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14 Regents: Acids, Bases and Salts

Total questions: 69

Worksheet time: 55mins

Name
Class
Date
1.

Acid is?

a)

A substance that reacts with metals and has a PH below 7.

b)

Often used in drain cleaner.

c)

Something that can only be found in a lab

d)

A bitter tasting substance

2.

A base is

a)

A substance that feels slippery, has a PH higher than 7, and is often used in drain cleaner.

b)

Has a PH of below 7 and can react with some metals

c)

Is only found in a lab

d)

Something water can never be

3.

A substance with a pH of lower than 7 is a

a)

Acid

b)

Redox

c)

Base

d)

Salt

4.

When you neutralize acid with a base you create

a)

a Salt and water

b)

You can not neutralize acid with a base

c)

You create carbon dioxide

d)

A moderate sized explosion

5.

A substance with a ph of higher that 7.5 is a?

a)

Home dog doggity

b)

Base

c)

Acid

d)

Salt

6.
An extremely strong acid would have a pH of...
a)
1
b)
7
c)
9
d)
14
7.
An extremely strong base would have a pH of...
a)
1
b)
7
c)
9
d)
14
8.
A neutral substance would have pH of...
a)
8
b)
7
c)
6
d)
14
9.
Indicators change color in the presence of a(n) _______________.
a)
acid or base
b)
buffer
c)
water molecule
d)
ester
10.
A base has a ___________ taste.
a)
bland
b)
salty
c)
bitter
d)
sour
11.

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

12.

Which of these taste sour?

a)

acids

b)

bases

c)

salts

13.

The pH scale is used to determine the strength of

a)

acids and bases

b)

chemical bonds

c)

electrical charges

d)

particles in a solution

14.

Complete the definition below:

Acids are....

a)

hydrogen donors.

b)

hydrogen acceptors.

c)

proton donors.

d)

proton acceptors.

15.

Which indicator is colourless in acid and pink in alkali?

a)

Litmus

b)

Phenolphthalein

c)

Universal Indicator

d)

Methyl Orange

16.

What is made when a proton reacts with a hydroxide ion?

a)

Water

b)

An acid

c)

An alkali

d)

A salt

17.

In a sample of solution, when methyl orange is added as an indicator, the solution turns yellow in colour , then resulting solution could be

a)

HCl

b)

Salt

c)

NaOH

d)

water

18.

What range of values on the pH scale represent solutions with a higher ratio of hydronium (H3O+) ions?

a)

0-14

b)

below 7

c)

7

d)

above 7

19.

An aqueous solution turns red litmus blue. The excess addition of which of the following would reverse the color change

a)

baking powder

b)

lime

c)

ammonium hydroxide solution

d)

HCL

20.

Which of the following is not a base?

a)

NaOH

b)

KOH

c)

NH4OH

d)

C2H5OH

21.

Which of the following are present in an aqueous solution of HCl

a)

H3O+ +CL-

b)

H30+ +OH-

c)

CL+ +OH-

d)

UNIONISED HCL

22.

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

a)

True

b)

False

23.

HCl is found in household products, including some toilet bowl cleaners. Is HCl an acid or a base?

a)

Acid

b)

Base

c)

Neither (Neutral)

24.

If a solution has an [H+] of 1 x 10-11, what is the pH? (Hint, you need to use the equation for -log (H+) to solve this.)

a)

11

b)

4

c)

3

d)

8

25.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
26.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
27.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

28.

A solution of Ca(OH)2 is 1.0 x 10-5 M. What is the hydronium ion concentration?

a)

1.0 x 10-5 M

b)

1.0 x 10-9 M

c)

5.0 x 10-10 M

d)

2.0 x 10-5 M

29.

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

30.

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

31.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

32.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

33.

In the equation below, what is the Bronsted Lowry acid (donates H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

34.

In the equation below, what is the Bronsted Lowry base (accepts H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

35.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

36.

What is the Bronsted Lowry base in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

37.

What is the conjugate acid in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

38.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

39.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

40.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

41.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

42.

Ammonia has a pOH of 2. Ammonia is a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

43.

Find the pH of a solution with [OH-] = 1 x 10-4.

a)

4

b)

10

c)

9

d)

11

44.

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

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

45.

If a solution has a very high pH, the hydroxide concentration is _______.

a)

very high

b)

very low

c)

zero

46.

If a solution has a very high hydrogen ion concentration, the hydroxide concentration is _______.

a)

very high

b)

very low

c)

zero

47.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
48.
In a ____ reaction, an acid and a base produce a salt and a water. 
a)
concentrated
b)
decomposition
c)
dilute
d)
neutralization
49.
What are the products to a neutralization reaction?
a)
H2 + Ionic Salt
b)
H2O + Ionic Salt
c)
H3O+ + Ionic Salt
d)
OH- + Ionic Salt
50.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

51.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
52.

What is the molarity of a 30 mL HCl which is neutralized by 48 mL of 0.1 M NaOH?


HCl + NaOH --> H2O + NaCl

a)

0.16 M

b)

6.25 M

c)

0.063 M

d)

.016M

53.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
d)

.08M

54.

What is the missing product in the following neutralization reaction?

HCl + NaOH → H2O + ______

a)

HNa

b)

ClOH

c)

NaCl

d)

CO2

55.

C6H12O6 is what kind of compound?

a)

electrolyte

b)

nonelectrolyte

c)

acid

d)

base

56.

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

57.

What is being donated/accepted between conjugate acid-base pairs?

a)

a hydrogen (H+) ion

b)

a hydroxide (OH-) ion

c)

water

d)

a neutron

58.

What are the conjugate bases in the following reaction?

a)

HCO3- & Cl-

b)

HCl & H2CO3

c)

H2CO3 & Cl-

d)

Cl- & HCl

59.

What are the conjugate acids in the following equation?

a)

NO3-  & PO43- 

b)

HNO3  & HPO42-

c)

NO3-  & PO43- 

d)

HPO42- & NO3- 

60.

Which of the following is an Arrhenius Acid?

a)

LiOH

b)

CO32-

c)

OH-

d)

H3PO4

61.
Which of the following shows the correct conjugate acid base pair?
a)
HCI (acid) / H3O+ (conjugate base)
b)
HCI (acid) / CI- (conjugate base)
c)
HCI (base) / CI- (conjugate acid)
d)
HCI (base) / H3O+ (conjugate acid)
62.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
63.

Which of the following will conduct electricity? Select all that apply

a)

Acidic solutions

b)

Basic solutions

c)

Ionic solutions

d)

Neutral covalent solutions

64.

An arrhenius acid

a)

produces hydroxide ions in a solution

b)

produces a hydrogen atom in a solution

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

65.

An arrhenius base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

66.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

67.

Water can act as both an acid and a base according to the bronsted lowry model. This means water is

a)

neutral

b)

conjugate

c)

ionic

d)

amphoteric

68.

Acid-base conjugate pairs differ by a single

a)

Electron

b)

Proton

c)

Neutron

d)

Oxygen

69.

Could C2H3O2- act as a base when placed in water?

a)

Yes, because it can accept a H+

b)

Yes, because it can donate a H+

c)

No, because it cannot donate a H+

d)

No, because it cannot accept a H+

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