Chemistry (CP) HW Chapter 19 (Due May 13, Test May 14)
Matching
Match each item with the correct statement below.
a. acid dissociation constant
d. Lewis acid
b. diprotic acid
e. pH
c. hydrogen-ion donor
____
____
____
____
____
1.
2.
3.
4.
5.
can accept an electron pair
acid with two ionizable protons
Brønsted-Lowry acid
negative logarithm of the hydrogen ion concentration
ratio of the concentration of the dissociated to the undissociated form
Match each item with the correct statement below.
a. salt hydrolysis
d. equivalence point
b. end point
e. buffer capacity
c. titration
____
____
____
____
____
6. process of adding a known amount of solution of known concentration to determine the concentration of
another solution
7. The number of moles of hydrogen ions equals the number of moles of hydroxide ions.
8. Indicator changes color.
9. Cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water.
10. the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 11. When an acid reacts with a base, what compounds are formed?
a. a salt only
c. metal oxides only
b. water only
d. a salt and water
____ 12. What is the formula for phosphoric acid?
a. H PO
c. HPO
b. H PO
d. HPO
____ 13. Which of the following is a property of an acid?
a. sour taste
c. strong color
b. nonelectrolyte
d. unreactive
____ 14. What is a property of a base?
a. bitter taste
c. strong color
b. watery feel
d. unreactive
____ 15. The formula of the hydrogen ion is often written as ____.
a. H O
c. H
b. OH
d. H N
____ 16. Which hydroxide compound yields the lowest concentration of hydroxide ions in aqueous solution?
a. sodium hydroxide
c. calcium hydroxide
b. potassium hydroxide
d. magnesium hydroxide
____ 17. What is an acid according to Arrhenius?
a. a substance that ionizes to yield protons in aqueous solution
b. a substance that is a hydrogen ion donor
c. a substance that accepts an electron pair
d. a substance that is a hydrogen ion acceptor
____ 18. Which of these is an Arrhenius base?
a. LiOH
c. H PO
b. NH
d. CH COOH
____ 19. What is transferred between a conjugate acid-base pair?
a. an electron
c. a hydroxide ion
b. a proton
d. a hydronium ion
____ 20. A Lewis acid is a substance that can ____.
a. donate a pair of electrons
c. donate a hydrogen ion
b. accept a pair of electrons
d. accept a hydrogen ion
____ 21. In the reaction of aluminum bromide with ionized sodium bromide, which compound is the Lewis acid?
a. aluminum bromide
c. sodium ion
b. bromide ion
d. None are Lewis acids.
____ 22. What type of acid is sulfuric acid?
a. monoprotic
c. triprotic
b. diprotic
d. none of the above
____ 23. Which compound can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
a. water
c. sodium hydroxide
b. ammonia
d. hydrochloric acid
____ 24. In the reaction CO
+H O
HCO + OH , the carbonate ion is acting as a(n) ____.
a. Arrhenius base
c. Brønsted-Lowry base
b. Arrhenius acid
d. Brønsted-Lowry acid
____ 25. What are the acids in the following equilibrium reaction?
CN + H O
HCN + OH
a. CN , H O
c. CN , OH
b. H O, HCN
d. H O, OH
____ 26. Which of the following represents a Brønsted-Lowry conjugate acid-base pair?
a. SO
c. H O and H
and SO
b. CO
d. NH and NH
and CO
____ 27. If the hydrogen ion concentration of a solution is 10 M, is the solution acidic, alkaline, or neutral?
a. acidic
c. neutral
b. alkaline
d. The answer cannot be determined.
____ 28. In a neutral solution, the [H ] is ____.
a. 10 M
b. zero
c. 1 10 M
d. equal to [OH ]
____ 29. What is the best description for a solution with a hydroxide-ion concentration of 1 10 M?
a. acidic
c. neutral
b. basic
d. The answer cannot be determined.
____ 30. What is pH?
a. the negative logarithm of the hydrogen ion concentration
b. the positive logarithm of the hydrogen ion concentration
c. the negative logarithm of the hydroxide ion concentration
d. the positive logarithm of the hydroxide ion concentration
____ 31. Which type of solution is one with a pH of 8?
a. acidic
b. basic
c. neutral
d. The type varies, depending on the solution.
