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Big Acid-Base Review

Total questions: 80

Worksheet time: 2hrs 30mins

Name
Class
Date
1.
Which of the following is a base?
a)
orange juice
b)
water
c)
vinegar
d)
dishwashing detergent
2.
Which of the following statements is correct?
a)
Blue litmus paper turns red when placed in a base.
b)
Red litmus paper turns blue when placed in a base.
c)
Blue litmus paper stays blue when placed in an acid.
d)
Red litmus paper stays red when placed in a base.
3.

What would be considered the weakest alkali? ( Hint: lowest [OH-] )

a)

8

b)

14

c)

7.8

d)

11.6

4.

What was phenolphthalein used as in the titration? Does it show an exact pH or a range?

a)

as an acid, exact

b)

as a base, exact

c)

as a titrant, range

d)

as an indicator, range

5.

Acids produce _________ ions when they break down or dissociate. 

a)

Hydroxide (OH-)

b)

Water

c)

Chlorine (Cl-)

d)

Hydrogen (H+) or Hydronium (H3O+)

6.
Bases release ____________ ions when they break down or dissociate. 
a)
Hydrogen (H+)
b)
Hydroxide (OH-)
c)
Chlorine (Cl-)
d)
no
7.

All are examples of Arrhenius bases except

NaOH, KOH, LiOH, HCl

a)

NaOH

b)

KOH

c)

LiOH

d)

HCl

8.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
9.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl -

10.
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
11.

A substance that remains when a base has accepted an H+ ion is... (Hint: What does the base turn into?)

a)

An acid

b)

A Base

c)

A Conjugate Acid

d)

A Conjugate Base

12.

If a solution is alkaline which ion will be more present?

a)

H+

b)

K+

c)

OH-

d)

H-

13.

A substance that remains when an acid has donated an H+ ion is... (Hint: What does the acid turn into?)

a)

An acid

b)

A Base

c)

A Conjugate Acid

d)

A Conjugate Base

14.

If the pOH of a substance is 5, what is the pH? Is it an acid or an alkali?

a)

5 : Acid

b)

9 : Alkali

c)

-5 : Acid

d)

9 : Acid

15.

If a solution has a [H+] of 1E-10 M (same as 1x10-10 M) What is it's pH? What is it's pOH?

a)

pH= 10 / pOH= 4

b)

pH= 4 / pOH= 10

c)

pH= 10 / pOH= 10

d)

pH= 4 / pOH= 4

16.

If a solution has a [H+] of 1E-2 M (same as 1x10-2 M) What is it's pH? Is it acidic or alkaline?

a)

2, acidic

b)

-2, acidic

c)

12, alkaline

d)

12, acidic

17.

If something has equal concentrations of hydrogen/ hydronium ion and hydroxide ion, what pH would it be?

a)

10

b)

2

c)

7

d)

5

18.

What is the acid in the following equation?

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

19.

What is the base in the following equation?

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

20.

A Limitation of the Bronsted- Lowry is that.....

a)

it cannot describe a base without OH-

b)

It cannot describe an acid- base reaction that has no proton (H+) transfer

c)

It cannot describe an acid with the H at the end

d)

it only works with solutions containing water.

21.

Limitations of the Arrhenius Model are that....

a)

it cannot describe a acid without H+

b)

It cannot describe a base without OH-

c)

Arrhenius' name is hard to spell

d)

it only works with solutions containing water.

22.

Which represents a strong acid?

a)

The left one, the acid is 100% disassociated

b)

The left one, the acid is partially disassociated

c)

The right one, the acid is 100% disassociated

d)

The right one, the acid is partially disassociated

23.

Which of the above, I, II, or III, show a strong acid? (HA is the original acid)

a)

I

b)

II

c)

III

d)

I and II

24.

Using this graphic, why do strong acids have a single arrow?

a)

Weak acids always have some of the original acid, this is because weak acids never fully disassociate.

b)

Weak acids never have some of the original acid, this is because weak acids fully disassociate.

c)

Strong acids always have some of the original acid, this is because weak acids never fully disassociate.

d)

Strong acids never have some of the original acid, this is because strong acids fully disassociate.

