Chemistry Review (Acids and Bases)
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Electrolytes
Definitions of Acids and Bases
Neutralization and Titration, Hydrolysis, Indicators
Conjugate Acid-Base Pairs
pH and pOH of Solutions
Electrolytes
__ 1) Which substance is an electrolyte?
a) C2H5OH
b) C6H12O6
c) C12H22O11
d) CH3COOH
__ 2)
Which of the following is the best conductor of electricity?
a) NaCl (s)
b) NaCl (aq)
c) C6H12O6 (s)
d) C6H12O6 (aq)
__ 3)
Which of the following 0.1 M solutions is the best conductor of electricity?
a) HC2H3O2 (aq)
b) HCl (aq)
c) C6H12O6 (aq)
d) C12H22O11 (aq)
__ 4)
Which is characteristic of an aqueous solution of HNO3?
a) it conducts electricity
b) it forms OH- ions
c) it turns litmus blue
d) it turns phenolphthalein pink
__ 5)
Based on Reference Table F, which saturated solution would be the most basic?
a) KOH (aq)
b) Fe(OH)2 (aq)
c) Mn(OH)2 (aq)
d) Al(OH)3 (aq)
Definitions of Acids and Bases
__ 6) All water-soluble acids
a) release hydrogen ions in water
b) produce salts that are very soluble in water
c) are equally strong
d) produce pH values above 7
__ 7)
A hydroxide ion is a water molecule
a) minus the oxygen
b) plus a neutron
c) minus a proton
d) minus an electron
__ 8)
Given the following reaction
HCl + HSO4Cl- + H2SO4
Which of the particles involved can be classified as bases?
a) Cl- and HSO4b) HCl and Clc) HCl and H2SO4
d) Cl- and H2SO4
__ 9)
In the reaction NH3 + H2O
a) conductor of electricity
b) weak base
c) proton acceptor
d) proton donor
NH4+ + OH-, the water molecule serves as a
__ 10) The OH- concentration is greater than the H+ concentration in an aqueous solution of
a) CH3OH
b) Ba(OH)2
c) HCl
d) H2SO4
Neutralization and Titration, Hydrolysis, Indicators
__ 11) When Na2CO3 is added to water, the pH of the solution
a) increases
b) decreases
c) stays the same
__ 12) A solution of NH3 (aq) would have a pH closest to
a) 1
b) 3
c) 5
d) 8
__ 13) What is the pH of the solution formed by completely neutralizing 50 millliters of 0.1 M HNO3 with 50
milliliters of 0.1 M NaOH at 298 K?
a) 1
b) 4
c) 7
d) 10
__ 14) An aqueous solution of NaC2H3O2 is basic. This is due to what reaction?
a) C2H3O2- + H2O
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HC2H3O2 + OH+
b) C2H3O2 + H3O
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HC2H3O2 + H2O
c) H2O
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H+ + OHd) HC2H3O2 + H2O
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C2H3O2- + OH__ 15) Why is ammonia NH3 basic?
a) It reacts with water to form H3O+ ions.
b) It reacts with water to form OH- ions.
c) It releases OH- ions.
d) It is a nonelectrolyte.
Conjugate acid-base pairs
__ 16) What is the conjugate acid of CO32-?
a) CO2
b) HCO3c) H2CO3
d) CO32+
__ 17) What are the two conjugate acid-base pairs in the following reaction?
(two answers, please)
HSO4- + CO32SO42- + HCO3a) HSO4- and HCO3b) HSO4- and CO32c) CO32- and HCO3d) HSO4- and SO42__ 18) The conjugate base of NH4+ is
a) OHb) NH2c) NH3
d) NH4OH
__ 19) In the reaction: H2SO4 + H2O
a) HSO4- and H3O+
b) H2O and H3O+
c) H2SO4 and H3O+
d) H2SO4 and H2O
HSO4- + H3O+, the two Brønsted acids are
__ 20) A Brønsted conjugate acid-base pair is related by the transfer of a(n)
a) electron
b) electron pair
c) proton
d) water molecule
pH and pOH of Solutions
__ 21) If [OH-] = 1.0 x 10-4 M for a given solution, then [H+] is equal to
a) 1.0 x 10-14 M
b) 1.0 x 10-10 M
c) 1.0 x 10-6 M
d) 1.0 x 10-4 M
__ 22) Compare solution A (pH = 4) with solution B (pH = 9). Solution A is
a) 5 times more acidic than solution B
b) 100,000 more acidic than solution B
c) 5 times more basic than solution B
d) 100,000 more basic than solution B
__ 23) What is the pH of a 0.10 M solution of NaOH?
a) 1
b) 2
c) 13
d) 14
__ 24) Adding 0.1 M NaOH to a 0.1 M solution of HCl will cause the pH of the solution to
a) increase
b) decrease
c) stay the same
__ 25) As a solution of NaOH is diluted from 0.1 M to 0.001 M the pH of the solution
a) decreases
b) increases
c) stay the same
Answers:
1)
D
2)
B
3)
B
4)
A
5)
A
6)
A
7)
C
8)
A
9)
D
10)
B
11)
A
12)
D
13)
C
14)
A
15)
B
16)
B
17)
C, D
18)
C
19)
C
20)
C
21)
B
22)
B
23)
C
24)
A
25)
A