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Chemistry II Unit 6 Review - Mostly Theory

Total questions: 75

Worksheet time: 5hrs 53mins

Name
Class
Date
1.

Which of these is a property of acidic solutions?

a)

they taste sour

b)

they feel slippery

c)

they are in many cleaning products

d)

they taste bitter

2.

Bases turn red litmus paper (a)   .

3.

The (a)   scale measures the strength of acids and bases.

4.

What are the products of a neutralization reactions

a)

water

b)

salt

c)

acid

d)

base

5.

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

6.

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

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

7.

Which reactant in the following equation is acting as a Brønsted-Lowry acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

8.

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-

9.

CO32-(aq) + H2O(l) → HCO3-(aq) + OH-(aq)

Using the above reaction, which species is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

10.

A substance that remains when a base has accepted an H+ ion is a(n)


(a)  
Choose from the below words
conjugate acid
acid
base
conjugate base
11.

Choose the conjugate acid of OH-

a)

HCO3-

b)

OH-

c)

CO32-

d)

H2O

12.

Choose the conjugate base of HNO3

a)

HNO3

b)

H2O

c)

H3O+

d)

NO3-

13.

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

a)

True

b)

False

14.

Which of the following substances is both a Brønsted-Lowry base and an Arrhenius base?

a)

NH3(aq)

b)

LiOH(aq)

c)

HCl(g)

d)

HCl(aq)

15.

Which of the following is a polyprotic acid?

a)

HCl

b)

H2SO4

c)

HNO3

d)

HF

16.

Which of the following is the hydronium ion?

a)

H+

b)

H2O

c)

OH–

d)

H3O+

17.

The conjugate acid for NH3 is

a)

NH2

b)

N

c)

H3

d)

NH4+

18.

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

19.

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

20.
Is HNO3 an acid or base?
a)
Acid
b)
Base
21.
KOH will release which ion?
a)
OH-
b)
H+
c)
OH+
d)
H-
22.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
23.

Match

a)

H+

1.

Acid

b)

OH-

2.

Base

c)

NaCl

3.

Salt

24.

Match the following

a)

higher than 7

1.

base

b)

lower than 7

2.

acid

c)

7

3.

neutral

25.

Match these

a)

strongly acidic

1.

3.3 mountain dew

b)

slightly acidic

2.

6.7 milk

c)

strongly basic (alkaline)

3.

13 ammonia

d)

slightly basic (alkaline)

4.

7.35 human blood

26.

The table shows the pH of several solutions. Which solution has the greatest concentration (amount) of OH- ions?

a)

vinegar

b)

milk

c)

water

d)

bleach

27.

Bases, also known as ​ (a)   will turn litmus paper ​ (b)   . This is because they have a pH ​ (c)   . They taste ​ (d)   .

Choose from the below words
alkali and OH-
blue
above 7
bitter
below 7
H+
red
sour
28.

Acids, also known as ​ (a)   , will turn litmus paper ​ (b)   . This is because they have a pH ​ (c)   . They taste ​ (d)   .

Choose from the below words
H+
red
below 7
sour
bitter
above 7
blue
29.

Match the following

a)

10

1.

base

b)

5

2.

acid

c)

salt

3.

neutral

30.

What does pH measure?

a)

strength of an acid

b)

strength of a base

c)

strength of both acids and bases

d)

concentration of H+ ions

31.

Which of the following is the correct definition for a strong acid?

a)

Partially dissociates into ions when dissolved in water and the change is not reversible

b)

Fully dissociates into ions when dissolved in water and the change is not reversible

c)

Fully dissociates into ions when dissolved in water and the change is reversible

d)

Partially dissociates into ions when dissolved in water and the change is reversible

32.

Which of the following is NOT an acid?

a)

HCl

b)

CH3COOH

c)

C2H6

d)

H2SO4

33.

For this reaction :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


Which one can act as an acid ?

a)

HA(aq) and A-(aq)

b)

H2O(l) and H3O+(aq)

c)

HA(aq) and H3O+(aq)

d)

H2O(l) and A-(aq)

34.

dissociation of weak acid, HA, is represented by following equation :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


The equilibrium constant for this reaction is represented by Ka . Which of the following equation represents expression of equilibrium constant, Ka?

a)
b)
c)
d)
35.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
36.

