydroxide

d)

hydrochloric acid

86.

Identify the acids involved in the equilibrium reaction:

CN– + H2O ↔ HCN + OH–

a)

CN– and H2O

b)

H2O and HCN

c)

CN– and OH–

d)

H2O and OH–

87.

A solution has a hydrogen ion concentration of 0.001 M. What is the pH of the solution?

a)

3

b)

7

c)

11

d)

13

88.

Which of the following is the most acidic?

a)

[H+] = 1 × 10–7 M

b)

[H+] = 1 × 10–4 M

c)

[H+] = 1 × 10–13 M

d)

[H+] = 1 × 10–10 M

89.

Which of the following is the most basic?

a)

[H+] = 1 × 10–2 M

b)

[OH–] = 1 × 10–4 M

c)

[H+] = 1 × 10–11 M

d)

[OH–] = 1 × 10–10 M

90.

What is transferred between a conjugate acid-base pairs?

a)

an electron

b)

a proton

c)

a hydroxide ion

d)

a hydronium ion

91.

The process of adding a known solution to determine the concentration of another, unknown solution is called ____.

a)

combustion

b)

hydrolysis

c)

titration

d)

indication

92.

According to Arrhenius, an acid is any species that can increase the

a)

hydrogen ion concentration in water

b)

hydroxide ion concentration in water

c)

nitrate ion in solutions of water

d)

pH

93.

According to the Bronsted theory of acids and bases, an acid is a (an)

a)

electron donor

b)

proton acceptor

c)

electron acceptor

d)

proton donor

94.

Any species that increases the hydroxide ion concentration in water according to Arrhenius is a (an)

a)

acid

b)

base

c)

neutral solution

d)

amphoteric species

95.

According to Bronsted, a base is any species that accepts a (an)

a)

proton

b)

electron

c)

neutron

d)

water molecule

96.

The conjugate base of HCl is

a)

H+

b)

Cl-

c)

H2O

d)

OH-

97.

The conjugate acid of CO32-

a)

CO2

b)

H2CO3

c)

HCO3-

d)

CO4

98.

The conjugate acid for NH3 is

a)

NH2

b)

N

c)

H3

d)

NH4+

99.

Which of the following would be the products of NH3 reacting with H2O?

a)

H2O and NH4+

b)

H3O+ and NH3

c)

NH4+ and OH-

d)

NH52+ and O2-

100.

Amphoteric species or chemicals are those that can act as both

a)

acid and base

b)

acid and salt

c)

base and salt

d)

salt and water

101.

Why is water considered amphoteric?

a)

it can act as an acid in freezing temperatures

b)

it can act as a base any time

c)

it can act as either an acid or base

d)

it can autoionize and form radicals

102.

What is the conjugate base for HClO4?

a)

ClO-

b)

ClO2-

c)

ClO3-

d)

ClO4-

103.

What were the limitations to Arrhenius' Theory?

a)

it does not account for basic substances that do not contain a OH- group

b)

it does not account for relative strength of acids and bases

c)

restricts acids to water solutions only

d)

it restricts who can use the acids and bases

104.
A substance that changes color when mixed with an acid or base is a(n) ___.
a)
indicator
b)
neutralizer
c)
corrosive
d)
electricity
105.

According to Bronsted-Lowry, what is the definition of an BASE?

a)

a substance that donates a hydrogen (H+) ion

b)

a substance that donates a hydroxide (OH-) ion

c)

a substance that accepts a hydrogen (H+) ion

d)

a substance that accepts a hydroxide (OH-) ion

106.

According to Brønsted-Lowry acid base theory, an acid ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces H+ when added to water

d)

turns phenolphthalein pink

107.

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq)

Identify the Brønsted-Lowry acid in the above reaction.

a)

HSO4-

b)

H2O

c)

H3O+

d)

SO42-

108.

Choose the conjugate base of HNO3

a)

HNO3

b)

H2O

c)

H3O+

d)

NO3-

109.

True or False: All Arrhenius acids are also Brønsted-Lowry acids.

a)

True

b)

False

110.

According to Brønsted-Lowry acid base theory, a base ___.

a)

is a proton donor

b)

is a proton acceptor

c)

produces OH- when added to water

d)

has a bitter taste

111.

According to Arrhenius acid-base theory, a base ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces OH- in water

d)

turns litmus paper red

112.
According to Lewis acid-base theory, a Lewis base is.....
a)
an electron pair acceptor
b)
an electron pair donor
c)
an oxidising agent
d)
a reducing agent
113.
According to which acid-base theory is a base a proton acceptor?
a)
Arrhenius
b)
Bronsted-Lowry
c)
Lewis
114.

