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Worksheets

Unit 9 Study Guide

Total questions: 182

Worksheet time: 6hrs 17mins

Name
Class
Date
1.

Raising solvent temperature causes solvent-solute collisions to become

a)

more frequent and less energetic

b)

more frequent and more energetic

c)

less frequent and less energetic

d)

less frequent and more energetic

2.

Which of the following will dissolve most rapidly?

a)

sugar cubes in cold water

b)

sugar cubes in hot water

c)

powdered sugar in cold water

d)

powdered sugar in hot water

3.

Increasing the surface area of the solute

a)

increases the rate of dissolution

b)

increases solubility

c)

decreases the rate of dissolution

d)

has no effect on the rate of dissolution

4.

Water in air is an example of which solute-solvent combination?

a)

gas-liquid

b)

liquid-liquid

c)

gas-gas

d)

liquid-gas

5.

Which mixture contains visible particles that settle out unless the mixture is stirred?

a)

a solution

b)

a colloid

c)

a suspension

6.

If the amount of solute present in a solution at a given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be

a)

supersaturated

b)

concentrated

c)

saturated

d)

unsaturated

7.

Two immiscible substances are

a)

carbon tetrachloride and benzene

b)

water and ammonia

c)

water and ethanol

d)

benzene and water

8.

When solutions of two ionic compounds are combined and solid forms, the process is called

a)

dissociation

b)

solvation

c)

hydration

d)

precipitation

9.

Carbon dioxide dissolved in water is an example of which solute-solvent combination?

a)

cannot be determined

b)

gas-liquid

c)

liquid-gas

d)

liquid-liquid

10.

The solubility of gases in liquids

a)

increases with increasing pressure

b)

cannot reach equilibrium

c)

does not depend on pressure

d)

decreases with increasing pressure

11.

Which is not an example of a colloid?

a)

sugar water

b)

smoke

c)

paint

d)

butter

12.

The Tyndall effect is used to distinguish between

a)

solutions and colloids

b)

solvents and solutes

c)

liquids and gases

d)

electrolytes and nonelectrolytes

13.

Which of the following does not increase the rate of dissolving a solid in water?

a)

stirring the solution

b)

crushing the solid

c)

using larger pieces of solid

d)

raising the temperature of the water

14.

A metal solution is a(n)

a)

suspension

b)

alloy

c)

emulsion

d)

colloid

15.

A mixture that appears to be uniform while being stirred but which separates into different phases when agitation ceases is a

a)

solvent

b)

suspension

c)

colloid

d)

solute

16.

In a solution at equilibrium,

a)

the rate of dissolution and the rate of crystallization are equal

b)

the rate of dissolution is greater than the rate of crystallization

c)

the rate of dissolution is less than the rate of crystallization

d)

no dissolution occurs

17.

Oxygen in nitrogen is example of which solute-solvent combination?

a)

gas-solid

b)

gas-liquid

c)

gas-gas

d)

liquid-gas

18.

As temperature incrases, the solubility of gases in lquid

a)

can increase or decrease

b)

increases

c)

decreases

d)

is not effected

19.

Stirring increases the rate of dissolution because it

a)

brings fresh solvent into contact with the solute

b)

raises the temperature

c)

lowers the temperature

d)

decreases the surface area of the solute

20.

Which mixture contains particles that are in a dispersed phase and do not settle out?

a)

a solution

b)

a suspension

c)

a colloid

21.

Effervescence is the

a)

dissolution of gas

b)

escape of gas from a gas-liquid solution

c)

escape of liquid from a liquid-liquid solution

d)

escape of solid from a solid-liquid solution

22.

mixture in which the composition is not uniform throughout

a)

homogeneous mixture

b)

heterogeneous mixture

23.

substance that dissolves the solute

a)

solution

b)

solvent

c)

saturation

24.

If a spoonful of sugar is mixed in a glass of water, what is the water called? 

a)

solute

b)

solution

c)

solvent

d)

element 

25.

Milk is a 

a)

solution

b)

suspension

c)

colloid

26.

What type of mixture separates upon standing?

a)

Solution

b)

Alloy

c)

Colloid

d)

Suspension

27.

A saturated solution is______

a)

No more solute can be dissolved

b)

More solute can be dissolved

c)

The solvent and solution

28.

