Deck 8: Acid and Bases

Question 1

Acidic materials can be identified by which of the following test outcomes:

A) They react with metals.
B) They feel slippery.
C) They may taste bitter.
D) They turn litmus paper red.
E) All of the above.

Answer 1

D

Question 2

Acidic materials typically react with some metals, such as calcium and aluminum, to form

A) insoluble salts.
B) red solutions.
C) hydrogen gas.
D) hydroxide ions.
E) all of the above.

Answer 2

C

Question 3

Common acidic materials are often easier to recognize than bases just from their chemical formula. Which answer below can explain this fact?

A) Acidic materials typically contain active hydrogen atoms.
B) Acidic materials are often ionic.
C) Acidic materials typically contain halogen atoms.
D) Acidic materials can contain ionic hydroxide groups.
E) all of the above.

Answer 3

A

Question 4

Which of the following statements regarding acids is true ?

A) All materials that contain hydrogen are acidic.
B) A bitter taste is an indicator for an acidic solution.
C) Acidic materials are poisonous.
D) Bases are more reactive than acids.
E) Litmus paper turns red in the presence of acids.

Question 5

Basic materials can be identified by which of the following test outcomes:

A) They form salts in the presence of acids.
B) They may feel slippery.
C) They may taste bitter.
D) They turn litmus paper blue.
E) All of the above.

Question 6

Which of the following statements regarding bases is true:

A) All materials that contain hydroxide are basic.
B) A sour taste is an indicator for an basic solution.
C) Litmus paper turns blue in the presence of bases.
D) Bases are more reactive than acids.
E) Basic materials are poisonous.

Question 7

A number of poets and famous quotations reference 'ashes in the mouth' as a way of describing something unpleasant, or bitter. What does this tell us about ashes?

A) They are acidic.
B) They are basic.
C) They are salts.
D) They are metals.
E) There is not enough information provided.

Question 8

Neutralization reactions typically produce which of the following:

A) water
B) salt
C) hydroxide
D) protons
E) a & b

Question 9

Carbon dioxide is produced in neutralizations that involve ______ .

A) water
B) salt
C) carbon
D) carbonate salts
E) vinegar

Question 10

What set of acid and base combinations below could be used to generate sodium iodide, NaI?

A) NaOH and HF
B) HIO₃ and Na₂CO₃
C) Na₂CO₃ and HI
D) NaOH and HI
E) both c & d

Question 11

Using the Brønsted-Lowry definition, when dissolved in water, what is the active component generated by compounds we consider to be acids?

A) H
B) H⁺
C) H₃O⁺
D) H₂
E) none of the above

Question 12

Which of the following would you expect to turn litmus paper red:

A) saliva
B) baking soda
C) grapefruit juice
D) sea salt
E) none of the above

Question 13

Which of the following would you expect to turn litmus paper blue:

A) chalk
B) baking soda
C) oven cleaner
D) all of the above
E) none of the above

Question 14

Which of the following is likely to behave as an acid:

A) CH₃CO₂H
B) NaHCO₃
C) CaCO₃
D) all of the above
E) none of the above

Question 15

Which of the following is likely to behave as a base:

A) NaOH
B) NaHCO₃
C) CaCO₃
D) all of the above
E) none of the above

Question 16

Which of the following statements is true:

A) Acid-base behavior can take place in the gas phase
B) All bases contain the OH- anion.
C) All acids contain the oxygen atom
D) Acids react with metals to release carbon dioxide gas.
E) All of the above are true.

Question 17

Two solutions, A and B, described below, were mixed together. Answer the following question regarding the solutions and the resulting mixture:
Solution A: 50 mL of 1.00 M aqueous HCl Solution B: 100 mL of 1.00 M NaOH
Before mixing, which of the following statements best describes the system:

A) The pH is greater in Solution B
B) The pH is greater in Solution A
C) The solutions are neutral.
D) None of the above are true.
E) All of the above are true.

Question 18

Two solutions, A and B, described below, were mixed together. Answer the following question regarding the solutions and the resulting mixture:
Solution A: 50 mL of 1.00 M aqueous HCl Solution B: 100 mL of 1.00 M NaOH
After mixing, which of the following statements best describes the mixture:

A) The pH of the mixture is greater than Solution B
B) The pH of the mixture is less than Solution A
C) The pH of the mixture is less than Solution B
D) The solutions are neutral.
E) All of the above are true.