____ 32. Which of these solutions is the most basic?
a. [H ] = 1 10 M
c. [H ] = 1 10 M
b. [OH ] = 1 10 M
d. [OH ] = 1 10 M
____ 33. An indicator is what type of compound?
a. oxidizing agent
c. strong base or acid
b. weak base or acid
d. salt
____ 34. What characterizes a strong acid or base?
a. polar covalent bonding
b. complete ionization in water
c. ionic bonding
d. presence of a hydroxide or hydrogen ion
____ 35. The acid dissociation constant for an acid dissolved in water is equal to the ____.
a. equilibrium constant
b. equilibrium constant times the concentration of water
c. equilibrium constant divided by the concentration of water
d. equilibrium constant times the equilibrium constant of water
____ 36. With solutions of strong acids and strong bases, the word strong refers to ____.
a. normality
c. solubility
b. molarity
d. degree of ionization
____ 37. What is another name for the acid dissociation constant?
a. equilibrium constant
c. rate constant
b. ionization constant
d. mole fraction
____ 38. How many ionization constants are associated with oxalic acid?
a. 0
c. 2
b. 1
d. 3
____ 39. Acetic acid ionizes in water as follows:
Fewer than 1% of ethanoic acid molecules are ionized at any instant. The acetate ion (CH COO ) is therefore
____.
a. a poor hydrogen-ion acceptor
c. a poor hydrogen-ion donor
b. a good hydrogen-ion acceptor
d. a good hydrogen-ion donor
____ 40. A 0.12M solution of an acid that ionizes only slightly in solution would be termed ____.
a. concentrated and weak
c. dilute and weak
b. strong and dilute
d. concentrated and strong
____ 41. Which of the following pairs consists of a weak acid and a strong base?
a. sulfuric acid, sodium hydroxide
c. acetic acid, sodium hydroxide
b. acetic acid, ammonia
d. nitric acid, calcium hydroxide
____ 42. A substance with a K of 1
a. strong acid
b. weak acid
10
would be classified as a ____.
c. strong base
d. weak base
____ 43. The ionization constant (K ) of HF is 6.7
acid?
a. [HF] is greater than [H ][F ].
b. [HF] is less than [H ][F ].
____ 44. The K of carbonic acid is 4.3
10 . Which of the following is true in a 0.1M solution of this
c. [HF] is equal to [H ][F ].
d. [HF] is equal to [H ][F ].
10 .
H CO
H + HCO
This means that H CO is a ____.
a. good hydrogen-ion acceptor
c. good hydrogen-ion donor
b. poor hydrogen-ion acceptor
d. poor hydrogen-ion donor
____ 45. Which acid has the greatest acid dissociation constant?
a. nitric acid
c. carbonic acid
b. acetic acid
d. boric acid
____ 46. Which base is strong, but never concentrated?
a. magnesium hydroxide
c. ammonia
b. sodium hydroxide
d. water
____ 47. A base has a K of 2.5 10 . Which of the following statements is true?
a. This is a concentrated base.
b. This base ionizes slightly in aqueous solution.
c. This is a strong base.
d. An aqueous solution of this base would be acidic.
____ 48. The process of adding a known amount of solution of known concentration to determine the concentration of
another solution is called ____.
a. neutralization
c. titration
b. hydrolysis
d. buffer capacity
____ 49. In a titration, when the number of moles of hydrogen ions equals the number of moles of hydroxide ions,
what is said to have happened?
a. The equivalence point has been reached.
b. The end point has been reached.
c. The point of neutralization has been reached.
d. The titration has failed.
____ 50. What kind of ion is contained in salts that produce an acidic solution?
a. a positive ion that releases a proton to water
b. a negative ion that releases a proton to water
c. a positive ion that attracts a proton from water
d. a negative ion that attracts a proton from water
Numeric Response
51. If the hydrogen ion concentration is 10 M, what is the pH of the solution?
52. If the hydroxide ion concentration is 10
53. If [OH ] = 1
M, what is the pH of the solution?
10 M, what is the pH of the solution?
54. What is the pH of a solution with a concentration of 0.01M hydrochloric acid?
55. What is the pH when the hydrogen ion concentration is 7.0
10 M?