Ch 14 Acids and Bases STUDY GUIDE Accelerated Chemistry

Ch 14 Acids and Bases STUDY GUIDE Accelerated Chemistry SCANTRON

Name___________________________________ No-Calculators Allowed /99

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) Which of the following is NOT a property of acids? 1)A) Acids dissolve many metals.B) Acids turn litmus paper red.C) Acids have a sour taste.D) Acids have a slippery feel.E) All of the above are properties of acids.

2) Which of the following statements about acids are TRUE?1. An acid is used in car batteries.2. The active ingredient of vinegar is an acid.3. Acids are used for cleaning metals.

2)

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) All of 1, 2, and 3E) Neither 1, 2, or 3

3) Carboxylic acids can be found in 3)A) lemons.B) apples.C) grapes.D) all of the aboveE) none of these

4) Which among the following acids is commonly used for etching and frosting glass? 4)A) Nitric acidB) Hydrobromic acidC) Hydrofluoric acidD) Hydrochloric acidE) All of the above are used.

5) Which of the following acids is commonly used for manufacturing fertilizer? 5)A) HBrB) HNO3C) HFD) HClE) all of the above

6) Which of the following is NOT a property of bases? 6)A) Bases have a bitter taste.B) Bases dissolve many metals.C) Bases turn litmus paper blue.D) Bases have a slippery feel.E) All of the above are properties of bases.

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7) Which of the following statements about a base are TRUE?1. Bases are used in the manufacturing of soap.2. Bases have a sour taste.3. Fertilizer manufacture and cotton processing use bases.

7)

A) 1 and 2 onlyB) 2 and 3 onlyC) 1 and 3 onlyD) All of 1, 2, and 3E) Neither 1, 2, or 3

8) Which of the following common bases is commonly used for manufacturing fertilizer? 8)A) NaOHB) NaHCO3C) KOHD) NH3E) all of the above

9) Which of the following is the active ingredient of baking soda? 9)A) KOHB) NH3C) NaHCO3D) NaOHE) none of the above

10) The Arrhenius definition of an acid is: 10)A) a proton donor.B) produces H in solution.C) a proton acceptor.D) produces OH in solution.E) none of the above

11) The Bronsted-Lowry definition of a base is: 11)A) a proton donor.B) produces OH in solution.C) produces H in solution.D) a proton acceptor.E) none of the above

12) The Bronsted-Lowry definition of an acid is: 12)A) a proton donor.B) produces OH in solution.C) produces H in solution.D) a proton acceptor.E) none of the above

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13) Which of the following is NOT true? 13)A) The Bronsted-Lowry Model applies to a wider range of acid-base phenomena than does

the Arrhenius Model.B) The Bronsted-Lowry Model can apply to bases that do not contain hydroxide ions.C) The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry

Model.D) The Arrhenius Model of acids and bases applies toward substances that are nonaqueous.E) none of the above

14) In examining the formula for acetic acid, HC2H3O2, the ionizable hydrogen atom(s) is/are 14)A) all of the H's on the right-side.B) the H on the left.C) all four H's.D) one of the H's on the right-side.E) none of the above.

15) Which of the following is NOT an acid-base conjugate pair? 15)A) H2S and OH-

B) H2CO3 and HCO3-

C) H2O and OH-

D) NH4+ and NH3E) none of the above

16) In the following reaction:HCO3- (aq) + H2O (aq) H2CO3 (aq) + OH- (aq)

16)

A) HCO3- is an acid and H2CO3 is its conjugate base.B) H2O is an acid and HCO3- is its conjugate base.C) HCO3- is an acid and OH- is its conjugate base.D) H2O is an acid and OH- is its conjugate base.E) H2O is an acid and H2CO3 is its conjugate base.

17) In the following reaction: NH4+ (aq) + H2O (aq) NH3 (aq) + H3O+ (aq) 17)A) H2O is a base and NH3 is its conjugate acid.B) NH4+ is an acid and H3O+ is its conjugate base.C) NH4+ is an acid and H2O is its conjugate base.D) NH4+ is a base and H2O is its conjugate acid.E) H2O is a base and H3O+ is its conjugate acid.

