TB_Acid and Bases Flashcards
Under the Bronsted concept of acids and bases, a base is
A. a proton donor
B. a proton acceptor
C. a hydroxide donor
D. an electron pair donor
B. a proton acceptor
Under the Lewis concept of acids and bases, an acid is
A. a proton donor
B. a proton acceptor
C. An electron pair donor
D. an electron pair acceptor
D. an electron pair acceptor
Under the Bronsted concept of acids and bases, an acid is
A. a proton donor
B. a proton acceptor
C. an electron pair donor
D. an electron pair acceptor
A. a proton donor
Which of the following is NOT an acid-base conjugate pair?
A. HCN and CN−
B. H2O and OH−
C. H2S and OH−
D. NH3 and NH4
+
C. H2S and OH−
Predict the products of the following acid-base reaction:HCl(aq) + NaOH(aq) →
A. H3O+
(aq) + OH−
B. Na+
(aq) + Cl−
(aq)
C. NaCl(aq) + H2O(l)
D. no reaction takes place
C. NaCl(aq) + H2O(l)
Predict the products of the following acid-base reaction: NH3(aq) + HNO3(aq) →
A. NH2OH(aq) + HNO2(aq)
B. NH4NO3(aq)
C. NH4OH(aq)
D. no reaction takes place
B. NH4NO3(aq)
What effect will addition of excess of HCl have on the pH of a solution of NH3?
A. increase the pH
B. decrease the pH
C. no effect
D. cannot tell from information given
B. decrease the pH
What effect will addition of sodium acetate have on the pH of a solution of acetic acid?
A. increase the pH
B. decrease the pH
C. no effect
D. cannot tell from information given
A. increase the pH
A solution that causes only a relatively small change in pH upon addition of small amounts of acids and bases is
A. saturated
B. a salt
C. a buffer
D. unsaturated
C. a buffer
Which of the following is buffer?
A. NaCl/NH4Cl
B. NH3/NH4Cl
C. NH3/CH3COOH
D. CH3COOH/NaOH
B. NH3/NH4Cl
A buffer solution may be a mixture of
A. a weak acid and its salt
B. a weak base and its salt
C. an excess of a weak acid with a strong base
D. all of the above
D. all of the above
The conjugate base of acetic acid is
A. HCOOH
B. NH3
C. CH3COO−
D. OH−
C. CH3COO−
The conjugate acid of ammonia is
A. H3O+
B. NH4+
C. HCOOH
D. OH−
B. NH4+
Effect produced by an ion, say from a salt, which is the same ion produced by the dissociation of a weak acid or
base is called
A. colloidal effect
B. precipitation effect
C. common ion effect
D. ligand effect
C. common ion effect
A principle stating that if stress is applied to a system at equilibrium, the equilibrium is shifted in the
direction that tends to reduce the stress.
A. Heisenberg Uncertainty Principle
B. Le Chatelier’s Principle
C. Hund’s Rule
D. Debye-Huckel Principle
B. Le Chatelier’s Principle
Water cannot function as which one of the following?
A. a Bronsted acid
B. a Bronsted base
C. a Lewis acid
D. a Lewis base
C. a Lewis acid
HCOOK is a/an
A. acid
B. base
C. salt
D. oxide
C. salt
When a strong acid is titrated with a weak base, the pH at the equivalence point is
A. basic
B. acidic
C. neutral
D. none of the above
B. acidic
When a strong acid is titrated with a strong base, the pH at the equivalence point is
A. basic
B. acidic
C. neutral
D. none of the above
C. neutral
When NH4Cl hydrolyzes, the resulting solution is
A. acidic
B. basic
C. neutral
D. none of the above
A. acidic
We have a 5.43 x 10−4 M solution of HNO3 at 25oC. What is the [OH−
] in this solution?
A. 1.84 x 10−11 M
B. 5.43 x 10−10 M
C. 5.43 x 10−4 M
D. 3.67 x 10−6 M
A. 1.84 x 10−11 M
What is the pH of a 5.82 x 10−3 M solution of NaOH at 25oC?
A. 4.76
B. 11.76
C. 7.00
D. 2.45
B. 11.76
The pH of a 0.20 M NH3 solution is Kb (NH3) = 1.8 x 10‒5
A. 0.70
B. 2.73
C. 11.28
D. 6.99
C. 11.28
The pH of a solution is 6.38. The hydrogen ion concentration is
A. 4.17 x 10−7 M
B. 4.17 x 10−6 M
C. 6.38 x 10−6 M
D. 0.638 M
A. 4.17 x 10−7 M
What is the [H3O+
] of a 0.100 M solution of HCN at 25oC? Ka (HCN) = 4.0 x 10−10
A. 1.58 x 10−8 M
B. 2.00 x 10−5 M
C. 6.32 x 10−6 M
D. 4.00 x 10−11 M
C. 6.32 x 10−6 M
A 0.200 M solution of an acid, HA, has a pH of 2.70 at 25oC. What is Ka for this acid?
A. 2.21 x 10−4
B. 4.55 x 10−6
C. 1.99 x 10−4
D. 2.00 x 10−5
D. 2.00 x 10−5
What is the pH of a 0.52 M solution of CH3COONa at 25oC? Ka (CH3COOH) = 1.76 x 10−5
A. 9.23
B. 4.77
C. 9.37
D. 10.21
A. 9.23
Acids and Bases Which statement is true?
a. The value of the equilibrium constant increases with the addition of a catalyst
b. A catalyst speeds up both the forward and reverse reaction rates
c. The greater the activation energy, the faster the rate of reaction.
d. A catalyst increases the rate of reaction by decreasing the number of collisions
b. A catalyst speeds up both the forward and reverse reaction rates
The lining of the stomach contains cells that secrete a solution of HCl. Which drink would best alleviate
heartburn (excess acid in the stomach)?
a. milk, pH = 6.5
b. wine, pH = 3.8
c. diet soda, pH = 4.3
d. milk of magnesia, pH = 10.5
d. milk of magnesia, pH = 10.5
Which species are acting as Bronsted acids in the reaction below?
HSO4
−
(aq) + H2O(l) ⇄ H3O+
(aq) + SO4
−2(aq)
a. H2O
b. H2O and H3O+
c. H2O and SO4−2
d. HSO4− and H3O+
d. HSO4− and H3O+
Which equation correctly describes the relationship between Kb and Ka for a conjugate acid/base pair?
a. Kb = Kw Ka
b. Kb = Ka / Kw
c. Kb = Kw / Ka
d. Kb = Ka + Kw
c. Kb = Kw / Ka