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 super amount of solvent in it. 

29.

When a certain amount of solvent cannot hold any more solute it is called a ________ solution.

a)

Diluted

b)

Saturated

30.

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

31.

What is an example of a colloid?

a)

fog

b)

water

c)

milk

d)

pepper and water 

32.

What type of solution will conduct electricity

a)

Ionic compound

b)

Molecular compound

c)

Sugar solution

d)

Saturated solution

33.

Which kind of mixture has the largest particles

a)

saturated solution

b)

suspension

c)

solution

d)

colloid

34.

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

35.

A solute that contains polar molecules will dissolve in a solvent that contains

a)

nonpolar molecules

b)

polar molecules

c)

covalent molecules

d)

equal-sized molecules

36.

Which key term describes the random movement of particles?

a)

a) Diffusion

b)

b) Osmosis

c)

c) Brownian Motion

d)

d) Absolute zero �

37.

what is another name for a homogeneous mixture? 

a)

solution 

b)

solids 

c)

elements 

d)

compound 

38.

What is the Tyndall effect? 

a)

the effect of light scattering in colloidal dispersion, while showing no light in a true solution

b)

something that is unwilling to dissolve in a solution

c)

a type of heterogeneous mixture where solid particles do not dissolve in a liquid solution

d)

something that do not settle out of the mixture and cannot be seen.

39.

What is an example of a colloid? 

a)

water 

b)

socks 

c)

whipped cream 

d)

computer 

40.

A solution that can hold more solute  is called

a)

saturated

b)

supersaturated

c)

unsaturated

d)

insoluble

41.

What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?

a)

0.018 M

b)

0.018 mol

c)

1.052 M

d)

1.052 mol

42.

The ___ is the thing being dissolved

a)

solute

b)

solvent

43.

True or false? Insoluble means that two substances can dissolve in one another.

a)

true

b)

false

44.

Which sweet tea would you expect to taste the sweetest?

a)

1M

b)

3M

c)

3.1M

d)

2.5M

45.

What is the formula for molarity?

a)

moles/grams

b)

moles/kilograms

c)

moles/milliliters

d)

moles/liters

46.

Molarity is measured in

a)

moles per kg

b)

mols per L

c)

moles per kJ

d)

moles per mL

47.

How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 

a)

3.18 L

b)

0.31 L

c)

3.85 L

d)

4.6 L

48.

If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?

a)

20.9 mol

b)

0.021 mol

c)

0.02 mol

d)

0.0209 mol

49.

What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?

a)

2.4 M

b)

0.86 M

c)

1.7 M

d)

0.54 M

50.

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

51.
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
52.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
53.
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
54.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
55.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
56.

What volume is needed to make a 2.45 M solution of KCl using 0.50 mol of KCl?

a)

4.9 L

b)

0.20 L

c)

1.2 L

57.

How many grams of C12H22O11(glucose) is saturated at 40 degrees?

a)

240

b)

220

c)

225

d)

250

58.

At what temperature can you fully dissolve 140g of NaNO3?

(a)   ​

Choose from the below words

62

73

81

330

100
85
59.

What type of a solution is 55g KCl at 70ºC in 100g H2O?

(a)  

Choose from the below words

Saturated

Unsaturated

Supersaturated
60.

Reacts with metals

a)

acid

b)

base

c)

both acid and base

61.

Has a pH more than 7

a)

acid

b)

base

c)

both an acid and a base

62.

Tastes bitter

a)

acid

b)

base

c)

both an acid and a base

63.

tastes sour

a)

acid

b)

base

c)

both an acid and a base

64.

Has a pH less than 7

a)

acid

b)

base

c)

both an acid and a base

65.

Ends with "OH-"

a)

acid

b)

base

c)

both an acid and a base

66.

Compound starts with an "H"

a)

acid

b)

base

c)

both an acid and a base

67.

Conducts electricity (has electrolytes)

a)

acid

b)

base

c)

both an acid and a base

68.

orange juice

a)

acid

b)

base

c)

both an acid and a base

69.

Soap

a)

acid

b)

base

c)

an acid and a base

70.

Feels slippery

a)

acid

b)

base

c)

an acid and a base

71.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

72.