18) What is the conjugate acid of OH ? 18)A) H2OB) NaOHC) O2-

D) OHE) none of the above

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19) What is the conjugate base of H2O? 19)A) OHB) O2-

C) NaOHD) H3O+

E) none of the above

20) A substance that acts as an acid or a base is called 20)A) isoprotic.B) amphoteric.C) a salt.D) hydrophillic.E) none of the above

21) What are the products of a neutralization reaction? 21)A) carbon dioxide and waterB) water and saltC) oil and waterD) salt and carbon dioxideE) none of the above

22) When an acid reacts with a metal, what is one of the usual products? 22)A) waterB) saltC) hydrogen gasD) carbon dioxideE) none of the above

23) A neutralization reaction between an acid and sodium hydroxide formed water and the saltnamed sodium sulfate. What was the formula of the acid that was neutralized?

23)

A) HClB) Na2SO4C) H2SO4D) H2SE) none of the above

24) A 25.0 ml sample of 0.105 M HCl was titrated with 31.5 ml of NaOH. What is the concentrationof the NaOH?

24)

A) 0.132 MB) 0.075 MC) 0.0833 MD) 0.105 ME) none of the above

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25) A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH. What is theconcentration of the KOH?

25)


26) Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H2SO4 solution?GIVEN: H2SO4 (aq) + 2NaOH (aq) 2H2O (l) + Na2SO4 (aq)

26)


27) Pure water cannot conduct electricity so why do we have to be careful with electricalappliances near water?

27)

A) Water dissociates fully into its ions.B) Water can be broken down by electricity.C) Water always has some ions dissolved in it.D) OSHA regulationsE) none of the above

28) Which of the following acids is diprotic? 28)A) HNO3B) HIC) H2SO4D) HClO4E) none of the above

29) Which of the following acids is a diprotic, weak acid? 29)A) carbonic acidB) phosphoric acidC) sulfuric acidD) hydrobromic acidE) none of the above

30) Which of the following acids is a monoprotic, strong acid? 30)A) sulfuric acidB) carbonic acidC) phosphoric acidD) hydrobromic acidE) none of the above

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31) A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is: 31)A) a strong base.B) a weak acid.C) a weak base.D) a strong acid.E) none of the above

32) What is the concentration of H in 2.0 M acetic acid, HC2H3O2? 32)A) 2.0 MB) 1.0 MC) < 2.0 MD) >2.0 ME) none of the above

33) What is the concentration of H in 0.50 M hydroiodic acid? 33)A) <0.50 MB) 1.50 MC) 1.0 MD) 0.50 ME) none of the above

34) Which of the following is a weak base? 34)A) potassium hydroxideB) sodium fluorideC) ammoniaD) calcium hydroxideE) none of the above

35) Ammonia (NH3) ionizes in water to form a basic solution. What is the concentration of OH-

ions in a 0.75 M NH3 solution?35)

A) No OH- ions exist in a solution of NH3.B) < 0.75 MC) > 0.75 MD) 0.75 ME) none of the above

36) Consider a 1.6 × 10-3 M solution of HNO3. Which of the following statements is NOT true? 36)A) This solution could neutralize a base.B) This solution has a pH of 11.20.C) This solution would turn litmus to red.D) This solution could dissolve metal.E) none of the above

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37) Substances that can act both as an acid and as a base are called: 37)A) buffers.B) amphoteric.C) neutral.D) indicators.E) none of these

38) What is the concentration of the hydronium ions in a neutral solution? 38)A) > 1.0 × 10-7 MB) < 1.0 × 10-7 MC) 1.0 × 10-7 MD) 1.0 × 10-14 ME) 0.0 M

39) What is the concentration of the hydroxide ions in an acidic solution? 39)A) < 1.0 × 10-7 MB) 1.0 × 10-14 MC) > 1.0 × 10-7 MD) 1.0 × 10-7 ME) 0.0 M