What is the name of this ion: H3O+?

a)

Helium ion.

b)

Hydrogen ion.

c)

Hepatic ion.

d)

Hydronium ion.

37.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

4.605.02.57

a)

4.6

b)

5.0

c)

2.5

d)

7.0

38.

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-

39.

What is the [OH-] if the [H+] is 1.0 x 10-3 M?

a)

1.0 x 10-3 M

b)

6.02 x 10-23 M

c)

1.0 x 10-14 M

d)

1.0 x 10-11 M

40.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
41.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
42.
Which of the following is the conjugate acid of HCO3-1?
a)
H2CO3
b)
CO3-2
c)
H2CO3-1
d)
CO3-1
43.

Phenol, C6H5OH, has a Ka =1.0 x 10-10. What is the pH of a 0.010 M solution of phenol?

a)

between 3-7

b)

10

c)

2

d)

between 7-10

e)

7

44.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

45.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

46.
The Acid-Base classification system that defined any chemical species that accepts a pair of electrons as a _______, and a _________ is a chemical species that donates a pair of electrons.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
47.
The Acid-Base classification system that defined a __________ is any compound that can donate a proton (an H+ ion) to an appropriate acceptor. A _________ is a compound that can remove (or accept) a proton.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
48.
Accepts a pair of electrons
a)
Lewis Acid
b)
Arrhenius Acid 
c)
Bronsted Lowry Acid 
d)
Arrhenius Base
49.

Lewis bases are defined as

a)

H+ acceptors

b)

electron pair acceptors

c)

H+ donors

d)

electron pair donors

50.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

51.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

52.
The Kw constant is:
a)
1.0 x 10-14
b)
1.0 x 1014
c)
6.022 x 1023
d)
6.0634 x 10-34
53.

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

a)

Ca(OH)2

b)

NH3

c)

NaOH

d)

KOH

54.

Hydrochloric acid (HCl) and acetic acid (HC2H3O2) are both acids. HCl completely dissociates in water, while HC2H3O2 does not. Which of the following statements best describes these two acids?

a)

HCl is a weak acid, HC2H3O2 is a weak acid.

b)

HCl is a strong acid, HC2H3O2 is a strong acid.

c)

HCl is a strong acid, HC2H3O2 is a weak acid.

d)

HCl is a weak acid, HC2H3O2 is a strong acid.

55.
Forms a OH- hydroxide ion
a)
Lewis Base
b)
Arrhenius Base
c)
Bronsted Lowry Base
d)
Bronsted Lowry Acid
56.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
57.

What is the conjugate acid of CO3-2?

a)

CO2-2

b)

HCO22-2

c)

H2CO3

d)

HCO3-1

58.

Of the following, which is the strongest acid

a)

HClO

b)

HClO2

c)

HClO3

d)

HClO4

59.

What is the pH of a 0.053 M solution of potassium hydroxide

a)

6.91

b)

12.72

c)

7.33

d)

1.28

60.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
61.

A solution contains 0.04 M of a weak acid. Calculate the pH of the solution knowing that the Ka for the acid is 1.6 x 10-7

a)

It is not possible to solve if the identity of the acid is not known

b)

4.1

c)

4.9

d)

Because the Ka is very small, the pH is close to neutral (about 6)

62.
I have a pOH have 4.23. Am I acidic or basic?
a)
Acidic
b)
Basic
c)
Neutral
63.

Which of the following describes H2SO4

a)

Weak acid

b)

Strong base

c)

Strong acid

d)

Weak base

64.

Which of these is a strong acid?

a)

NH3

b)

CH3COOH

c)

HClO3

d)

HF

65.

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

66.

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

a)

M

b)

mol

c)

g

d)

g/L

67.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

68.
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
69.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
70.

The units "M" can also be written as:

a)

mol/L

b)

moles

c)

g/L

d)

g/mol

71.

If 1 mole of solute is dissolved in 1 liter of water, what is the molarity?

a)

2M

b)

.5M

c)

1M

d)

It can't be determined unless you know the solute

72.
What is the molality of a solution containing 1.3 mol in 13.4 kg of solution?
a)
9.7 m
b)
17.42 m
c)
0.097 m
73.

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

74.

What is the molality of a solution in which 15 g if I2 is dissolved in 2.0 Kg of water?

a)

1.5 M

b)

1.5 M

c)

13.3 N

d)

0.12 m

75.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

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