Name
Class
_
Date
Acids and Bases
_
Chapter
Test
16
DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that best
completes the statement.
1
1. Acids taste (a) sweet; (b) sour; (c) bitter; (d) salty;
2. The basis for the traditional definition of acids was provided by the observations of
(a) Bn/msted; (b) Lewis; (c) Arrhenius; (d) Faraday.
3. A substance that ionizes nearly completely in aqueous solutions, producing
2
H30 +, is a
3
(a) weak base; (b) strong base; (c) weak acid; (d) strong acid.
4. Compared to acids that have the suffix -ic, acids that have the suffix -GUS contain
(a) more hydrogen; (b) more oxygen; (c) less oxygen; (d) the same amount of oxygen.
4
5. Which of the following is the electron-dot structure for hypochlorous acid?
(a)
5
(b) H :~:¢):g:
H:O:CI:
:0:
(d) H:O:CI:O:
(c)
H:9.':Q:
:0:
..
:0:
6. The electron-dot structure
H :~:~::~: H
:0:
is that of (a) sulfurous acid;
6
(b) hydrosulfuric acid; (c) sulfuric acid; (d) hyposulfurous acid.
7. The acid manufactured in largest quantity is (a) hydrochloric acid; (b) phosphoric acid;
(c) nitric acid; (d) sulfuric acid.
7
8. Bases react with (a) acids to produce salts and water; (b) salts to produce acids and water;
(c) water to produce acids and salts; (d) neither acids, salts, nor water.
8
9. Traditional bases (a) produce H30 + ions; (b) produce hydroxide ions; (c) are electron-pair
donors; (d) are proton acceptors.
9
10. A solution that contains OH - from a soluble base is (a) nonelectrolytic; (b) acidic; (c) alkaline;
(d) nonconducting.
___
11. Which of the following is the net ionic equation for a neutralization reaction?
(a) HCl(aq) + NaOH(aq) ---.,> NaCl(aq) + H20(t) (b) H+(aq) + Cl-(aq) + Na+(aq)---">
Na+(aq) + Cl-(aq) + H20(t) (c) H30+(aq) + OH-(aq) ---.,> 2H20(t)
(d) NaOH(s) ---.,> Na+(aq) + OH-(aq)
10
11
12. The reaction HCl(aq) + NH3(aq) ---.,> NH: (aq) + Cl- (aq) is a (a) traditional acid-base reaction;
(b) Br~nsted acid-base reaction; (c) single-replacement reaction; (d) precipitation reaction.
___
12
13. Which of the following is a strong base? (a) NH3 (b) aniline (c) NaOH (d) acetate ion
___
13
14. In a conjugate acid-base pair, the acid typically has (a) one more proton than the base;
(b) one fewer proton than the base; (c) two fewer protons than the base; (d) the same number
of protons as the base.
___
14
15. In the reaction HF + H20 ~ H30+ + F-, a conjugate acid-base pair is (a) F- and H20;
(b) HF and F-; (c) H30+ ·and HF; (d) HF and H20.
___
15
16. If H20 in the equation H20 + HC2H302 ~ H30 + + C2H302 - is a weak base, then H30 + is a
(a) strong acid; (b) strong base; (c) weak acid; (d) weak base.
___
16
17. Proton-transfer reactions favor production of the (a) stronger acid and stronger base;
(b) weaker acid and weaker base; (c) stronger acid and weaker base; (d) weaker acid and
stronger base.
___
17
Chapter 16
Acids and Bases
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77
18. The products of a reaction between a strong acid and a strong base are a (a) stronger acid and
a stronger base; (b) stronger acid and a weaker base; (c) weaker acid and a stronger base;
(d) weaker acid and a weaker base.
___
18
19. In the reaction H3P04 + H20 ~ H30+
(c) spectator species; (d) salt.
+ H2PO;,
H2PO;
acts as a(n) (a) acid; (b) base;
___
19
20. When water is added to a basic anhydride, (a) an acidic solution results; (b) a basic solution
results; (c) a neutral solution results; (d) a hydrate is formed.
___
20
21. When water is added to an acid anhydride, (a) an acidic solution results; (b) a basic solution
results; (c) a neutral solution results; (d) a hydrate is formed.
