Atoms and Elements Ch.3 Test Bank 2nd Edition

Student name:__________

MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
1) Which is present in all aqueous Brønsted acid solutions?

A) H ₂
B) H ⁺
C) OH ^–
D) H₂SO₄
E) Cl ^–

2) What is the name of a proton donor in an acid-base reaction?

A) Arrhenius acid
B) Arrhenius base
C) Brønsted acid
D) Brønsted base
E) Lewis base

3) What is the name of a proton acceptor in an acid-base reaction?

A) Arrhenius acid
B) Arrhenius base
C) Brønsted acid
D) Brønsted base
E) Lewis base

4) Which is a strong acid?

A) Ba(OH) ₂
B) H₃PO₄
C) HC₂H₃O₂
D) NaCl
E) HClO ₄

5) Identify the major ions present in an aqueous LiOH solution.

A) Li²⁺, O⁻, H⁻
B) Li⁺, OH⁻
C) LiO⁻, H⁺
D) Li⁺, O²⁻, H⁺
E) Li⁻, OH⁺

6) Identify the major ions present in an aqueous HNO3 solution.

A) HN²⁺, O²⁻
B) OH⁻, NO₃⁻
C) OH⁻, NO⁺
D) H⁺, N³⁻, O²⁻
E) H⁺, NO₃⁻

7) Which of the following is a weak acid?

A) H₂SO₄
B) HNO ₃
C) HF
D) HBr
E) HCl

8) Which of the following is a strong acid?

A) H₃PO₄
B) HNO ₃
C) HF
D) CH₃COOH
E) H₂O

9) Which of the following is a strong base?

A) NH ₃
B) Ca(OH) ₂
C) Al(OH) ₃
D) B(OH) ₃
E) CH₃OH

10) Which one of the following is a strong acid?

A) H₂CO₃
B) H₂SO₃
C) H₂SO₄
D) H₃PO₄
E) CH₃COOH

11) Which one of the following is a strong acid?

A) CH₃COOH
B) H₂SO₃
C) NH ₃
D) H₃PO₄
E) HClO ₃

12) The substance HClO4 is considered to be

A) a weak acid.
B) a weak base.
C) a strong acid.
D) a strong base.
E) neither acidic nor basic.

13) Which is a strong base?

A) LiOH
B) CH₃COOH
C) NH ₃
D) H₃PO₄
E) HClO ₂

14) The substance NH3 is considered to be

A) a weak acid.
B) a weak base.
C) a strong acid.
D) a strong base.
E) neither acidic nor basic.

15) The substance (CH3CH2)2NH is considered to be

A) a weak acid.
B) a weak base.
C) a strong acid.
D) a strong base.
E) neither acidic nor basic.

16) Which is a weak base?

A) NH ₃
B) Ca(OH) ₂
C) Ba(OH) ₂
D) NaOH
E) CH₃COOH

17) Which is the strongest acid?

A) HBrO ₄
B) HBr
C) HBrO ₂
D) HBrO
E) HBrO ₃

18) Which is the strongest acid?

A) HBrO ₃
B) HClO
C) HBrO ₂
D) HBrO
E) HClO ₃

19) Which is the strongest acid?

A) SO₄²⁻
B) H ₂SO ₃
C) H₂SO₄
D) HSO₄⁻
E) HSO₃⁻

20)

A) NaH(aq) + HOCl(aq); NaOH is the acid.
B) NaH(aq) + HOCl(aq); HCl is the acid.
C) NaCl(aq) + H₂O(l); NaOH is the acid.
D) NaCl(aq) + H₂O(l); HCl is the acid.
E) NaCl(aq) + H₂O(l); NaCl is the acid.

21)

A) Na(aq) + HOCl(aq); NaOH is the base.
B) NaCl(aq) + OH⁻(aq); HCl is the base.
C) NaCl(aq) + OH⁻(aq); NaOH is the base.
D) H ₂O( l) + NaCl( aq); HCl is the base.
E) NaCl(aq)+ H₂O(l); NaOH is the base.

22)

A) LiOH(aq) → Li⁺(aq) + OH⁻(aq)
B) HBr(aq) → H⁺(aq) + Br⁻(aq)
C) H⁺(aq) + OH⁻(aq) → H₂O(l)
D) Li⁺(aq) + Br⁻(aq) → LiBr(aq)
E) Li⁺(aq) + OH⁻(aq)+ H⁺(aq) + Br⁻(aq) → H₂O(l) + LiBr(aq)

23) What is the conjugate acid of the acetate ion?

A) CH₃O²⁻
B) COOH
C) HC₂H₃O₂
D) H₂O
E) CH ₄

24) What is the conjugate base of sulfuric acid?

A) HSO₄⁻
B) H ₃O ⁺
C) OH⁻
D) SO₄²⁻
E) H ₃SO ₄ ⁺

25) What is the conjugate base of water?

A) H₃O⁺
B) OH⁻
C) H₃O
D) OH
E) H₂O₂

26) What is the conjugate base of NH3?

