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AP Ch5 Acid and Base Types and Strengths

Total questions: 79

Worksheet time: 3hrs 3mins

Name
Class
Date
1.

The value of Kw for water at 0°C is 1×10−15. What is the pOH of water at 0°C?

a)

6.5

b)

7.0

c)

7.5

d)

8.0

2.

The pH of a solution prepared by the addition of 10. mL of 0.002 M KOH(aq) to 10. mL of distilled water is closest to

a)

12

b)

11

c)

10

d)

4

3.

What is the H+(aq) concentration in 0.05 M HCN(aq)? (Ka for HCN is 5.0 x 10-10)

a)

2.5 x 10-11 M

b)

2.5 x 10-10 M

c)

5.0 x 10-10 M

d)

5.0 x 10-6 M

4.

A solution prepared by mixing 10 mL of 1 M HCl and 10 mL of 1.2 M NaOH has a pH of

a)

1

b)

5

c)

7

d)

13

5.

The table above provides the chemical structures for weak bases and their ionization constants, Kb. Based on the data, which of the following provides the best reason for the trend in base strengths?

a)

The number of hydrogen atoms

b)

The number of resonance structures

c)

The different electronegativities of H, I, and Br

d)

The different molar masses

6.
Consider the reaction of CaCN2 and water to produce CaCO3 and NH3:
CaCN2 + 3H2O → CaCO3 + 2NH3
How much NH3 is produced upon reaction of 160. g of CaCN2 and 4.0. moles of H2O?
a)
2.00 moles NH3
b)
4.00 moles NH3
c)
2.67 moles NH3
d)
6.00 moles NH3
7.
If 5.0 moles of NaOH are mixed with 5.0 moles of H2SO4 in a neutralization reaction in aqueous solution, the limiting reactant is
a)
H2SO4
b)
NaOH
c)
H2O
d)
Na2SO4
8.
If a solution has a [H+] of 1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M 
b)
8.3 x 10-11M 
c)
1.2 x 1010M 
d)
1.2 x 10-4M 
9.
If a solution has a [OH-] of 3.42 x 10-12M what is the [H+]?
a)
2.92 x 10-3M 
b)
3.42 x 102M 
c)
2.92 x 10-2M 
d)
3.42 x 10-5M 
10.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
11.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
12.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
13.
Which donates protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
14.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

15.
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
16.
Which is the weakest acid?
a)
HF
b)
HNO2
c)
CH3COOH
d)
HClO
17.

What is the pH of a solution that has an [H+] of 2.5 × 10–5?

a)

4.60

b)

5.0

c)

2.5

d)

7

18.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
19.

A 1-molar solution of a very weak monoprotic acid has a pH of 5. What is the value of Ka for the acid?

a)

1 × 10–10

b)

1 × 10–7

c)

1 × 10–5

d)

1 × 10–2

20.

Which is a strong acid?

a)

12.0 M HNO2

b)

10.0 M H2SO3

c)

5.0 M HI

d)

5.0 M HF

21.

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

22.

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

a)

Acid

b)

Base

c)

Neutral

23.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
24.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
25.
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
26.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

27.

If we dissolve 20.0 grams of HCl in 1.2 L of water, what is the pH of that solution?

a)

0.34

b)

4.21

c)

7.20

d)

10.34

28.

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

29.

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

30.

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

31.

What is the difference between a conjugate Brønsted–Lowry acid–base pair?

a)

Electron pair

b)

Positive charge

c)

Proton

d)

Hydrogen atom

32.

Which is an example of an amphiprotic species?

a)

Al2O3

b)

CO32−

c)

P4O10

d)

HPO42−

33.

Which two species act as Brønsted–Lowry acids in the reaction?


H2PO4− (aq) + OH− (aq) ⇌

HPO42− (aq) + H2O (l)

a)

HPO42− (aq) and OH− (aq)

b)

H2PO4− (aq) and HPO42− (aq)

c)

HPO42− (aq) and H2O (l)

d)

H2PO4− (aq) and H2O (l)

34.

Which of the following is correct?

a)

A weak acid is a proton donor and its aqueous solution shows good conductivity.

b)

A weak acid is a proton donor and its aqueous solution shows poor conductivity.

c)

A weak acid is a proton acceptor and its aqueous solution shows good conductivity.

d)

A weak acid is a proton acceptor and its aqueous solution shows poor conductivity.

35.

Which species acts as a Lewis and Brønsted–Lowry base?

a)

[Al(H2O)6]3+

b)

BF3

c)

NH4+

d)

OH−

36.

Which species behave as Brønsted–Lowry bases in the following reaction?