40) What is the concentration of the hydronium ions in an acidic solution? 40)A) 1.0 × 10-14 MB) < 1.0 × 10-7 MC) 1.0 × 10-7 MD) 0.0 ME) > 1.0 × 10-7 M

41) What is the value of the ion product constant for water (Kw)? 41)A) 1.0 × 1014

B) 1.0 × 107C) 0.0D) 1.0 × 10-7

E) 1.0 × 10-14

42) What is the concentration of the hydroxide ion given that the concentration of the hydroniumion is 1.5 × 10-5 M?

42)

A) 1.5 × 109 MB) 6.7 × 10-10 MC) 1.0 × 10-19 MD) 1.0 × 10-14 ME) none of the above

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43) What is the concentration of hydronium ions in a solution given that the concentration ofhydroxide ions is 2.31 × 10-4 M?

43)

A) 1.01 × 10-5 MB) 2.31 × 10-18 MC) 4.33 × 10-11 MD) 2.31 × 1010 ME) none of the above

44) Which solution below has the highest concentration of hydroxide ions? 44)A) pH = 12.49B) pH = 7.00C) pH = 7.93D) pH = 10.12E) pH = 3.21

45) The pH of a solution is 5.00. Which of the following is TRUE about the solution? 45)A) Its [H3O+] is 1.0 × 105 MB) Its [H3O+] is 1.0 × 10-5 MC) Its [H3O+] is 1.0 × 10-9 MD) It is more acidic than a solution whose pH is 4.00.E) none of the above

46) In order for a solution to be acidic, 46)A) [H3O+] > [OH-]B) [H3O+] < [OH-]C) [H3O+] = [OH-]D) pH = pOHE) none of the above

47) In order for a solution to be basic, 47)A) [H3O+] < [OH-]B) [H3O+] = [OH-]C) pH = pOHD) [H3O+] > [OH-]E) none of the above

48) In a solution that has a pH = 7.0, 48)A) [H3O+] > [OH-]B) [H3O+] + [OH-] = KwC) [H3O+] = [OH-]D) [H3O+] < [OH-]E) none of the above

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49) A solution at 25°C has a hydrogen ion concentration of 2.6 × 10-5 M. Which of the following isTRUE?

49)

A) [H3O+] > [OH-]

B) [H3O+] =[OH-]

Kw

C) [H3O+] < [OH-]D) [H3O+] = [OH-]E) none of the above

50) Which solution below is considered to have basic character? 50)A) pOH = 13B) pOH = 7C) pOH = 4D) pH = 2E) none of the above

51) What is the pH of a solution that has a H concentration equal to 1.7 × 10-5 M? 51)A) 0.22B) 4.77C) 10.20D) 5.20E) none of the above

52) If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydroniumion concentration?

52)

A) It became zero.B) It increased.C) It decreased.D) It became less than zero.E) none of the above

53) What is the pOH of a solution that has a OH- concentration equal to 1.3 × 10-10 M? 53)A) 4.12B) 4.29C) 9.89D) -4.3E) none of the above

54) What is the [H ] in a solution that has a pH of 3.35? 54)A) 1 × 103.35 MB) 3.35 × 10-14 MC) 2.2 × 103 MD) 4.5 × 10-4 ME) none of the above

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55) What is the [OH-] in a solution that has a pOH of 9.65? 55)A) 4.5 × 105 MB) 2.2 × 10-10 MC) 9.8 × 10-1 MD) 4.5 × 10-9 ME) none of the above

56) Which of the following is TRUE of alkaloid compounds? 56)A) Some alkaloids are addictive.B) Alkaloids are organic bases.C) Alkaloids occur naturally in many plants.D) Some narcotic drugs are alkaloids.E) All of the above are true.

57) A buffer solution is all of the following EXCEPT: 57)A) a solution that resists a change in pH when an acid is added.B) a solution that regulates pH by the addition of a strong acid or base.C) a solution that resists a change in pH when a base is added.D) a solution that contains both a weak acid and its conjugate base.E) All of the above are true.