25.

Phenolphthalein is an ___________ it turns from ____________ to ______________ in a base.

a)

indicator/ colorless/ pink

b)

indicator/ pink/ colorless

c)

acid/ colorless/ pink

d)

base/ colorless/ pink

26.

Which of the following are polyprotic acids? (Hint: poly means many)

a)

HClO3

b)

H3PO4

c)

H3P

d)

H2SO4

e)

HCl

27.

Which of the following are monoprotic acids?

a)

HClO3

b)

H3PO4

c)

H3P

d)

H2SO4

e)

HCl

28.

Which of the following are oxyacids acids?

a)

HClO3

b)

H3PO4

c)

H3P

d)

H2SO4

e)

HCl

29.

Which of the following are binary acids?

a)

HClO3

b)

H3PO4

c)

H3P

d)

H2SO4

e)

HCl

30.

What is the name of this acid: HCN

a)

hydrocyanic acid

b)

cyanic acid

c)

cyanous acid

31.

What is the name of this acid: HClO4

a)

hydroperchloric acid

b)

perchloric acid

c)

perchlorous acid

32.

What is the name of this acid: H3PO3

a)

hydrophosphoric acid

b)

phosphoric acid

c)

phosphorous acid

33.

What is the name of this base: Fe(OH)3

a)

Iron (III) hydroxide

b)

Iron hydroxide

c)

ferrium hydroxide

d)

Fe three hydroxide

34.

30mL of NaOH is neutralized by 12.3mL of 0.2M HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

35.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
36.
What indicator is commonly used in titrations?
a)
Phenolphthalein
b)
Bromothymol Blue 
c)
Litmus
d)
Universal 
37.
If phenolphthalein turns bright pink, it indicates
a)
an acid 
b)
a base
c)
a neutral
38.

What is the endpoint in a titration?

a)

When the indicator is added

b)

When neutralization occurs and the color of the indicator is a soft light pink

c)

When the standard solution is prepare

d)

When neutralization occurs and the color of the indicator is violently bright pink

39.

Identify the products of the chemical equation

3LiOH + H3PO4 →

a)

Li3PO4 + 3H2O

b)

LiPO4 + 3H2O

c)

Li(PO4)3 + 3H2O

d)

LiPO43 + 3H2O

40.

The __________ of a titration occurs when you have added just enough of the one solution to completely react with the other solution.

a)

endpoint

b)

neutralization

c)

base

d)

acid

41.

A reaction between an acid and base is called...

a)

decomposition

b)

single displacement

c)

neutralization

d)

salt & water

42.

NaCl is...

a)

an acid

b)

a base

c)

a salt

43.

Which has more OH ions? A solution with a pH of 4 or a pH of 10?

a)

pH of 4

b)

pH of 10

44.

Which of the following will not react with an acid?

a)

NaOH

b)

CaCO3

c)

Mg

d)

Acids will react with all of these

45.

A strong acid and a strong base are misced together, assuming they are the same concentration... What ratio will create a neutral solution?

a)

1:1

b)

2:1

c)

1:2

d)

coronal mass ejection

46.

Main difference between an amphoteric substance and a buffer?

a)

only buffers regulate small changes in pH

b)

only amphoteric substances can act as an acid or as a base

c)

only buffers have small amounts of conjugate acid and conjugate base

d)

ALL of these are the main difference!

47.
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)
48.

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

a)

11

b)

-3

c)

3

d)

1

49.

A pH of 8 is how many times more acidic than a pH of 11?

a)

3

b)

30

c)

100

d)

1000

50.

Which pH has the most hydrogen ions (H+)?

a)

2

b)

7

c)

10

d)

13

51.

Which of the following formulas is used to determine the pH of a solution?

a)

pH = –log[H+]

b)

pH = log[H+]

c)

pH = log[OH+]

d)

pH = [OH–]

52.

CH3CH2COOH(aq) + H2O(l) ⇄ CH3CH2COO─(aq) + H3O+(aq)

 

Is this a strong or Weak Base... why?

a)

Strong, double arrow

b)

weak, double arrow

c)

Strong, single arrow

d)

Weak, single arrow

53.

