testbank to accompany gob chemistry, 3e … 10... · web viewthe exam will come from those...
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General, Organic, and Biological Chemistry, 3e (Timberlake) This set includes all problems but you can focus only on the following numbers; 6,8,13,14,21,23,24,25,31,35,36,37,39,41,44,47-48,52,53,54,56,59,61,62 and 65. The exam will come from those problems.Chapter 10
1
Acids and Bases10.1
2
Multiple-Choice Questions1)
3
According to the Arrhenius concept, if NaOH were dissolved in water, it would act as A)
4
a base. B)
5
an acid. C)
6
a source of hydronium ions. D)
7
a source of H- ions. E)
8
a proton donor.
9
2)
10
According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as A)
11
a base. B)
12
an acid. C)
13
a source of hydroxide ions. D)
14
a source of H- ions. E)
15
a proton acceptor.
16
3)
17
The name given to an aqueous solution of HBr is A)
18
hydrogen bromide. B)
19
hydrobromic acid. C)
20
bromic acid. D)
21
bromous acid. E)
22
hypobromous acid.
23
4)
24
The name given to an aqueous solution of HNO3 is A)
25
nitric acid. B)
26
nitrous acid. C)
27
hydrogen nitrate. D)
28
hydronitrogen acid. E)
29
hyponitric acid.
30
5)
31
The name given to an aqueous solution of HClO3 is A)
32
chlorous acid. B)
33
hypochlorous acid. C)
34
chloric acid. D)
35
hydrochloric acid. E)
36
hypochloric acid.
37
38
6)
39
Which one of the following is characteristic of a base? A)
40
produces H3O+ in water B)
41
has a sour taste C)
42
has a slippery, soapy feel D)
43
turns blue litmus red E)
44
is insoluble in water
45
7)
46
According to the Bronsted-Lowry definition, A)
47
an acid is a proton acceptor. B)
48
a base produces H+ ions in aqueous solutions. C)
49
a base is a proton donor. D)
50
a base is a proton acceptor. E)
51
an acid acts as the solvent.
52
8)
53
Identify the Bronsted-Lowry acid in the following reaction.H2O + CO32- → HCO3- + OH-
A)
54
H2O B)
55
CO32- C)
56
HCO3- D)
57
OH- E)
58
H2CO3
59
9)
60
The correct formula for sulfuric acid is A)
61
H2SO4. B)
62
H2SO3. C)
63
H2SO4-. D)
64
H2SO3-. E)
65
SO42-.
66
10)
67
The name of Al(OH)3 is A)
68
aluminum trihydroxide. B)
69
monoaluminum trihydroxide. C)
70
aluminum hydroxide. D)
71
aluminum(III) hydroxide. E)
72
aluminum oxygen hydride.
73
74
11)
75
Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?
A)
76
In acids, [OH-] is greater than [H3O+]. B)
77
In bases, [OH-] = [H3O+]. C)
78
In neutral solutions, [H3O+] = [H2O]. D)
79
In bases, [OH-] is greater than [H3O+]. E)
80
In bases, [OH-] is less than [H3O+].
81
12)
82
The conjugate base of HClO3 is A)
83
HClO2. B)
84
ClO3-. C)
85
Cl(OH)2. D)
86
ClO3. E)
87
HClO.
88
13)
89
The conjugate acid of HSO4- is A)
90
SO42-. B)
91
HSO4. C)
92
H2SO4. D)
93
H2SO4-. E)
94
HSO3-.
95
14)
96
For Kw, the product of [H3O+] and [OH-] is A)
97
1.0 x 10-14. B)
98
1.0 x 10-7. C)
99
1.0 x 10-1. D)
100
1.0. E)
101
1.0 x 1014.
102
15)
103
What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M? A)
104
1 x 10-12 M B)
105
1 x 102 M C)
106
1 x 10-7 M D)
107
1 x 10-8 M E)
108
1 x 10-2 M
109
110
16)
111
What is the [OH-] in a solution that has a [H3O+] = 1 x 10-6 M? A)
112
1 x 10-2 M B)
113
1 x 10-6 M C)
114
1 x 10-8 M D)
115
1 x 10-10 M E)
116
1 x 10-12 M
117
17)
118
What is the [OH-] in a solution that has a [H3O+] = 2.0 x 10-4 M? A)
119
2.0 x 10-10 M B)
120
5.0 x 10-10 M C)
121
1.0 x 10-10 M D)
122
2.0 x 10-4 M E)
123
5.0 x 10-11 M
124
18)
125
A solution with a pH of 4 is A)
126
extremely acidic. B)
127
moderately acidic. C)
128
neutral. D)
129
slightly basic. E)
130
extremely basic.