H2SO4 + HNO3 H2NO3+ + HSO4-

a)

HNO3 and HSO4-

b)

HNO3 and H2NO3+

c)

H2SO4 and HSO4-

d)

H2NO3+ and HSO4-

37.

Which is a conjugate Brønsted–Lowry acid-base pair?

a)

CH3COO− / H3O+

b)

H2O / CH3COO−

c)

H2O / H3O+

d)

CH3COOH / H2O

38.

Which of the following is an example of a Lewis acid–base reaction, but not a Brønsted–Lowry acid–base reaction?

a)

2CrO2−4(aq) + 2H+(aq) →

Cr2O2−7(aq) + H2O(l)

b)

Co(H2O)2+6(aq) + 4HCl(aq) →

CoCl2−4(aq) + 4H+(aq) + 6H2O(l)

c)

NH3(aq) + H+(aq) →

NH+4(aq)

d)

CH3COO−(aq) + H2O(l) →

CH3COOH(aq) + OH−(aq)

39.

Consider the equilibrium below.

CH3CH2COOH(aq) + H2O(l) ⇌ CH3CH2COO−(aq) + H3O+(aq)


Which species represent a conjugate acid-base pair?

a)

CH3CH2COOH and H2O

b)

H2O and CH3CH2COO−

c)

H3O+ and H2O

d)

CH3CH2COO− and H3O+

40.

With which do most acids react?

I. sodium hydrogen carbonate

II. magnesium

III. calcium sulfate

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

41.

What are the products of the reaction between sulfuric acid and sodium hydrogen carbonate?

a)

NaSO4 + H2O + CO2

b)

Na2SO4 + CO2

c)

Na2SO4 + H2O + CO2

d)

NaSO4 + H2CO3

42.

Which solution is basic at 25 °C?

Kw = 1.0 × 10−14

a)

[H+] = 1.0 × 10−3 mol dm−3

b)

[OH−] = 1.0 × 10−13 mol dm−3

c)

solution of pH = 4.00

d)

[H3O+] = 1.0 × 10−13 mol dm−3

43.

What is the pH of 0.001 mol dm−3 NaOH (aq)?

a)

1

b)

3

c)

11

d)

13

44.

What is the pH of a solution in which the hydroxide ion concentration is 1 × 10−11 mol dm−3 at 298 K?

Kw = 1 × 10−14 at 298 K

a)

3

b)

7

c)

11

d)

14

45.

10.0 cm3 of an aqueous solution of sodium hydroxide of pH = 10 is mixed with 990.0 cm3 of distilled water. What is the pH of the resulting solution?

a)

8

b)

9

c)

11

d)

12

46.

A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must be correct?

a)

The [H+] in the solution of HY is 2 times GREATER than the [H+] in the solution of HX.

b)

The [H+] in the solution of HY is 100 times GREATER than the [H+] in the solution of HX.

c)

The [H+] in the solution of HY is 2 times LESS than the [H+] in the solution of HX.

d)

The [H+] in the solution of HY is 100 times LESS than the [H+] in the solution of HX.

47.

The pH of a solution changes from pH=2 to pH=5. What happens to the concentration of the hydrogen ions during this pH change?

a)

It decreases by a factor of 1000

b)

It increases by a factor of 1000

c)

It decreases by a factor of 100

d)

It increases by a factor of 100

48.

An example of a strong acid solution is perchloric acid, HClO4, in water. Which statement is correct for this solution?

a)

HClO4 is completely dissociated in the solution.

b)

HClO4 exists mainly as molecules in the solution.

c)

The solution reacts only with strong bases.

d)

The solution has a pH value greater than 7.

49.

What is the correct expression for the ionic product constant of water, Kw?

a)

Kw=[H+][OH−]K_w=\frac{\left[H^+\right]}{\left[OH^-\right]}

b)

Kw=[H2O][H+][OH−]K_w=\frac{\left[H_2O\right]}{\left[H^+\right]\left[OH^-\right]}

c)

Kw=[H+]+[OH−]K_w=\left[H^+\right]+\left[OH^-\right]

d)

Kw=[H+][OH−]K_w=\left[H^+\right]\left[OH^-\right]

50.

What is the order of increasing pH for the following solutions of the same concentration?

a)

HCl (aq) < NH3 (aq) < NaOH (aq) < CH3COOH (aq)

b)

CH3COOH (aq) < HCl (aq) < NH3 (aq) < NaOH (aq)

c)

HCl (aq) < CH3COOH (aq) < NH3 (aq) < NaOH (aq)

d)

NaOH (aq) < NH3 (aq) < CH3COOH (aq) < HCl (aq)

51.