Question 19

Magnesium bicarbonate, Mg(HCO₃)₂ , contains two bicarbonate ions. How many moles of hydrochloric acid, HCl would be required to completely neutralize 0.100 mol of the magnesium bicarbonate?

A) 0.050 mol
B) 0.100 mol
C) 0.200 mol
D) 1.00 mol
E) 2.00 mol

Question 20

Magnesium carbonate, MgCO₃ , contains one carbonate ions. How many moles of magnesium carbonate would be required to completely neutralize 0.100 mol of the hydrochloric acid, HCl?

A) 0.050 mol
B) 0.100 mol
C) 0.200 mol
D) 1.00 mol
E) 2.00 mol

Question 21

Which of the following statements describes the acid-base properties of water?

A) Water can act as an acid.
B) Water can act as a base.
C) Water can donate H⁺ ions.
D) Water can form OH^- ions.
E) all of the above.

Question 22

How would you describe the behavior of water act under the following conditions: in the presence of a base.

A) Water is neutral and is unreactive.
B) Water can split into two new molecules.
C) Water will donate H⁺ ions.
D) Water will form OH^- ions.
E) all of the above.

Question 23

How would you describe the behavior of water acting under the following conditions: in the presence of an acid.

A) Water is neutral and is unreactive.
B) Water can split into two new molecules.
C) Water can donate H⁺ ions to form OH^-.
D) Water can accept H⁺ ions to form H₃O⁺.
E) none of the above.

Question 24

Which of the following statements about pure water is true?

A) Water is composed of only H₂O molecules.
B) Water contains a larger number of OH^- ions than H₃O⁺ ions.
C) Water contains a larger number of H₃O⁺ ions than OH^- ions.
D) Water contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 25

Which of the following statements about acidic water is true?

A) Acid has no effect on the H₂O molecules.
B) The solution contains a larger number of OH^- ions than H₃O⁺ ions.
C) The solution contains a larger number of H₃O⁺ ions than OH^- ions.
D) The solution contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 26

Which of the following statements about basic water is true?

A) Base has no effect on the H₂O molecules.
B) The solution contains a larger number of OH^- ions than H₃O⁺ ions.
C) The solution contains a larger number of H₃O⁺ ions than OH^- ions.
D) The solution contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 27

Which of the following statements accurately describes a solution that has a pH = 5.4

A) It is not possible to answer without the identity of the solution.
B) The solution contains a larger number of OH^- ions than H₃O⁺ ions.
C) The solution contains a larger number of H₃O⁺ ions than OH^- ions.
D) The solution contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 28

Which of the following statements accurately describes a solution that has a pH = 10.3

A) It is not possible to answer without the identity of the solution.
B) The solution contains a larger number of OH^- ions than H₃O⁺ ions.
C) The solution contains a larger number of H₃O⁺ ions than OH^- ions.
D) The solution contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 29

Which of the following statements accurately describes a solution that has a pH = 7.0

A) It is not possible to answer without the identity of the solution.
B) The solution contains a larger number of OH^- ions than H₃O⁺ ions.
C) The solution contains a larger number of H₃O⁺ ions than OH^- ions.
D) The solution contains an equal number of H₃O⁺ ions and OH^- ions.
E) none of the above.

Question 30

What is the expected change in the pH under the following conditions: acid is added to the solution.

A) It is not possible to answer without the identity of the acid.
B) The pH will increase.
C) The pH will decrease.
D) The pH will stay the same.
E) The pH will fluctuate and then stabilize.

Question 31

What is the expected change in the pH under the following conditions: base is added to the solution.

A) It is not possible to answer without the identity of the acid.
B) The pH will increase.
C) The pH will decrease.
D) The pH will stay the same.
E) The pH will fluctuate and then stabilize.

Question 32

You accidentally forget to label a sample bottle with the correct pH. You decide to do a quick litmus test. The litmus paper turns blue. Which of the following pH values could your sample be?

