Deck 11: Acids and Bases

Question 1

Which of the following is the strongest acid?

A)H₃
PO₄
B)NH₄
+
C)NaOH
D)H2CO₃
E)HCl

Answer 1

HCl

Question 2

According to the Arrhenius concept, if HNO₃ were dissolved in water, it would act as

A)a base.
B)an acid.
C)a source of hydroxide ions.
D)a source of H- ions.
E)a proton acceptor.

Answer 2

an acid.

Question 3

According to the Brønsted-Lowry definition,

A)an acid is a proton acceptor.
B)a base produces H+ ions in aqueous solutions.
C)a base is a proton donor.
D)a base is a proton acceptor.
E)an acid acts as the solvent.

Answer 3

a base is a proton acceptor.

Question 4

The name given to an aqueous solution of HNO₃ is

A)nitric acid.
B)nitrous acid.
C)hydrogen nitrate.
D)hydronitrogen acid.
E)hyponitric acid.

Question 5

The name given to an aqueous solution of HBr is

A)hydrogen bromide.
B)hydrobromic acid.
C)bromic acid.
D)bromous acid.
E)hypobromous acid.

Question 6

Identify the Brønsted-Lowry acids in the following reaction. H2O + CO₃ 2- → HCO₃ - + OH-

A)H2O/HCO₃
-
B)CO₃
2-/HCO₃
-
C)OH-/HCO₃
-
D)CO₃
2-/OH-
E)H2CO₃
/H2O

Question 7

The name given to an aqueous solution of HClO₃ is

A)chlorous acid.
B)hypochlorous acid.
C)chloric acid.
D)hydrochloric acid.
E)hypochloric acid.

Question 8

Which of the following is the weakest acid?

A)HF (Ka for HF is 7.2 × 10-4)
B)HCN (Ka for HCN is 4.9 × 10-10)
C)HCNO (Ka for HCNO is 2 × 10-4)
D)H₃
BO₃
(Ka for H₃
BO₃
Is 5.4 × 10-10)

Question 9

Which one of the following is characteristic of a base?

A)produces H₃
O+ in water
B)has a sour taste
C)has a slippery, soapy feel
D)turns blue litmus red
E)is insoluble in water

Question 10

The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is

A)neutral in water solution.
B)able to react with HCl.
C)a weak acid.
D)a strong acid.
E)ionic.

Question 11

The conjugate acid of HSO₄ - is

A)SO₄
2-.
B)HSO₄
.
C)H2SO₄
.
D)H2SO₄
-.
E)HSO₃
-.

Question 12

Which of the following is correctly identified?

A)NH₃
, strong acid
B)NaOH, strong base
C)HCl, weak acid
D)H2CO₃
, strong acid
E)Ca(OH)₂
, weak base

Question 13

The conjugate base of HClO₃ is

A)HClO2.
B)ClO₃
-.
C)Cl(OH)₂
.
D)ClO₃
.
E)HClO.

Question 14

According to the Arrhenius concept, if NaOH were dissolved in water, it would act as

A)a base.
B)an acid.
C)a source of hydronium ions.
D)a source of H- ions.
E)a proton donor.

Question 15

The correct formula for sulfuric acid is

A)H2SO₄
.
B)H2SO₃
.
C)H2SO₄
-.
D)H2SO₃
-.
E)SO₄
2-.

Question 16

The name of Al(OH)3 is

A)aluminum trihydroxide.
B)monoaluminum trihydroxide.
C)aluminum hydroxide.
D)aluminum(III)hydroxide.
E)aluminum oxygen hydride.

Question 17

Which of the following is the strongest base?

A)H₃
PO₄
B)NH₃
C)NaOH
D)NaCl
E)HCl

Question 18

The stronger the acid, the ________ the conjugate base.

A)stronger
B)weaker

Question 19

Which of the following is the strongest acid?