131
19)
132
What is the pH of a solution with [H3O+] = 1 x 10-9 M? A)
133
1.0 x 10-5 M B)
134
-9.0 C)
135
5.0 D)
136
-5.0 E)
137
9.0
138
20)
139
What is the pH of a solution with [H3O+] = 3.0 x 10-3 M? A)
140
3.0 x 10-3 B)
141
2.52 C)
142
3.0 D)
143
-2.52 E)
144
9.0
145
21)
146
What is the pH of a solution with [OH-] = 1 x 10-4 M? A)
147
10.0 B)
148
-10.0 C)
149
4.0 D)
150
-4.0 E)
151
1.0 x 10-10
152
22)
153
What is the pH of a solution with [OH-] = 2.0 x 10-10 M? A)
154
9.70 B)
155
-9.70 C)
156
4.30 D)
157
-4.30 E)
158
2.0 x 10-10
159
23)
160
The [H3O+] of a solution with pH = 2 is A)
161
10 M. B)
162
-10 M. C)
163
1 x 102 M. D)
164
1 x 10-2 M. E)
165
1 x 10-12 M.
166
24)
167
In which of the following are the pH values arranged from the most basic to the most acidic?
A)
168
1, 3, 6, 8, 11, 14 B)
169
2, 5, 7, 9, 10, 11 C)
170
14, 10, 7, 4, 3, 1 D)
171
14, 10, 7, 1, 3, 5 E)
172
7, 10, 14, 4, 3, 1
173
25)
174
In which of the following are the pH values arranged from the most acidic to the most basic?
A)
175
1, 3, 6, 8, 11, 14 B)
176
2, 5, 7, 9, 10, 1.1 C)
177
14, 10, 7, 4, 3, 1 D)
178
14, 10, 7, 1, 3, 5 E)
179
7, 10, 14, 4, 3, 1
180
26)
181
Which of the following is the strongest acid? A)
182
H3PO4 B)
183
NH4+ C)
184
NaOH D)
185
H2CO3 E)
186
HCl
187
188
27)
189
Which of the following is the strongest acid? A)
190
HF (Ka for HF is 7.2 x 10-4) B)
191
HCN (Ka for HCN is 4.9 x 10-10) C)
192
HCNO (Ka for HCNO is 2 x 10-4) D)
193
H3BO3 (Ka for H3BO3 is 5.4 x 10-10)
194
28)
195
Which of the following is the weakest acid? A)
196
HF (Ka for HF is 7.2 x 10-4) B)
197
HCN (Ka for HCN is 4.9 x 10-10) C)
198
HCNO (Ka for HCNO is 2 x 10-4) D)
199
H3BO3 ( Ka for H3BO3 is 5.4 x 10-10)
200
29)
201
The stronger the acid, the __________ the conjugate base. A)
202
stronger B)
203
weaker
204
30)
205
Which of the following is the strongest base? A)
206
H3PO4B)
207
NH3 C)
208
NaOH D)
209
NaCl E)
210
HCl
211
31)
212
Which of the following is correctly identified? A)
213
NH3, strong acid B)
214
NaOH, strong base C)
215
HCl, weak acid D)
216
H2CO3, strong acid E)
217
Ca(OH)2, weak base
218
32)
219
Ammonium hydroxide is a weak base because A)
220
it is a dilute solution. B)
221
it is only slightly soluble in water. C)
222
it cannot hold on to its hydroxide ions. D)
223
it dissociates only slightly in water. E)
224
it is completely ionized in aqueous solution.
225
226
33)
227
Predict whether the equilibrium of the following reaction favors reactants or products:NH4+ + H2O ⇌ NH3 + H3O+
A)
228
Reactants are favored. B)
229
Products are favored. C)
230
Neither side is favored.
231
34)
232
An acid and base react to form a salt and water in a(n) __________ reaction. A)
233
ionization B)
234
dissociation C)
235
oxidation D)
236
neutralization E)
237
reduction
238
35)
239
In a neutralization reaction A)
240
two acids react to form water. B)
241
water and a salt react to form an acid and a base. C)
242
an acid and a salt react to form water and a base. D)
243
a base and a salt react to form water and an acid. E)
244
an acid and a base react to form a salt and water.
245
36)
246
Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 with Ca(OH)2?