A) pH = 3.0
B) pH = 5.0
C) pH = 7.0
D) pH = 9.0
E) None of the above.

Question 33

A strong acid solution has a concentration between 1.0 x 10^-4 M and 1.0 x 10^-6 M. Which of the following is a reasonable pH for the solution?

A) pH = 3.0
B) pH = 5.0
C) pH = 7.0
D) pH = 9.0
E) None of the above.

Question 34

Which of the following statements is true for a dilute weak acid solution:

A) The H₃O⁺ concentration will equal the anion concentration.
B) The H₃O⁺ concentration will equal the original acid concentration.
C) The OH^- concentration will be greater than the H₃O⁺ concentration.
D) All of the above.
E) None of the above.

Question 35

Which of the following pH values would correspond to a solution with an OH^- concentration of 1.0 x 10^-9?

A) pH = 3.0
B) pH = 5.0
C) pH = 7.0
D) pH = 9.0
E) None of the above.

Question 36

An unknown material has a pH of 3.0 and its concentration is found to be 0.00100 M. What can be said about the solution?

A) It contains a strong acid.
B) It contains a weak acid.
C) It contains a weak base.
D) It contains a strong base.
E) There is not enough information available to make an assessment.

Question 37

An unknown material has a pH of 8.0 and its concentration is found to be 0.00100 M. What can be said about the solution?

A) It contains a strong acid.
B) It contains a weak acid.
C) It contains a weak base.
D) It contains a strong base.
E) There is not enough information available to make an assessment.

Question 38

Many strong acids share a common feature that led early chemist to incorrectly identify this as " a single characteristic " of all acids: What is this feature?

A) They would smoke when exposed to air.
B) They were formed from 'burning' metals.
C) They contained halogens.
D) They contained oxygen.
E) None of the above

Question 39

Water isn't the only material to undergo ionization and recombination with itself. Under special conditions, typically nonaqueous conditions, other materials can 'self-ionize'. What would be the self ionization products of liquid hydrochloric acid?

A) H₂ and Cl₂
B) H₂O and HCl
C) H⁺ and Cl^-
D) H₂Cl⁺ and Cl^-
E) None of the above

Question 40

Metal carbonates are weak bases. They react with acids to release carbon dioxide. What does that mean regarding the metal ions that make up the carbonate salt?

A) The amount of metal ion in solution stays the same as pH changes.
B) The amount of metal ion in solution decreases as pH drops.
C) The amount of metal ion in solution increases as pH drops.
D) The amount of metal ion in solution depends on the strength of the acid.
E) None of the above

Question 41

Most naturally occurring freshwater has a pH between 7 and 5.6. This is due to dissolved, naturally occurring acids. Which is the most common acid associated with this process?

A) hydrochloric acid
B) carbonic acid
C) sulfuric acid
D) nitric acid
E) Both c and d

Question 42

Acid rain is precipitation that has a pH that is lower than 5.6. This is due to dissolved, man-made acids that arise from pollution. Which is the most common acid(s) associated with this process?

A) hydrochloric acid
B) carbonic acid
C) sulfuric acid
D) nitric acid
E) Both c and d

Question 43

What acidic functional group is very common in foods that are considered acidic?

A) carboxylic acid
B) hydroxyl group
C) carbonyl group
D) alpha-hydroxy group
E) Both c and d

Question 44

Which of the following is commonly used as a digestive antacid?

A) sodium hydroxide
B) ammonia
C) magnesium hydroxide
D) calcium carbonate
E) Both c and d

Question 45

What chemical characteristic is common for compounds used as digestive antacids?

A) They are weak bases.
B) They are weak acids.
C) They are strong acids.
D) They are strong bases.
E) They are buffers.

Question 46

What is the major source of carbonic acid found in naturally occurring waters?

A) metal carbonates
B) carbon dioxide
C) nitric acid
D) sulfur impurities in fossil fuels
E) Both c and d

Question 47

What happens to carbon dioxide gas when it dissolves in naturally occurring waters?

A) It forms metal carbonates.
B) It forms carbonic acid.
C) It is converted into nitric acid.
D) It becomes basic.
E) Gases do not dissolve readily in water.

Question 48

What chemical characteristic is common in polluting compounds released by combustion of fossil fuels?