Which is the correct set of acid properties:

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

73.

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)

74.

Is laundry detergent an acid or a base?

a)

Acid

b)

Base

c)

Neither (Neutral)

75.

Is pure water acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

76.

The pH scale is a range from:

a)

1-7

b)

0-14

c)

1-5

d)

1-14

77.

A solution with a pH of 8.6 would be a(n)

a)

Acid

b)

Base

c)

Neutral

d)

Acid and Base

78.

What type of paper is used to test for acids and bases?

a)

Red paper

b)

Blue paper

c)

Lined paper

d)

Litmus paper

79.

This ion is responsible for the properties of acids

a)

Sodium ion

b)

Hydrogen ion

c)

Hydroxide ion

d)

Oxide ion

80.

This ion is responsible for the properties of bases

a)

Sodium ion

b)

Hydrogen ion

c)

Hydroxide ion

d)

Oxide ion

81.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

82.

When acids react with metals, they produce hydrogen gas and salt.

a)

True

b)

False

83.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

84.

When an acid is dissolved in water, it turns red litmus paper blue.

a)

True

b)

False

85.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

86.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

87.

All bases have a sour taste.

a)

True

b)

False

88.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

89.

Which of the following is the strongest base?

a)

oven cleaner - 13.5

b)

lemon juice - 2.5

c)

soap - 10

d)

blood - 7.4

90.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

91.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
92.
When using pH paper, the pH of a solution can be determined by looking at the _______ of the paper.
a)
texture
b)
color
c)
length
d)
mass
93.
When using pH paper, the pH of a solution can be determined by looking at the _______ of the paper.
a)
texture
b)
color
c)
length
d)
mass
94.
Acids are what range on the pH scale?
a)
0-14
b)
0-6.99
c)
7
d)
7.1-14
95.
Bases are what range on the pH scale?
a)
0-6.99
b)
7
c)
7.1-14
d)
0-14
96.
7 on the pH scale means that it is...
a)
Acidic
b)
Basic
c)
Neutral
97.
When found in food, acids are ________
a)
Sour
b)
Bitter
c)
Salty
d)
Slippery
98.
When found in food, bases are _______.
a)
Sour
b)
Bitter
c)
Salty
d)
Soggy
99.
phosphorous acid
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
100.
hydrochloric acid
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
101.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
102.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
103.
Barium hydroxide
a)
BaOH
b)
Ba2OH
c)
Ba(OH)2
104.
Cu(OH)2
a)
Copper (II) hydroxide
b)
Copper (I) hydroxide
c)
Copper (II) hydride
d)
Copper (I) hydride
105.
Nitrous Acid
a)
HNO2
b)
H2NO2
c)
HNO3
106.
Select the name for the following acid: H2S
a)
Hydrosulfuric acid
b)
Sulfuric acid
c)
Sulfurous
107.
Is the following compound an acid or a base? 
HF
a)
Acid
b)
Base
108.
Is the following compound an acid or a base? 
Ca(OH)2
a)
Acid
b)
Base
109.
What is the name of bromic acid?
a)
HBr
b)
HBrO2
c)
HBrO3
d)
H3BrO3
110.
chloric acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
111.
Predict the products for the following reaction:
LiOH + H2SO4 -->
a)
LiSO4 + HOH
b)
LiSO4 + H2(OH)
c)
Li2SO4 + HOH
d)
Li2SO4 + H2(OH)
112.

____ change color in the presence of an acid or a base.

a)

Acids

b)

Buffers

c)

Glycerins

d)

Indicators

113.

Do acids and bases conduct electricity?

a)

Only acids conduct electricity

b)

Only bases conduct electricity

c)

Bases and acids conduct electricity

d)

Neither conduct electricity

114.

When magnesium reacts with dilute hydrochloric acid, a gas is given off.


Which gas is given off?

a)

Carbon dioxide

b)

Chlorine

c)

Hydrogen

d)

Oxygen

115.
In a ____ reaction, an acid and a base produce a salt and a water. 
a)
concentrated
b)
decomposition
c)
dilute
d)
neutralization
116.

Acids feel

a)

like water

b)

sticky

c)

slippery

d)

gooey

117.