A)
247
H3PO4 + Ca(OH)2 → CaHPO4 + 2 H2O B)
248
3 H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5 H2O C)
249
H3PO4 + Ca(OH)2 → Ca3(PO4)2 + H2O D)
250
2 H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6 H2O E)
251
4 H3PO4 + 6Ca(OH)2 → 2 Ca3(PO4)2 + 12 H2O
252
37)
253
The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula A)
254
H2O. B)
255
. C)
256
. D)
257
. E)
258
NO3OH.
259
38)
260
How many moles of H2O are produced when 1 mole of Mg(OH)2 reacts with 1 mole of H2 H2SO4?
A)
261
1 B)
262
2 C)
263
3 D)
264
4 E)
265
5
266
39)
267
In a neutralization reaction, how many moles of HClO4 react with 1 mole of Al(OH)3? A)
268
1 B)
269
2 C)
270
3 D)
271
4 E)
272
5
273
40)
274
Which of the following is a neutralization reaction? A)
275
KCl + NaNO3 → KNO3 + NaCl B)
276
HNO3 + KOH → H2O + KNO3 C)
277
H2O + SO3 → H2SO4 D)
278
4Na + O2 → 2 Na2O E)
279
2 NO2 → 2NO + O2
280
41)
281
The function of a buffer is to A)
282
change color at the end point of a titration. B)
283
maintain the pH of a solution. C)
284
be a strong base. D)
285
maintain a neutral pH. E)
286
act as a strong acid.
287
42)
288
The normal blood pH is about A)
289
6.8. B)
290
7.0. C)
291
7.2. D)
292
7.4. E)
293
7.6.
294
43)
295
In a buffer system of HF and its salt, NaF, A)
296
the HF neutralizes added acid. B)
297
the HF neutralizes added base. C)
298
the HF is not necessary. D)
299
the F- neutralizes added H2O. E)
300
the F- neutralizes added base.
301
44)
302
Which of the following is a buffer system? A)
303
NaCl and NaNO3 B)
304
HCl and NaOH C)
305
H2CO3 and KHCO3 D)
306
NaCl and NaOH E)
307
H2O and HCl
308
309
45)
310
Which of the following could be a buffer? A)
311
NaF B)
312
HF + NaF C)
313
HF + H2O D)
314
NaF + H2O E)
315
NaCl + HF
316
46)
317
What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30? A)
318
respiratory acidosis B)
319
respiratory alkalosis C)
320
metabolic acidosis D)
321
metabolic alkalosis E)
322
diabetes mellitus
323
47)
324
If a condition of hypoventilation occurs, the blood pH of the patient is expected to A)
325
saturate. B)
326
increase. C)
327
decrease. D)
328
stay the same. E)
329
concentrate.
330
48)
331
When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO2, the blood pH rises in a condition called
A)
332
metabolic acidosis. B)
333
metabolic alkalosis. C)
334
respiratory acidosis. D)
335
respiratory alkalosis. E)
336
pulmonary distress.
337
49)
338
25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the NaOH solution is
A)
339
0.212 M B)
340
0.115 M C)
341
0.500 M D)
342
0.390 M E)
343
0.137 M
344
50)
345
What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution?
A)
346
0.267 M B)
347
0.143 M C)
348
0.200 M D)
349
0.280 M E)
350
0.100 M
351
352
51)
353
A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid?
H3PO4 + 3NaOH → Na3PO4 + 3 H2O
A)
354
0.333 M B)
355
3.00 M C)
356
1.50 M D)
357
1.00 M E)
358
0.750 M
359
52)
360
A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid?
H2SO4 + 2KOH → K2SO4 + 2 H2O
A)
361
2.00 M B)
362
2.50 M C)
363
0.800 M D)
364
1.60 M E)
365
1.25 M
366
53)
367
A 10.0 mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is
A)
368
0.207 M B)
369
0.4141 M C)
370
0.0708 M D)
371
0.428 M E)
372
0.142 M
373
54)
374
How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl?
A)
375
50.0 mL B)
376
40.0 mL C)
377
0.100 mL D)
378
20.0 mL E)
379
10.0 mL
380
55)
381
How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO4?
A)
382
7.50 mL B)
383
2.50 mL C)
384
0.833 mL D)
385
5.00 mL E)
386
15.0 mL
387
56)
388
How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl?
A)
389
100. mL B)
390
50.0 mL C)
391
25.0 mL D)
392
0.250 mL E)
393
0.50 mL
394
57)
395
The Ka for hydrofluoric acid is 7.2 x 10-4. This means that HF is A)
396
neutral in water solution. B)
397
able to react with HCl. C)
398
a weak acid. D)
399
a strong acid. E)
400
ionic.