58) Which of the following statements are TRUE of buffer solutions?1. A buffer solution can be made by mixing equal concentrations of

acetic acid and sodium acetate.2. A buffer solution can be made by mixing equal concentrations of

hydrochloric acid and sodium chloride.3. A buffer solution resists changes in pH when small quantities of acid

or base are added.

58)

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) All of 1, 2, and 3E) None of 1, 2, and 3

59) Which combination below will be a buffer solution? 59)A) HNO3 and NaNO3B) HC2H3O2 and NaC2H3O2C) NaBr and NaOHD) HCl and ClE) All of the above are true.

60) Which of the following contributes to acid rain? 60)A) The use of volatile acids in industry.B) The reaction of nonmetal oxides with water.C) The reaction of metal oxides with water.D) The reaction of alkali metals with water.E) all of the above

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61) Acid rain legislation targeted the release of which compound by industry? 61)A) dioxinB) benzeneC) CO2D) SO2E) none of the above

TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments bychanging the underlined word(s).

62) Acids have a bitter taste. 62)

63) Acids produce H ions in solution. 63)

64) Acids turn litmus paper blue. 64)

65) The main component of stomach acid is sulfuric acid. 65)

66) The main component of vinegar is acetic acid. 66)

67) Bases have a bitter taste. 67)

68) Bases feel slippery. 68)

69) Bases feel slippery because they react with oils on your skin to form soap-like substances. 69)

70) Sodium hydroxide is often used in the manufacturing of soap. 70)

71) The sour taste of bases warns humans against eating poisonous alkaloids found in someplants.

71)

72) An Arrhenius base is a proton acceptor. 72)

73) A Bronsted-Lowry acid is a proton donor. 73)

74) H is called the hydronium ion. 74)

75) A conjugate acid-base pair are two substances related to each other by the transfer of a proton. 75)

76) The conjugate base to HSO4- is SO42-. 76)

77) H2SO3 and H2SO4 are considered an acid-base conjugate pair. 77)

78) The products of a neutralization reaction are carbon dioxide and water. 78)

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79) The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has theformula Ca3P2.

79)

80) When a metal reacts with an acid it produces salt and water. 80)

81) Aluminum is one of the few metals that dissolves in a strong base. 81)

82) In a titration, the indicator is used to signal when the endpoint has been reached. 82)

83) A 100 mL sample of 4.0 M H2SO4 could be neutralized by 100 mL of 4.0 M NH3. 83)

84) A strong acid is one that completely dissociates into ions in solution. 84)

85) The equation HCl (aq) + H2O (l) H3O+ (aq) + Cl- (aq) properly depicts the behavior ofhydrochloric acid in water.

85)

86) A strong acid must also be a strong electrolyte. 86)

87) A strong acid is one that is very concentrated. 87)

88) In general, the stronger the acid, the weaker is its conjugate base. 88)

89) A neutral solution does not contain any H or OH . 89)

90) The ion product constant for water (Kw) is best stated as Kw = [H2O] [H+]. 90)

91) A solution of pH 2 contains ten times more H3O+ than a solution of pH 3. 91)

92) The pH of 0.001 M HCl is 3.0. 92)

93) The pH of a 0.0001 M NaOH solution is 4. 93)

94) A solution that has a pH of 8.5 is considered a weak base. 94)

95) A pH of 7 is equivalent to a pOH of 7. 95)

96) A solution that has a pH of 10 would also have a pOH of 4. 96)

97) A buffer resists a change in pH by being able to react with an acid or a base. 97)

98) The burning of fossil fuels produces nitrogen oxides and sulfur oxides which can react to formacid rain (nitric and sulfuric acids).

98)

99) Rain is naturally somewhat acidic because of atmospheric carbon dioxide. 99)

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Ch 14 Acids and Bases STUDY GUIDE Accelerated Chemistry