Lewis bases are defined as

a)

H+ acceptors

b)

electron pair acceptors

c)

H+ donors

d)

electron pair donors

115.

True or False? All acids are Lewis acids.

a)

True

b)

False

116.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

117.

Complete the following reaction:

H3PO4 + NaOH -->

a)

Na3PO4 + H2O

b)

Na +H2O

c)

Na3PO4 + H2

d)

Na3PO4 + H2O + CO2

118.

Complete the following reaction:

HNO3 + Ca(OH)2 -->

a)

Ca(NO3)2 + H2O

b)

Ca +H2O

c)

Ca(NO3)2 + H2

d)

Ca(NO3)2 + H2O + CO2

119.
What indicator is commonly used in titrations?
a)
Phenolphthalein
b)
Bromothymol Blue 
c)
Litmus
d)
Universal 
120.
If phenolphthalein turns bright pink, it indicates
a)
an acid 
b)
a base
c)
a neutral
121.

According to the Kinetic Molecular Theory a liquid's (SELECT ALL THAT APPLY)

a)

particles are held close together by intermolecular forces

b)

particles are in constant motion

c)

particles are vibrating in place and closely packed

d)

particles are not moving

122.

The energy of movement is ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

123.

The more energy that particles have, the ___ they move.

a)

slower

b)

faster

124.
Solids are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
125.

The force of attraction is greatest between the particles of a

a)

mixture

b)

gas

c)

solid

d)

pure substance

126.

According to kinetic molecular model, in gases,

a)

The particles are closely packed together, they occupy minimum space and are usually arranged in a regular pattern

b)

The particles occur in clusters with molecules slightly further apart

c)

The molecules are very far apart and occupy all space made available to them

d)

The particles vibrate about fixed positions and are held together by strong intermolecular bonds between them

127.

The particles of ___ generally have the least amount of energy.

a)

solids

b)

liquids

c)

gases

128.

In this phase of matter, particles do NOT stop moving. Instead they vibrate in place

a)

Plasma

b)

Solid

c)

Liquid

d)

Gas

129.

The particles in a gas are ______ away from each other than the particles in a solid

a)

farther

b)

closer

c)

the same distance

130.
Which temperature scale has no negative temperatures?
a)
Celsius
b)
Fahrenheit 
c)
Joule
d)
Kelvin
131.
This happens to water at 0 degrees Celsius.
a)
Boils
b)
Freezes
c)
Heats
d)
All of them
132.
The faster molecules move, 
a)
the higher the temperature
b)
the less temperature
c)
the same temperature
d)
I don't know
133.

Temperature is a measure of the average _____________ energy of the particles of a substance.

a)

potential

b)

kinetic

c)

gravitational

d)

heat

134.
Which of the following terms identifies the change from a liquid to gas?
a)
Vaporization
b)
Condensation
c)
Deposition
d)
Sublimation
135.
Phase change from a solid to a gas.
a)
sublimation
b)
deposition
c)
condensation
d)
evaporation
136.
Phase change from a solid to a liquid.
a)
melting
b)
sublimation
c)
boiling
d)
condensation
137.
Phase change from a gas to a liquid.
a)
condensation
b)
evaporation
c)
melting
d)
deposition
138.
Change from Gas to Solid is called........
a)
Sublimation
b)
Deposition
c)
Fusion
d)
condensation
139.

Paris has a average temperature of 5ºC in winter season, that means in Kelvin scale is:

a)

170 K

b)

5 K

c)

268 K

d)

278 K

140.
Diffusion is the movement of molecules from an area of _____ concentration to an ______ concentration
a)
High, low
b)
Low, high
c)
Low, low,
d)
High, high
141.

What process is being shown in this picture

a)

Diffusion

b)

Fermentation

c)

Effusion

d)

Chaos

142.

why would O2 effuse faster than CO2 in the same room

a)

because it has more energy

b)

because it has a lower molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

143.
If an unknown gas diffuses twice the speed of O2 (M=32) , what would its molar mass be
a)
2
b)
4
c)
6
d)
8
144.
how many times faster does He effuse compared to N2 (He = 4  N2 = 28)
a)
1.2 times faster
b)
2.65 times faster
c)
7 times faster
d)
0.377 times faster
145.
what is the rate of effusion for NH3 (M=17) if the rate of effusion for SO2 (M=17) is 0.800m/s
a)
1.55 m/s
b)
2.00 m/s
c)
0.500m/s
d)
0.800m/s
146.
An unknown gas diffuses 0.25 times as fast as helium gas (He). What is the molecular mass of the unknown gas? 
a)
64 g/mol
b)
16 g/mol
c)
32 g/mol
d)
4 g/mol

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