A)HF (Ka for HF is 7.2 × 10-4)
B)HCN (Ka for HCN is 4.9 × 10-10)
C)HCNO (Ka for HCNO is 2 × 10-4)
D)H₃
BO₃
(Ka for H₃
BO₃
Is 5.4 × 10-10)

Question 20

Ammonium hydroxide is a weak base because

A)it is a dilute solution.
B)it is only slightly soluble in water.
C)it cannot hold on to its hydroxide ions.
D)it dissociates only slightly in water.
E)it is completely ionized in aqueous solution.

Question 21

What is the pH of a solution with [OH-] = 1 × 10^-4 M?

A)10.0
B)-10.0
C)4.0
D)-4.0
E)1.0 × 10^-10

Question 22

What is the [OH-] in a solution that has a [ H₃ O+] = 1 × 10-6 M?

A)1 × 10-2 M
B)1 × 10-6 M
C)1 × 10-8 M
D)1 × 10-10 M
E)1 × 10-12 M

Question 23

What is the [ H₃ O+] in a solution that has a [OH-] = 5.0 × 10-2 M?

A)2.0 × 10-12 M
B)2.0 × 10-2 M
C)1.0 × 10-14 M
D)2.0 × 10-4 M
E)5.0 × 10-12 M

Question 24

The [ H₃ O+] of a solution with pH = 2 is

A)10 M.
B)-10 M.
C)1 × 102 M.
D)1 × 10-2 M.
E)1 × 10-12 M.

Question 25

What is the pH of a solution with [ H₃ O+] = 3.0 × 10^-3 M?

A)3.0 × 10^-3
B)2.52
C)3.0
D)-2.52
E)9.0

Question 26

In a sulfuric acid solution, where the [ H₃ O+] is 0.01 M, what is the pH?

A)pH = 12.0
B)pH = 2.0
C)pH = 3.0
D)pH = 11.0
E)pH = 5.0

Question 27

What is the [ H₃ O+] in a solution with [OH-] = 1 × 10-12 M?

A)1 × 10-12 M
B)1 × 102 M
C)1 × 10-7 M
D)1 × 10-8 M
E)1 × 10-2 M

Question 28

A solution which has [OH-] = 4.6 × 10-6 M is

A)acidic.
B)basic.
C)neutral.

Question 29

Predict whether the equilibrium of the following reaction favors reactants or products: NH₄ + + H2O ⇌ NH₃ + H₃ O+

A)Reactants are favored.
B)Products are favored.
C)Neither side is favored.

Question 30

Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?

A)In acids, [OH-] is greater than [ H₃
O+].
B)In bases, [OH-] = [ H₃
O+].
C)In neutral solutions, [ H₃
O+] = [ H2O].
D)In bases, [OH-] is greater than [ H₃
O+].
E)In bases, [OH-] is less than [ H₃
O+].

Question 31

What is the pH of a solution with [ H₃ O+] = 1 × 10^-9 M?

A)1.0 × 10^-5 M
B)-9.0
C)5.0
D)-5.0
E)9.0

Question 32

A solution with a pH of 4 is

A)extremely acidic.
B)moderately acidic.
C)neutral.
D)slightly basic.
E)extremely basic.

Question 33

In which of the following are the pH values arranged from the most acidic to the most basic?

A)1, 3, 6, 8, 11, 14
B)2, 5, 7, 9, 10, 1.1
C)14, 10, 7, 4, 3, 1
D)14, 10, 7, 1, 3, 5
E)7, 10, 14, 4, 3, 1

Question 34

The [ H₃ O+] of a solution with pH = 5.60 is

A)3 × 10-6 M.
B)2.5 × 10-8 M.
C)2.5 × 10-6 M.
D)4.0 × 10-6 M.
E)4.0 × 10-9 M.

Question 35

A solution which has [ H₃ O+] = 6.7 × 10-8 M is

A)acidic.
B)basic.
C)neutral.

Question 36

What is the pH of a solution with [OH-] = 2.0 × 10^-10 M?