What is a mixture of chemicals that react with a base/acid to keep pH in a narrow range?

a)

catalyst

b)

amphoteric

c)

water

d)

buffer

54.

Bleach is a strong base, how many times stronger (more basic/concentrated) is bleach than Milk of Magnesia?

a)

3

b)

10

c)

100

d)

1000

55.

Which substance has the most hydrogen ions?

a)

bananas

b)

lemon juice

c)

orange juice

d)

Milk of Magnesia

56.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
57.

When H+ concentration is greater than OH- concentration, [H+] > [OH-] , the solution is

a)

basic

b)

neutral

c)

acidic

d)

alkaline

58.

When OH- concentration is greater than H+ concentration, [H+] < [OH-] , the solution is

a)

alkaline

b)

acidic

c)

neutral

d)

amphoteric

59.

Each change of a single pH unit signifies a ________ change in the concentration of the hydrogen ion.

a)

onefold

b)

hundredfold

c)

tenfold

60.

As the concentration of the hydrogen or hydronium ion increases, the concentration of the hydroxide ion

a)

remains the same

b)

decreases

c)

increase

61.

As phenolphthalein loses its hydrogen ion (proton), the indicator turns

a)

colorless

b)

pink

c)

purple

d)

yellow

62.

As the H+ or H3O+ ion concentration of a solution increases, the pH of the solution

a)

decreases

b)

increases

c)

remains the same

63.

Which substance has the least hydrogen ions?

a)

bananas

b)

lemon juice

c)

orange juice

d)

Milk of Magnesia

64.

Which substance has the most hydroxide ions?

a)

bananas

b)

lemon juice

c)

orange juice

d)

Milk of Magnesia

65.

Which substance has the least hydroxide ions?

a)

bananas

b)

lemon juice

c)

orange juice

d)

Milk of Magnesia

66.

Acid rain is a weak acid, how many times weaker (less acidic/concentrated) is acid rain than hydrochloric acid?

a)

3

b)

10

c)

100

d)

1000

67.

Write the formula of the following compound.

Nitrous acid

a)

HN

b)

HNO2

c)

HNO3

68.

Write the formula of the following compound.

Hydrochloric acid

a)

HCl

b)

HClO2

c)

HClO3

69.

What is the formula for nitric acid?

a)

HNO3

b)

HNO2

c)

HNO4

d)

NO

70.

The suffix -ite in the name of a polyatomic ion becomes ______ in the acid name.

a)

-ous acid

b)

-ate acid

c)

-ide acid

d)

-ic acid

71.

What prefix is used to name binary acids?

a)

per-

b)

hydro-

c)

hypo-

d)

bi-

72.

The suffix -ate in the name of a polyatomic ion becomes ______ in the acid name.

a)

-ous acid

b)

-ite acid

c)

-ide acid

d)

-ic acid

73.

Titration: Where on the graph is the midpoint/ equivalence point?

a)

The center of the vertical line with a pH of 7

b)

The top of the vertical line with a pH of 7

c)

The bottom of the vertical line with a pH of 7

d)

The end of the top line where the graph stops, with a pH of 7

74.

According to one acid-base theory, the water acts as

a)

a base because it accepts an H+

b)

a base because it donates an H+

c)

an acid because it accepts an H+

d)

an acid because it donates an H+

75.

According to one acid-base theory, the reactant that donates an H+ ion in the forward reaction is

a)

b)

c)

d)

76.

In which forward reaction is water acting only as a proton acceptor?

a)

b)

c)

d)

77.

When using the Arrhenius model, what types of ions indicate that a compound is an acid?

a)

H+

b)

OH-1

78.

When using the Bronsted Lowry definition of acids and bases, the acid will ______________ a hydrogen proton.

a)

donate

b)

accept

79.

Which of the following correctly identifies a conjugate Pair?

a)

HH4+ , OH-

b)

H2O , OH-

c)

CaCO3 ,CaCl2

d)

HNO3 , H2SO4

80.

Which of the following shows the correct conjugate 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)

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