401
58)
402
In a sulfuric acid solution, where the [H2SO4] is 0.005 M, what is the pH? A)
403
pH = 12.0 B)
404
pH = 2.0 C)
405
pH = 3.0 D)
406
pH = 11.0 E)
407
pH = 5.0
408
59)
409
When a piece of magnesium metal is added to hydrochloric acid, what gas is produced? A)
410
oxygen B)
411
chlorine C)
412
nitrogen D)
413
carbon dioxide E)
414
hydrogen
415
60)
416
The salt made from a weak acid and a strong base should give a solution of A)
417
high concentration. B)
418
low concentration. C)
419
pH > 7. D)
420
pH < 7 E)
421
pH = 7.
422
61)
423
Which solution has the highest pH? A)
424
a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B)
425
a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C)
426
a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D)
427
a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E)
428
All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.
429
430
62)
431
Which solution has the lowest pH? A)
432
a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B)
433
a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C)
434
a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D)
435
a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E)
436
All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.
437
63)
438
Acid rain has a A)
439
pH < 7. B)
440
pH > 7. C)
441
pH < 6.2. D)
442
pH < 2.6.
443
64)
444
A major cause of acid rain is A)
445
CO2 production. B)
446
CaCO3 production. C)
447
SO2 production. D)
448
NH3 production.
449
For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution .
Mg(s) + 2HCl(aq) → MgCl2 (aq) + H2 (g)
65)
450
If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?
A)
451
1.65 M B)
452
80.0 M C)
453
8.00 M D)
454
0.823 M E)
455
3.29 M
456
10.2
457
Short Answer Questions1)
458
The conjugate acid of HPO42- is __________.
459
2)
460
Write the proper Ka expression for the ionization of acetic acid, HC2H3O2.
461
3)
462
If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?
463
4)
464
Is a solution of sodium phosphate in water acidic or basic?
465
466
5)
467
What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?
468
6)
469
In a titration experiment, a student used 24.13 mL of 0.111 M sodium hydroxide to neutralize 20.00 mL of a hydrochloric acid solution. What was the molarity of the acid solution?
470
7)
471
A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?
472
8)
473
Identify the conjugate acid-base pairs in the following reaction:HCl + NH3 → NH4+ + Cl-
474
9)
475
A student had 25.0 mL of 0.100 M H2SO4 solution. How many mL of a 0.100 M NaOH solution will the sulfuric acid neutralize?
476
10.3
477
True/False Questions1)
478
If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.
479
2)
480
Alkalosis is the blood condition in which the blood pH is higher than normal.
481
3)
482
A buffer is a solution that tends to maintain a neutral pH.
483
4)
484
In any water solution, [H3O+] [OH-]= 1.0 x 10-7.
485
5)
486
An ammonium chloride solution should have an acidic pH.
487
6)
488
Magnesium metal is not attacked by sulfuric acid solutions.
489
7)
490
Sodium carbonate gives a basic solution in water.
491
8)
492
For most reactions of acids with bases, the resulting products are a salt and water.
493
494
10.4
495
Matching QuestionsIdentify each of the following compounds as an acid, a base, or neither.
1)
496
HCl
497
A)
498
base
2)
499
NaOH
500
B)
501
neither
3)
502
NH3
503
C)
504
acid
4)
505
H2SO4
5)
506
CO32-
6)
507
NaCl
7)
508
CN-
8)
509
H2CO3
510
511
512
513
514
515
516
517
518
519
520
521
522
523
In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]?
9)
524
acid
525
A)
526
greater than
10)
527
base
528
B)
529
equal to
11)
530
[H3O+]= 1.0 x 10-6 M
531
C)
532
less than
12)
533
[H3O+] = 1.0 x 10-10 M
13)
534
[H3O+] = 1.0 x 10-7 M
14)
535
pH = 2
15)
536
pH = 9
537
538
539
540
541
542
543
544
545
546
547
548
549
Identify the following as acids, bases, or neutral solutions.
16)
550
has a sour taste
551
A)
552
neutral
17)
553
has a pH = 4.5
554
B)
555
acid
18)
556
turns blue litmus paper red
557
C)
558
base
19)
559
contains more hydronium ions than hydroxide ions
20)
560
H2O
21)
561
[H3O+] = 3.4 x 10-5 M
22)
562
[OH-]= 2.8 x 10-2 M
23)
563
Ca(OH)2
24)
564
pH =9.0
25)
565
[H3O+] = 1.0 x 10-7 M
566
567
568
569
570
571
572
573
574
575
576
577
578
579
580
581
582
583
584