Chapter 11 Which of the following is correctly identified

General, Organic & Biological Chemistry, 5e (Timberlake)

Chapter 11 Acids and Bases

11.1 Multiple-Choice Questions

1) 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.

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.

3) 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.

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.

5) 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.

6) Which one of the following is characteristic of a base?

A) produces H3O+ in water

B) has a sour taste

C) has a slippery, soapy feel

D) turns blue litmus red

E) is insoluble in water

7) The correct formula for sulfuric acid is

A) H2SO4.

B) H2SO3.

C) H2SO4–.

D) H2SO3–.

E) SO42-.

8) The name of Al(OH)3 is

A) aluminum trihydroxide.

B) monoaluminum trihydroxide.

C) aluminum hydroxide.

D) aluminum(III) hydroxide.

E) aluminum oxygen hydride.

9) 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.

10) Identify the Brønsted-Lowry acids in the following reaction.

H2O + CO32- → HCO3– + OH–

A) H2O/HCO3–

B) CO32-/HCO3–

C) OH-/HCO3–

D) CO32-/OH–

E) H2CO3/H2O

11) The conjugate base of HClO3 is

A) HClO2.

B) ClO3–.

C) Cl(OH)2.

D) ClO3.

E) HClO.

12) The conjugate acid of HSO4– is

A) SO42-.

B) HSO4.

C) H2SO4.

D) H2SO4–.

E) HSO3–.

13) Which of the following is the strongest acid?

A) H3PO4

B) NH4+

C) NaOH

D) H2CO3

E) HCl

14) The stronger the acid, the ________ the conjugate base.

A) stronger

B) weaker

15) Which of the following is the strongest base?

A) H3PO4

B) NH3

C) NaOH

D) NaCl

E) HCl

16) 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

17) 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.

18) 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) H3BO3 (Ka for H3BO3 is 5.4 × 10–10)

19) 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)

20) 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.

21) 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.

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22) 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.

23) 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+] = [ H2O].

D) In bases, [OH–] is greater than [ H3O+].

E) In bases, [OH–] is less than [ H3O+].

24) 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

25) 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

26) 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

27) What is the [ H3O+] 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

28) A solution which has [ H3O+] = 6.7 × 10–8 M is

A) acidic.

B) basic.

C) neutral.

29) A solution which has [OH–] = 4.6 × 10–6 M is

A) acidic.

B) basic.

C) neutral.

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

A) acidic.

B) basic.

C) neutral..

31) A solution with a pH of 4 is

A) extremely acidic.

B) moderately acidic.

C) neutral.

D) slightly basic.

E) extremely basic.

32) 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

33) 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

34) 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

35) 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

36) 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.

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

38) 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

39) 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

40) The [ H3O+] 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.

41) 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.

42) 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

43) 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

44) 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.

45) 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 + 12H2O

46) 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.