A)9.70
B)-9.70
C)4.30
D)-4.30
E)2.0 × 10^-10

Question 37

In which of the following are the pH values arranged from the most basic to the most acidic?

A)1, 3, 6, 8, 11, 14
B)2, 5, 7, 9, 10, 11
C)14, 10, 7, 4, 3, 1
D)14, 10, 7, 1, 3, 5
E)7, 10, 14, 4, 3, 1

Question 38

What is the [OH-] in a solution that has a [ H₃ O+] = 2.0 × 10-4 M?

A)2.0 × 10-10 M
B)5.0 × 10-10 M
C)1.0 × 10-10 M
D)2.0 × 10-4 M
E)5.0 × 10-11 M

Question 39

For Kw, the product of [ H₃ O+] and [OH-] is

A)1.0 × 10-14.
B)1.0 × 10-7.
C)1.0 × 10-1.
D)1.0.
E)1.0 × 1014.

Question 40

A solution which has [OH-] = 3.4 × 10-12 M is

A)acidic.
B)basic.
C)neutral..

Question 41

When a piece of magnesium metal is added to hydrochloric acid, what gas is produced?

A)oxygen
B)chlorine
C)nitrogen
D)carbon dioxide
E)hydrogen

Question 42

The neutralization reaction between Al(OH)3 and HNO₃ produces the salt with the formula

A)H2O.
B)AlNO₃
.
C)AlH2.
D)Al(NO₃)3.
E)NO₃
OH.

Question 43

How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl?

A)50.0 mL
B)40.0 mL
C)0.100 mL
D)20.0 mL
E)10.0 mL

Question 44

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H₃ PO₄ ?

A)7.50 mL
B)2.50 mL
C)0.833 mL
D)5.00 mL
E)15.0 mL

Question 45

A 25.0 mL sample of H2SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H2SO₄ + 2KOH → K₂ SO₄ + 2H2O

A)2.00 M
B)2.50 M
C)0.800 M
D)1.60 M
E)1.25 M

Question 46

How many moles of H2O are produced when 1 mole of Mg(OH)₂ reacts with 1 mole of H2SO₄ ?

A)1
B)2
C)3
D)4
E)5

Question 47

Which of the following is a neutralization reaction?

A)KCl + NaNO₃
→ KNO₃
+ NaCl
B)HNO₃
+ KOH → H2O + KNO₃
C)H2O + SO₃
→ H2SO₄
D)4Na + O2 → 2Na2O
E)2NO2 → 2NO + O2

Question 48

What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution?

A)0.267 M
B)0.143 M
C)0.200 M
D)0.280 M
E)0.100 M

Question 49

An acid and base react to form a salt and water in a(n) ________ reaction.

A)ionization
B)dissociation
C)oxidation
D)neutralization
E)reduction

Question 50

Which of the following is the correctly balanced equation for the complete neutralization of H₃ PO₄ with Ca(OH)₂ ?

A)H₃
PO₄
+ Ca(OH)₂
→ CaHPO₄
+ 2H2O
B)3H₃
PO₄
+ Ca(OH)₂
→ Ca3(PO₄)₂
+ 5H2O
C)H₃
PO₄
+ Ca(OH)₂
→ Ca3(PO₄)₂
+ H2O
D)2H₃
PO₄
+ 3Ca(OH)₂
→ Ca3(PO₄)₂
+ 6H2O
E)4H₃
PO₄
+ 6Ca(OH)₂
→ 2Ca3(PO₄)₂
+ 12H2O

Question 51

In a neutralization reaction

A)two acids react to form water.
B)water and a salt react to form an acid and a base.
C)an acid and a salt react to form water and a base.
D)a base and a salt react to form water and an acid.
E)an acid and a base react to form a salt and water.

Question 52

A 10.0 mL of 0.121 M H2SO₄ is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is

A)0.207 M.
B)0.4141 M.
C)0.0708 M.
D)0.428 M.
E)0.142 M.