As a product, if H2CO3 is produced it

a)

stays the same

b)

breaks apart into H2 and CO2

c)

breaks apart into H2 and salt

d)

breaks apart into H2O and CO2

118.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

119.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

120.

When an acid and base has been neutralized the pH will be?

a)

1

b)

4

c)

7

d)

10

121.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

122.

An acid

a)

is a substance that releases H+ ions when dissolved in water

b)

is a substance that does not release any ions when dissolved in water

c)

is a substance that releases OH- when dissolved in water

d)

releases an equal amount of OH- and H+ ions when dissolved in water

123.

A solution has a pH of 7.0. What would happen to the pH if OH- ions were added?

a)

pH would go up

b)

pH would go down

c)

pH would stay the same

d)

None of these

124.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
125.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
126.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
127.
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
128.
If the [H+] of a solution is 1 x 10-2 mol/L the pH is
a)
2
b)
12
c)
-2
d)
1
129.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

130.
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
131.
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
132.

A solution has 1.0 x 10-8 M hydronium ions. Another solution has 1.0 x 10-3 M hydronium ions. Which solution has a larger number of hydronium ions? Hint this solution is an acid.

a)

1.0 x 10-3 M hydronium ion solution

b)

1.0 x 10-8 M hydronium ion solution

c)

Neither solution is an acid

133.
Limes have a [H3O+] of 1.3 x 10-2 mol/L.  Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
134.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
135.

Water has a neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

136.
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
137.

What is the pOH of a 0.0124 M HCl solution?

a)

1.91

b)

12.09

c)

1.61

d)

12.39

138.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

139.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

140.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
141.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
142.
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
143.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

144.
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
145.
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
146.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

147.

The pH of a solution is 8.43. What is the hydronium ion H3O+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

148.

The pH of a solution is 8.43. What is the hydroxide ion OH- concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

antilog (-pH)

d)

1.0 x 10-14/-pH

149.

What is the hydronium ion concentration of 4.0 M H2SO4?

a)

4.0 M

b)

8.0 M

c)

1.0 x 10-4 M

d)

2.5 x 10-15 M

150.

A solution has 1.0 x 10-8 M hydronium ions. Another solution has 1.0 x 10-3 M hydronium ions. Which solution has a larger number of hydronium ions? Hint this solution is an acid.

a)

1.0 x 10-3 M hydronium ion solution

b)

1.0 x 10-8 M hydronium ion solution

c)

Neither solution is an acid

151.
Limes have a [H3O+] of 1.3 x 10-2 mol/L.  Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
152.

What is the [OH-] if the pH is 4.900?

a)

7.94 x 10-10 M

b)

1.00 x 10-4 M

c)

7.94 x 10-14 M

d)

4.90 x 10-10 M

153.
If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of HCl?
a)
0.043 M
b)
23.148 M
c)
0.231 M
154.
If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solutions, what is the concentration of the NaOH solution?
a)
0.004 M
b)
276 M
c)
0.036 M
155.
If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of sulfuric acid, what is the concentration of the acid?
a)
0.2 M
b)
5 M
c)
0.5 M
156.
How many milliliters of 0.360 M H2SO4 are required to neutralize 25 mL of 0.1 M Ba(OH)2?
a)
6.944 mL
b)
0.144 mL
c)
0.069 mL
157.
What is the molarity of a 30 mL HCl which is neutralized by 48 mL of 0.1 M NaOH?
a)
0.16 M
b)
6.25 M
c)
0.063 M
158.
A neutralization reaction involves when an acid and base reacts to produce
a)
a new acid and a new base
b)
water and salt
c)
carbon dioxide and water
159.
Titration is a process in which a neutralization reaction is used to determine the ______ of a solution.
a)
molarity
b)
volume
c)
moles 
160.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
161.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
162.
Changes the color of indicators.
a)
Acids
b)
Bases
c)
All
163.
If phenolphthalein turns bright pink, it indicates
a)
an acid 
b)
a base
c)
a neutral
164.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
165.

What is the concentration of a HCl solution if 24.7 cm3 of HCl are completely neutrilized by 35.8 cm3 of a 0.25 M NaOH solution?

a)

0.362 M

b)

3.62 M

c)

0.172 M

d)

35.4 M

166.