A) They form weak bases.
B) They form weak acids.
C) They form strong acids.
D) They form strong bases.
E) They form buffers.

Question 49

Which compound is considered to be the leading cause of ocean acidification?

A) hydrochloric acid
B) carbonic acid
C) sulfuric acid
D) nitric acid
E) Both c and d

Question 50

Which of the following are the most likely side effects of ocean acidification?

A) a pH less than 7.0 in the ocean
B) more metal salts altering the ocean chemistry
C) dissolution of the shells of marine organisms
D) Both a & b
E) All of the above.

Question 51

Acid rain can harm soil chemistry by ________.

A) dissolving and leaching beneficial minerals
B) releasing harmful ions that are normally undissolved
C) removing beneficial hydroxide ions
D) Both a & b
E) All of the above.

Question 52

Which of the following is a trait of buffer:

A) adding a strong acid lowers the pH significantly
B) adding a strong acid raises the pH significantly
C) adding a strong acid doesn't significantly change the pH
D) Both a & c
E) None of the above.

Question 53

Which of the following is a trait of an unbuffered solution?

A) adding a strong acid lowers the pH significantly
B) adding a strong acid raises the pH significantly
C) adding a strong acid doesn't significantly change the pH
D) Both a & c
E) None of the above.

Question 54

One common biological buffer is the carbonic acid (H₂CO₃) / bicarbonate (HCO₃^-) buffer. Which of the following statements describes what happens when a small amount of a strong acid is added to the buffer system:

A) the amount of bicarbonate increases
B) the amount of bicarbonate decreases
C) the amount of carbonic acid increases
D) the amount of carbonic acid decreases
E) Both b & c.

Question 55

Which of the following could be paired with hydrofluoric acid, HF, to create a buffer solution:

A) NaF
B) KF
C) CaF₂
D) All of the above.
E) Both b & c.

Question 56

Which of the following acids is the conjugate acid of the bisulfate ion, HSO₄^- ?

A) HSO₃^-
B) SO₄^2-
C) SO₃^2-
D) H₂SO₄
E) None of the above.

Question 57

Which of the following acids is the conjugate base of the bisulfate ion, HSO₄^- ?

A) HSO₃^-
B) SO₄^2-
C) SO_3s
D) H₂SO₄
E) None of the above.

Question 58

One primitive technology that has been utilized for centuries is the creation of slaked lime, calcium hydroxide, Ca(OH)₂ by reaction of calcium oxide, CaO, with water according to the following chemical reaction:
CaO_(s) + H₂O_(l) Ca(OH)_2(s)
Which of the following statements is true regarding the formation of slaked lime:

A) Water is acting as an acid.
B) The calcium hydroxide is acting as a base
C) The calcium oxide and the calcium hydroxide are a conjugate acid/base pair.
D) This is a buffer system.
E) None of the above.

Question 59

Seltzer water is created by placing water under pressure with carbon dioxide gas. Which of the following statements best describe seltzer water:

A) The solution will be slightly acidic.
B) The solution will be slightly basic.
C) The solution will be strongly acidic.
D) The solution will be strongly basic.
E) The solution will be neutral.

Question 60

You encounter a solution that is basic and you decide to test it by adding a small amount of a strong acid. The pH lowers by approximately 2 pH units, but still remains basic. What can you say about the solution?

A) It is a buffer solution.
B) It is not a buffer solution.
C) It is a strong base solution.
D) The solution has been neutralized.
E) The solution has excess acid present.

Question 61

You encounter a solution that is acidic and you decide to test it by adding a small amount of a strong acid. The pH lowers slightly but is approximately unchanged, and still remains acidic. What can you say about the solution?

A) It is a buffer solution.
B) It is not a buffer solution
C) It is a strong acid solution.
D) The solution has been neutralized.
E) The solution has excess acid present.

Question 62

Which of the following would you expect to turn litmus paper red:

A) saliva
B) blood
C) tears
D) gastric juices
E) none of the above

Question 63

Most bodily fluids, except for a few notable exceptions have components that are:

A) either weak acids or weak bases
B) either strong acids or strong bases
C) buffers
D) All of the above.
E) None of the above.