Question 53

The normal blood pH is about

A)6.8.
B)7.0.
C)7.2.
D)7.4.
E)7.6.

Question 54

In a neutralization reaction, how many moles of HClO₄ react with 1 mole of Al(OH)3?

A)1
B)2
C)3
D)4
E)5

Question 55

A 25.0 mL sample of H₃ PO₄ requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid? H₃ PO₄ + 3NaOH →Na3PO₄ + 3H2O

A)0.333 M
B)3.00 M
C)1.50 M
D)1.00 M
E)0.750 M

Question 56

For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution .
Mg(s) + 2HCl(aq) → MgCl₂
(aq) + H2(g)
If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?

A)1.65 M
B)80.0 M
C)8.00 M
D)0.823 M
E)3.29 M

Question 57

The [OH-] of a solution with pH = 8.34 is

A)5 × 10-9 M.
B)4.6 × 10-9 M.
C)2.2 × 10-9 M.
D)3 × 10-6 M.
E)2.2 × 10-6 M.

Question 58

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is

A)0.212 M.
B)0.115 M.
C)0.500 M.
D)0.390 M.
E)0.137 M.

Question 59

How many milliliters of 0.100 M Ba(OH)₂ are required to neutralize 20.0 mL of 0.250 M HCl?

A)100. mL
B)50.0 mL
C)25.0 mL
D)0.250 mL
E)0.50 mL

Question 60

The function of a buffer is to

A)change color at the end point of a titration.
B)maintain the pH of a solution.
C)be a strong base.
D)maintain a neutral pH.
E)act as a strong acid.

Question 61

The pH of 0.0001 M KOH is ________.

Question 62

If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?

Question 63

In a titration experiment, a student used 24.13 mL of 0.111 M sodium hydroxide to neutralize 20.00 mL of a hydrochloric acid solution. What was the molarity of the acid solution?

Question 64

Which solution has the highest pH?

A)a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate
B)a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate
C)a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate
D)a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate
E)All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

Question 65

If a condition of hyperventilation occurs, the blood pH of the patient is expected to

A)saturate.
B)increase.
C)decrease.
D)stay the same.
E)concentrate.

Question 66

What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30?

A)respiratory acidosis
B)respiratory alkalosis
C)metabolic acidosis
D)metabolic alkalosis
E)diabetes mellitus

Question 67

When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO₂, the blood pH rises in a condition called

A)metabolic acidosis.
B)metabolic alkalosis.
C)respiratory acidosis.
D)respiratory alkalosis.
E)pulmonary distress.

Question 68

A student had 25.0 mL of 0.100 M H2SO₄ solution. How many mL of a 0.100 M NaOH solution will the sulfuric acid neutralize?

Question 69

HCl is hydrochlorous acid.

Question 70

Which of the following is a buffer system?

A)NaCl and NaNO₃
B)HCl and NaOH
C)H2CO₃
And KHCO₃
D)NaCl and NaOH
E)H2O and HCl

Question 71

In a buffer system of HF and its salt, NaF,

A)the HF neutralizes added acid.
B)the HF neutralizes added base.
C)the HF is not necessary.
D)the F- neutralizes added H2O.
E)the F- neutralizes added base.

Question 72

What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?

Question 73

Identify the conjugate acid-base pairs in the following reaction:
HCl + NH₃ → NH₄ + + Cl-

Question 74

A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

Question 75

Which of the following could be a buffer?

A)NaF
B)HF + NaF
C)HF + H2O
D)NaF + H2O
E)NaCl + HF

Question 76

Which solution has the lowest pH?

A)a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate
B)a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate
C)a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate
D)a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate
E)All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

Question 77

The name of HCl is________.

Question 78

The conjugate acid of H₂PO₄ ^2- is ________.

Question 79

The pH of 0.0010 M HCl is ________.

Question 80

Write the proper Ka expression for the ionization of acetic acid, HC₂H₃O₂.