___
21
___
22
23. Where, in the Periodic Table, are elements that form basic anhydrides located? (a) in the left
and center (b) far to the right (c) in the center only (d) toward the right, but not far to the right
___
23
24. Chromium forms OH compounds that are (a) all acidic; (b) all basic; (c) all amphoteric;
(d) acidic, basic, and amphoteric.
___
24
25. Reactions of dilute nonoxidizing acids with metals produce (a) hydrogen gas and salts;
(b) water and salts; (c) hydrogen gas and water; (d) hydrogen gas, water, and salts.
___
25
26. Reactions between carbon dioxide and hydroxide bases are essentially (a) neutralization
reactions; (b) decomposition reactions; (c) single-replacement reactions; (d) Lewis reactions.
___
26
27. With what type of oxide do hydroxide bases generally react to produce salts and water?
(a) nonmetal oxides (b) metal oxides (c) basic oxides (d) salt oxides
___
27
28. The acid anhydride of carbonic acid is (a) CH4; (b) CO2; (c) CO; (d) H2CO.
___
28
___
29
22. The balanced equation for the reaction of P40lO with water is
(b) 4PH3 + 802; (c) 4HP03; (d) 4P03 + 2H2.
P40lO
+
6H20
29. What are the products of the reaction between aqueous magnesium oxide and
(a) MgP03 and P02 (b) Mg3(P04h (c) Mg3P2 and P03 (d) Mg and P03
~ (a) 4H3P04;
P4010?
30. Oxidizing acids produce salts when they react with (a) metals above or below hydrogen in the
activity series; (b) only metals above hydrogen in the activity series; (c) only metals below
hydrogen in the activity series; (d) no metals.
30
Write on the line at the right of each statement the word or expression that best completes the
31
meaning when substituted for the corresponding number.
DIRECTIONS:
31. In the presence of active ~
, acids generally release hydrogen gas.
32. An acid that contains hydrogen and only one other element is called a(n) ~
33. Bases cause red litmus to turn ~
.
34. A(n) ~
32
37
40
38
36
35
34
33
39
acid.
is defined as an electron-pair acceptor.
35. The species that remains after an acid has given up a proton is called a(n) ~
36. The conjugate acid of F- is ~
in the reaction HF
+ H20
+:t
H30+
base.
+ F-.
37. A(n) -.!TIL is the conjugate of a strong acid.
38. The reaction of N20S with water produces ~
.
39. Barium hydrogen carbonate (Ba(HC03h) is the product of a reaction between ~
Ba(OHh.
and
40. The products of the reaction between magnesium metal and hydrochloric acid are ~
78
.
Chapter 16
Acids and Bases
HRW material
copyrighted
under notice
appearing
earlier in this work.
"------
Name
_
Class
Date
Acid-Base Titration
and pH
_
Test
Chapter
17
DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that best
completes the statement.
1. To which of the following is 1 equiv KOH chemically equivalent in a complete neutralization
reaction? (a) l/2 mol Mg(OHh (b) 1 mol Mg(OHh (c) l/2 equiv Mg(OHh (d) 2 equiv Mg(OHh
1
2. In proton-transfer reactions, the mass of one equivalent of a base is the quantity, in grams,
that (a) accepts one mole of protons; (b) accepts two moles of protons; (c) supplies one mole of
protons; (d) supplies two moles of protons.
2
3. Normality is the number of (a) equivalents of solute per liter solution; (b) equivalents of solute
per kilogram solvent; (c) moles of solute per liter solution; (d) moles of solute per kilogram
solvent.
3
4. Pure water partially breaks down into charged particles in a process called (a) hydration;
(b) hydrolysis; (c) self-ionization; (d) dissociation.
4
5. The symbols used to represent concentration are (a) parentheses; (b) brackets;
(c) degree symbols; (d) delta signs.
5
6. If [H30 +] of a solution is less than [OH-], the solution (a) is always acidic; (b) is always basic;
(c) is always neutral; (d) may be either acidic, basic, or neutral.
6
7. The common logarithm of a number is the (a) inverse of the number; (b) square root of the
number; (c) power to which the number must be raised to equal 10; (d) power to which 10
must be raised to equal the number.
7
8. The pH of any basic solution is (a) less than zero; (b) less than seven, but greater than zero;
(c) greater than seven; (d) exactly zero.
8
9. The pH scale in general use ranges from (a) 0 to 1; (b) -1 to 1; (c) 0 to 7; (d) 0 to 14.
9
10. The range over which an indicator changes color is called its (a) equivalence point;
(b) end point; (c) transition interval; (d) pH interval.
