Deck 10: Acids and Bases

Question 1

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.

Answer 1

hydrobromic acid.

Question 2

Which of the following is the strongest acid?

A) H3PO₄
B) NH4+
C) NaOH
D) H₂CO₃
E) HCl

Answer 2

HCl

Question 3

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

Answer 3

NaOH, strong base

Question 4

According to the Bronsted-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.

Question 5

Identify the Bronsted-Lowry acid in the following reaction. H₂O + CO₃2- → HCO₃- + OH-

A) H₂O
B) CO₃2-
C) HCO₃-
D) OH-
E) H₂CO₃

Question 6

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 7

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 × 10-10)
D) H3BO₃ (Ka for H3BO₃ is 5.4 × 10-10)

Question 8

Which one of the following is characteristic of a base?

A) produces H30+ in water
B) has a sour taste
C) has a slippery, soapy feel
D) turns blue litmus red
E) is insoluble in water

Question 9

The correct formula for sulfuric acid is

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

Question 10

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) H3BO₃ (Ka for H3BO₃ is 5.4 × 10-10)

Question 11

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 12

The stronger the acid, the __________ the conjugate base.

A) stronger
B) weaker

Question 13

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 14

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 15

According to the Arrhenius concept, if HNO₃were 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.

Question 16

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 17

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 18

Which of the following is the strongest base?

A) H3PO₄
B) NH3
C) NaOH
D) NaCl
E) HCl

Question 19

The conjugate acid of HSO₄- is

A) SO₄2-.
B) HSO₄.
C) H₂SO₄.
D) H₂SO₄-.
E) HSO₃-.

Question 20

The conjugate base of HClO₃ is

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

Question 21

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 22

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 23

What is the [OH-] in a solution that has a [H3O+] = 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 24

What is the [OH-] in a solution that has a [H3O+] = 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 25

Predict whether the equilibrium of the following reaction favors reactants or products: NH₄⁺ + H₂O ⇌ NH₃ + H₃O⁺

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

Question 26

What is the [H3O+] 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 27

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) NO₃OH.

Question 28

In a sulfuric acid solution, where the [H3O+] 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 29

For Kw, the product of [H3O+] 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 30

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 31

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

A) In acids, [OH-] is greater than [H₃O+].
B) In bases, [OH-] = [H₃O+].
C) In neutral solutions, [H₃O+] = [ $\mathrm { H } _ { 2 }$ O].
D) In bases, [OH-] is greater than [H₃O+].
E) In bases, [OH-] is less than [H₃O+].

Question 32

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 33

What is the pH of a solution with [H3O+] = 1 × 10-9 M?

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

Question 34

What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?

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

Question 35

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 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

A solution with a pH of 4 is

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

Question 38

Which of the following is the correctly balanced equation for the complete neutralization of H3PO₄ with Ca(OH)₂?

A) H3PO₄ + Ca(OH)₂→ CaHPO₄ + 2H₂O
B) 3H3PO₄ + Ca(OH)₂ → Ca₃(PO₄)₂ + 5H₂O
C) H3PO₄ + Ca(OH)₂ → Ca₃(PO₄)₂ + H₂O
D) 2H3PO₄ + 3Ca(OH)₂ → Ca₃(PO₄)₂ + 6H₂O
E) 4H3PO₄ + 6Ca(OH)₂ → 2Ca₃(PO₄)₂+ 12H3O

Question 39

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 40

The [H₃O⁺] 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 41

A 25.0 mL sample of H3PO₄ requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid? H3PO₄ + 3NaOH → Na3PO₄ + 3H₂O

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

Question 42

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 43

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 44

The normal blood pH is about

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

Question 45

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 46

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 → K2SO₄ + 2H₂O

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

Question 47

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

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

Question 48

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 49

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 50

How many milliliters of 0.100 M Ba(OH)₂are 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 51

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 52

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

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

Question 53

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 54

A major cause of acid rain is

A) CO₂ production.
B) CaCO₃ production.
C) SO₂ production.
D) NH3 production.

Question 55

Acid rain has a

A) pH < 7.
B) pH > 7.
C) pH < 6.2.
D) pH < 2.6.

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

Which of the following could be a buffer?

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

Question 58

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO₄?

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

Question 59

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 60

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 61

A solution with a pH of 4.0 is basic.

Question 62

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

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

Question 63

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

Question 64

HCl is hydrochlorous acid.

Question 65

A solution with a pH of 4.0 is more acidic than a solution with a pH of 6.0.

Question 66

HCl is a strong acid.

Question 67

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 68

The conjugate acid of HPO₄^2- is __________.

Question 69

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 70

The conjugate base of HCl is Cl-.

Question 71

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 72

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 73

Magnesium metal is not attacked by sulfuric acid solutions.

Question 74

In any water solution, [H₃O+] [OH-]= 1.0 × 10^-7.

Question 75

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

Question 76

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 77

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

Question 78

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 79

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

Question 80

The pH of 0.001 M HCl is 12.0.