A) NH ₂
B) NH₂⁺
C) NH₂⁻
D) NH ₄
E) NH₄⁺

27) What is the name given to a substance that can act as a Brønsted acid or as a Brønsted base according to what it is reacting with?

A) hydrophilic
B) hydrophobic
C) amphoteric
D) isoprotic
E) isoelectronic

28) What is [OH−] for a solution at 25°C that has [H3O+] = 2.35 × 10−3 M?

A) 4.26 × 10⁻⁵ M
B) 2.35 ×10⁻¹¹ M
C) 4.26 × 10⁻¹² M
D) 2.35 × 10⁻¹⁷ M
E) 2.35 ×10⁻³ M

29) What is the concentration of H+ in a 0.025 M HCl solution?

A) 0
B) 0.013 M
C) 0.025 M
D) 0.050 M
E) 0.010 M

30) What is the concentration of OH− in a 0.083 M NaOH solution?

A) 0.083 M
B) 1.21 × 10⁻¹³ M
C) 8.30 × 10⁻¹⁶ M
D) 7 M
E) 8.30 × 10¹² M

31) What is the concentration of OH− in a 1.0 × 10−3 M Ba(OH)2 solution?

A) 0.50 × 10⁻³ M
B) 1.0 × 10⁻³ M
C) 2.0 × 10⁻³ M
D) 1.0 × 10⁻² M
E) 3.3 × 10⁻⁴ M

32) What is [OH−] for a solution at 25°C that has [H3O+] = 8.23 × 10−2 M?

A) 8.23 × 10⁻² M
B) 1.22 × 10⁻⁶ M
C) 8.23 × 10⁻¹² M
D) 1.22 × 10⁻¹³ M
E) 8.23 × 10⁻¹⁶ M

33) What is the H+ ion concentration in a 2.1 × 10−4 M Ca(OH)2 solution?

A) 7.3 × 10⁻⁴ M
B) 4.2 × 10⁻⁴ M
C) 2.1 × 10⁻⁴ M
D) 2.4 × 10⁻¹¹ M
E) 4.8 × 10⁻¹¹ M

34) Which solution is the most acidic?

rev: 01_06_2017_QC_CS-72707

A) 3 ×10⁻⁴ M H⁺
B) 5 × 10⁻² M H⁺
C) 6 × 10⁻³ M H⁺
D) 1 × 10⁻⁶ M H⁺
E) 5 × 10⁻² M H⁺

35) Which solution is the most acidic?

A) 1 × 10⁻⁴ M H⁺
B) 1 × 10⁻⁹ M H⁺
C) 1 × 10⁻³ M H⁺
D) 1 × 10⁻⁷ M H⁺
E) 1 × 10⁻¹⁰ M H⁺

36) Which solution is the most acidic?

A) pH = 1.00
B) pH = 10.00
C) pH = 5.00
D) pH = 3.00
E) pH = 4.00

37) Which solution is basic?

A) pH = 1.00
B) pH = 10.00
C) pH = 5.00
D) pH = 3.00
E) pH = 4.00

38) A solution with a pH of 8.15 is

A) slightly acidic.
B) very basic.
C) neutral.
D) very acidic.
E) slightly basic.

39) Which one of these responses is true with regard to a 0.1 M solution of a weak acid HA?

A) [H⁺] > 0.1 M.
B) pH = 1.0
C) [H⁺] < [A^–]
D) pH > 1.0
E) [OH^–] > [H⁺]

40) What is the pH of a 0.056 M HNO3 solution?

A) 0.056
B) 1.25
C) 12.75
D) 2.88
E) 11.11

41) What is the pH of a solution in which [H+] is 1.22 ×10−4 M?

A) −3.914
B) 1.220
C) 3.914
D) 4.000
E) 4.086

42) What is the pH of a 0.056 M HNO3 solution?

A) 0.056
B) 1.25
C) 12.75
D) 2.88
E) 11.11

43) What is the pH of a 0.050 M LiOH solution?

A) 1.30
B) 3.00
C) 11.00
D) 12.39
E) 12.70

44) What is the pH of a 0.014 M Ca(OH)2 solution?

A) 1.85
B) 1.55
C) 12.15
D) 12.45
E) 15.85

45) What is the pOH of a 0.025 M HI solution?

A) 0.025
B) 0.94
C) 1.60
D) 12.40
E) 10.31

46) What is the pOH of a 0.0085 M KOH solution?

A) 2.07
B) 4.85
C) 9.15
D) 11.93
E) 0.0085

47) What is the [H+] in a solution with a pH of 5.63?

A) 2.344 × 10⁻⁶ M H⁺
B) 2.344 × 10⁻⁵ M H⁺
C) 5.63 M H⁺
D) 2.3 × 10⁻⁶ M H⁺
E) 2.3 × 10⁻⁵ M H⁺

48) The pH of a Ba(OH)2 solution is 10.00. What is the H+ ion concentration of this solution?