___
10
11. Which of the following indicators is useful in studying neutralizations involving strong acids
and strong bases? (a) phenolphthalein (b) methyl orange (c) bromthymol blue (d) none of
the above
___
11
12. Which of the following is the pH range for an indicator that is useful in studying
neutralizations involving strong acids and weak bases? (a) 1.2-3.0 (b) 3.1-4.6 (c) 6.0-7.6
(d) 9.5-11.0
___
12
___
13
14. In highly acidic solutions, indicators tend to be mostly in the form (a) Hln; (b) In -;
(c) Hln and In - in roughly equal amounts; (d) In +.
___
14
15. Which of the following indicators is the weakest acid? (a) phenolphthalein
(c) litmus (d) bromthymol blue
__
15
___
16
___
17
___
18
13. Which of the following represents indicator ionization equilibrium? (a) Hln ~ H+
(b)InOH~In+
+ OH- (c)In2~In+
+In- (d)In+ H20~H+
+ InOH-
+ In -
(b) methyl orange
16. In acid-base titration, (a) base is always added to acid; (b) acid is always added to base;
(c) base is added to acid or acid is added to base; (d) base is not added to acid, nor is acid
added to base.
17. An acid-base titration determines the solution volumes that are (a) chemically equivalent;
(b) of equal molarity; (c) of equal mass; (d) of equal molality.
18. The formula that relates acid-base volumes and normalities is (a) VtNb - VaNa = 10-14;
(b) VaNb
=
VbNa; (c) VaNa
=
VbNb; (d) Va -
=
Na - Nb.
Chapter 17
Acid-Base Titration and pH
HRW material copyrighted under notice appearing earlier in this
Vb
'NOrle:.
81
DIRECTIONS: Write on the line at the right of each statement the word or expression that best completes the
meaning when substituted for the corresponding number.
19. ~
are solute quantities that have the same combining capacity.
20. The concentration of H30
+
19
M.
ion in pure water is ~
20
21. The negative of the logarithm of hydronium-ion concentration is called ~
22. A(n) ~
is a dye whose colors are sensitive to H30
+
.
21
concentration.
22
23. ~
is the controlled measurement of the amount of solution of known concentration
needed to react with a measured amount of solution of unknown concentration.
23
DIRECTIONS: Write the answer to questions 24-38 on the line to the right, and show your work in the space
provided. (atomic masses are: H 1.007 94, 0 15.9994, P 30.973 76, S 32.06, K 39.0983, Ca 40.08)
24. What is the mass of 2.00 equiv Ca(OHh in a complete neutralization reaction?
____
24
25. How many moles are in 0.239 equiv of H3P04 in a complete neutralization reaction?
____
25
26. What mass of KOH is required to react with 0.881 equiv H2S04 in the reaction
2KOH + H2S04 -> K2S04 + 2H20?
____
26
27. How many grams of H2S04 are contained in 1.45 L of a 0.600 N solution that is to be used in
a complete neutralization reaction?
____
27
28. What is the pH of a 10-4 M HCl solution?
____
28
29. What is the pH of a solution whose hydronium-ion concentration is 5.03 x 10 -1 M?
____
29
30. What is the hydroxide-ion concentration of a solution whose pH is 12.40?
____
30
31. What is the molarity of an H2S04 solution if 49.0 mL of the solution is titrated completely by
68.4 mL of an NaOH solution whose concentration is 0.333 M?
____
31
32. If 114 mL of 0.008 04 M NaOH titrates completely 118 mL of H3P04 solution, what is the
molarity of the H3P04 solution?
____
32
33. What is the molarity of a Ba(OHh solution if 93.9 mL of it is titrated completely by 15.3 mL
of 0.247 M H2S04?
____
33
____
34
35. What is the mass of 1.00 equiv of H3P04 in a complete neutralization reaction?
____
35
36. What is the normality of a 1.037 M H3P04 solution?
____
36
34. What is the normality of a Ba(OHh solution, 1435 mL of which is titrated by 139.0 mL of
1.100 N H2S04?
___
37. What is the pH of a 0.002 45 M HCl solution?
38. What is the concentration of H30
82
+
____
in a solution whose pH is 8.400?
37
38
Acid-Base Titration and pH
Chapter 17
HRW material
copyrighted
under notice
appearing
earlier in this work.