What mass of KHP will be completely neutrilized by 32.57 cm3 0.175 M standard NaOH solution? The Molar Mass of KPH is 204.22 g/mol. (1:1 molar ratio).

a)

23.28 g KHP

b)

1.164 g KHP

c)

11.64 g KHP

d)

2.328 g KHP

167.

Calculate the volume of a 0.15 M Ba(OH)2 solution required to completely neutralize 45 cm3 of a 0.29 M HNO3 solution.

a)

43.5 cm3

b)

87 cm3

c)

23.3 cm3

d)

51.9 cm3

168.

If it takes 54 cm3 of 0.1 M NaOH to neutralize 125 cm3 of an HCl solution, what is the concentration of HCl?

a)

0.043 M

b)

23.148 M

c)

0.231 M

169.

If it takes 25 cm3 of 0.05 M HCl to neutralize 345 cm3 of NaOH solutions, what is the concentration of the NaOH solution?

a)

0.004 M

b)

276 M

c)

0.0036 M

170.

How many milliliters of 0.360 M H2SO4 are required to neutralize 25 cm3 of 0.1 M Ba(OH)2?

a)

6.944 cm3

b)

0.144 cm3

c)

0.069 cm3

171.

What is the equivalence point of a titration?

a)

Where the amount of acid and base are balanced according to the equation

b)

Where there is no base

c)

At the end

172.

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?

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

a)

1.44 M

b)

4 M

c)

0.72 M

d)

None of the above

173.

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?

a)

2 M

b)

0.40 M

c)

1.2 M

d)

None of the above

174.

A 0.125L solution of NaOH is neutralized by 0.0425L of a 0.65 M H2SO4 solution. What is the concentration of the NaOH solution?

a)

0.1 M

b)

1.6 M

c)

0.44 M

d)

None of the above

175.

A 0.0800L solution of Ca(OH)2 is neutralized by 0.0293L of a 3.58 M H2CrO4 solution. What is the concentration of the Ca(OH)2 solution?

a)

1.31 M

b)

0.49 M

c)

5.32 M

d)

None of the above

176.

HCl + NaOH --> NaCl + H2O

How many moles of NaOH will neutralise 18.3cm3 of 1.0 mol / dm3 HCl solution?

a)

6.02 x 1023 mol

b)

1.83 x 104 mol

c)

0.0183 mol

d)

18.3 mol

177.

H2SO4 + 2NaOH --> Na2SO4 + 2H2O

How many moles of H2SO4 will neutralise 14.2 cm3 of 0.01 mol/dm3 NaOH? 

a)

1.42 x 104 mol

b)

7.1 x 10-5 mol

c)

1.42 x 10-4 mol

d)

7.1 x 105 mol

178.

HCl + NaOH --> NaCl + H2O

What volume of 0.01 mol/dm3 HCl solution will neutralise

50cm3 of 0.01 mol/dm3 NaOH solution?

a)

0.25cm3

b)

25cm3

c)

50cm3

d)

100cm3

179.

HCl + NaOH --> NaCl + H2O

What volume of 0.5 mol/dm3 HCl solution will neutralise

25cm3 of 1.0 mol/dm3 NaOH solution?

a)

0.5cm3

b)

12.5cm3

c)

25cm3

d)

50cm3

180.

H2SO4 + 2NaOH --> Na2SO4 + 2H2O

To 2 dp, what volume of 2.0 mol/dm3 H2SO4 solution will neutralise

36.20cm3 of 2.0 mol/dm3 NaOH solution?

a)

36.20cm3

b)

18.10cm3

c)

0.04cm3

d)

0.02cm3

181.

H3PO4 + 3NaOH --> Na3PO4 + 3H2O

What volume of 1.0 mol/dm3 H3PO4 will neutralise

36.0cm3 of 2.0 mol/dm3 NaOH?

a)

216.0cm3

b)

36.0cm3

c)

72.0cm3

d)

24.0cm3

182.

What concentration of H2SO4 solution

contains 0.04 mol of H+ ions in 25cm3?

a)

0.8 mol/dm3

b)

1.6 mol/dm3

c)

1.6 x 10-3 mol/dm3

d)

8.0 x 10-4 mol/dm3

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