A) 4.0 × 10⁻¹¹ M
B) 1.6 × 10⁻¹⁰ M
C) 1.3 × 10⁻⁵ M
D) 1.0 × 10⁻¹⁰ M
E) 10.00 M

49) What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

A) 2.34 × 10⁻⁴ M
B) 2.29 × 10⁻⁶ M
C) 4.37 × 10⁻⁹ M
D) 4.27 × 10⁻¹¹ M
E) 8.360 M

50) After a substance acting as a strong base reacts, what remains of the base?

A) a weaker base
B) a strong conjugate acid
C) a strong conjugate base
D) a strong acid
E) a weak conjugate acid

51) After a substance acting as a strong acid reacts, what remains of the acid?

A) a weak conjugate base
B) a strong conjugate base
C) a strong conjugate acid
D) a strong acid
E) a weak conjugate acid

52) HCO₃⁻ + SO₄²⁻

A) HCO₃⁻
B) HSO₄⁻
C) OH⁻
D) H ₃O ⁺
E) SO₄²⁻

53) HCO₃⁻ + SO₄²⁻

A) HSO₄⁻
B) CO₃²⁻
C) OH⁻
D) H₃O⁺
E) SO₄²⁻

54) In the reaction, HSO4−(aq) + OH−(aq)SO42−(aq) + H2O(l), the conjugate acid-base pairs are

pair 1 pair 2

A) HSO₄⁻ and SO₄²⁻;H₂O and OH⁻.
B) HSO₄⁻ and H₃O⁺;SO₄^{2 −} and OH⁻.
C) HSO₄⁻ and OH⁻;SO₄^{2 −} and H₂O.
D) HSO₄⁻ and H₂O;OH ⁻ and SO₄²⁻.
E) HSO₄⁻ and OH⁻;SO₄^{2 −} and H₃O⁺.

55) H₂CO₃ + PO₄³⁻

A) H ₂O
B) HCO₃⁻
C) H₂CO₃
D) PO₄³⁻
E) None of the answers is correct.

56) A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid in the original solution?

A) 0.243 M
B) 0.200 M
C) 1.13 M
D) 0.563 M
E) 0.0313 M

57)

A) 0.045 L
B) 0.28 L
C) 0.56 L
D) 0.90 L
E) 1.1 L

58) Vinegar is a solution of acetic acid, HC2H3O2, dissolved in water. A 5.54-g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?

A) 0.0543%
B) 1.08%
C) 3.26%
D) 5.43%
E) 9.23%

59) A 34.62-mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H2SO4 solution. What is the concentration of the original sulfuric acid solution?

A) 0.0229 M
B) 0.218 M
C) 0.0523 M
D) 0.209 M
E) 0.105 M

60) During a titration, it is found that 53.5 mL of a solution of NaOH is needed to neutralize a solution that contains 1.86 g of HCl. What is the concentration of the NaOH solution?

A) 0.051 M
B) 0.686 M
C) 1.05 M
D) 0.035 M
E) 0.953 M

61) What volume of a 0.442 M NaOH solution is needed to neutralize 65.0 mL of a 0.296 M solution of HNO3?

A) 8.71 mL
B) 21.8 mL
C) 43.5 mL
D) 87.1 mL
E) 174 mL

62) What volume of a 0.452 M NaOH solution is needed to neutralize 85.0 mL of a 0.176 M solution of H2SO4?

A) 218.3 mL
B) 66.2 mL
C) 38.4 mL
D) 436.6 mL
E) 33.1 mL

63) A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. Which statement about the solution is correct?

A) The solution is basic.
B) The solution is neutral.
C) The solution is acidic.
D) The concentrations of fluoride ions and sodium ions are equal.
E) The concentrations of hydronium ions and hydroxide ions are equal.

64) Which one of these salts will form a basic solution upon dissolving in water?

A) NaCl
B) NaNO ₂
C) NH₄NO₃
D) KBr
E) AlCl ₃

65) Which one of these salts will form an acidic solution upon dissolving in water?

A) LiBr
B) NaF
C) NH₄Br
D) KOH
E) NaCN

66) Which results in a buffered solution?

A) a solution containing a strong acid and its conjugate base
B) a solution containing a strong base and its conjugate acid
C) a solution containing a catalyst
D) a solution containing two organic liquids
E) a solution containing a weak acid and its conjugate base

67) Which pair of substances could form a buffered aqueous solution?

A) HCl, NaCl
B) HNO₃, NaNO₃
C) H₃PO₄, NaH₂PO₄
D) H₂SO₄, CH₃COOH
E) NH₃, NaOH

68) Which pair of substances cannot form a buffered aqueous solution?

A) HCN and KCN
B) NH₃ and (NH₄)₂SO₄
C) HNO ₃ and NaNO ₃
D) HF and NaF
E) HNO ₂ and NaNO ₂

69) Which pair of substances is capable of forming a buffer in aqueous solution?

A) H₃PO₄, Na₃PO₃
B) HNO₃, NaNO₃
C) HCl, NaCl
D) H₂CO₃, NaNO₂
E) CH ₃COOH, CH ₃COONa