Which statement is correct?

a)

A strong acid is a good proton donor and has a strong conjugate base.

b)

A weak acid is a poor proton acceptor and has a strong conjugate base.

c)

A strong acid is a good proton donor and has a weak conjugate base.

d)

A strong base is a good proton donor and has a weak conjugate acid.

52.

Which 1.0 moldm–3 solution has the highest pH?

a)

Ammonium chloride

b)

Sulfuric acid

c)

Sodium chloride

d)

Ammonia

53.

Which compound is a strong acid?

a)

NH3

b)

HNO3

c)

H2CO3

d)

CH3COOH

54.

Which group of three compounds contains only weak acids and bases?

a)

A

b)

B

c)

C

d)

D

55.

Which list contains only strong bases?

a)

ammonia, sodium hydroxide, ethylamine

b)

potassium hydroxide, ammonia, sodium hydroxide

c)

lithium hydroxide, potassium hydroxide, barium hydroxide

d)

ammonia, ethylamine, barium hydroxide

56.

A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?

a)

Acid A is stronger than acid B.

b)

[A] > [B].

c)

The concentration of H+ ions in A is higher than in B.

d)

The concentration of H+ ions in B is twice the concentration of H+ ions in A.

57.

Which of the following are weak acids in aqueous solution?

I. CH3COOH

II. H2CO3

III. HCl

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

58.

For equal volumes of 1.0 moldm−3 solutions of hydrochloric acid, HCl(aq), and methanoic acid, HCOOH(aq), which statements are correct?

I. HCl dissociates more than HCOOH

II. HCl is a better electrical conductor than HCOOH

III. HCl will neutralize more NaOH than HCOOH

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

59.

Which list contains only strong acids?

a)

CH3COOH, H2CO3, H3PO4

b)

HCl, HNO3, H2CO3

c)

CH3COOH, HNO3, H2SO4

d)

HCl, HNO3, H2SO

60.

Which molecule is acting as a base in the following reaction?

OH– + NH4+ → H2O + NH3

a)

OH–

b)

NH4+

c)

H2O

d)

NH3

61.

What is the pH of a solution that has an [H+] of 2.5 × 10–5?

a)

4.60

b)

5.0

c)

2.5

d)

7

62.

What is the pOH of a solution where the [OH–] is 7.3 × 10–2 M?

a)

-1.14

b)

2.0

c)

1.14

d)

7.3

63.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
64.

What is the pOH of a solution where the [H+] is 2.5 × 10–12 M?

a)

11.6

b)

2.40

c)

12

d)

2.5

65.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
66.
When a hydrogen ion is released what does the solution become?
a)
Basic
b)
Acidic
c)
Amphoteric
d)
Proton
67.
When a hydroxide ion is released what does the solution become?
a)
Basic
b)
Acidic
c)
Amphoteric
d)
Proton
68.
Which of the following represents the chemical formula for hydronium?
a)
H2O
b)
H+
c)
H3O+
d)
OH-
69.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

70.
When the chemical reaction A + B ↔ C+ D is at equilibrium,
a)
both the forward and reverse reactions have stopped.
b)
the sum of the concentrations of A and B equals the sum of the concentrations of C and D.
c)
all four concentrations are equal.
d)
neither the forward nor the reverse reactions have stopped.
71.

A solution with a pOH of 4.23. Is this solution acidic or basic?

a)

Acidic

b)

Basic

c)

Neutral

72.

Water can act as both an acid and a base in an ionization reaction to form H+ and OH– ions. What is this phenomenon called?

a)

neutralization

b)

auto-ionization

c)

base dissociation

d)

acid dissociation

73.
Why is equilibrium called a dynamic state?
a)
Chemists try to convert as much reactants as possible into products.
b)
The reactions at equilibrium continue to take place once equilibrium is established.
c)
The products of a forward reaction are favored, so equilibrium lies to the right.
d)
All chemical reactions are considered to be reversible under suitable conditions.
74.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
75.

Complete the following reaction:

H3PO4 + NaOH -->

a)

Na3PO4 + H2O

b)

Na +H2O

c)

Na3PO4 + H2

d)

Na3PO4 + H2O + CO2

76.
What are the weak acids and bases?
a)
all acids and bases are weak
b)
if not classified as strong, the acid/base is considered weak
c)
all acids and bases are strong
d)
there are more strong acids and bases than there are weak acids/bases
77.
What are the products of the following reaction?
H2SO4  +  KOH  -->  
a)
HK  +  HSO4
b)
H2O  +  KSO4
c)
H2O  +  K2SO4
d)
H2  +  K2SO4
78.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
79.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

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