8... · Web viewsemiconductor. D) nonconductor. E) strong electrolyte. 14) In water, a substance...
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This set includes all problems but you can focus only on the following numbers; 10-14, 22-24, 26-36, 50-57 and 64-65. The exam will come from those problems. General, Organic, and Biological Chemistry, 3e (Timberlake) Chapter 8 1
Transcript of 8... · Web viewsemiconductor. D) nonconductor. E) strong electrolyte. 14) In water, a substance...
This set includes all problems but you can focus only on the following numbers; 10-14, 22-24, 26-36, 50-57 and 64-65. The exam will come from those problems.
General, Organic, and Biological Chemistry, 3e (Timberlake) Chapter 8
1
Solutions8.1
2
Multiple-Choice Questions1)
3
The O-H bond in water is polar because A)
4
it is an ionic bond. B)
5
oxygen is much more electronegative than hydrogen. C)
6
oxygen occupies more space than hydrogen. D)
7
hydrogen is much more electronegative than oxygen. E)
8
it is a hydrogen bond.
9
2)
10
A hydrogen bond is A)
11
an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom. B)
12
a covalent bond between H and O. C)
13
an ionic bond between H and another atom. D)
14
a bond that is stronger than a covalent bond. E)
15
the polar O-H bond in water.
16
3)
17
Hydrogen bonds are a major factor in the structure of A)
18
DNA. B)
19
hydrogen chloride. C)
20
dry ice. D)
21
air. E)
22
table salt.
23
4)
24
In a liquid, the strength of the intermolecular interactions is considered A)
25
very weak. B)
26
weak. C)
27
moderate. D)
28
strong. E)
29
very strong.
30
5)
31
In a solution, the solvent A)
32
is a liquid. B)
33
can be a liquid or gas. C)
34
can be a solid, liquid, or gas. D)
35
is never a solid. E)
36
is the substance present in the smallest concentration.
37
6)
38
In water, the melting point is unusually high because of A)
39
covalent bonds in the individual molecules. B)
40
ionic bonds in the individual molecules. C)
41
hydrogen bonding between the molecules. D)
42
dispersion forces between the molecules. E)
43
the heat content of the hydrogen-oxygen bonds.
44
7)
45
Which of the following molecules can form hydrogen bonds? A)
46
CH4B)
47
NaH C)
48
NH3D)
49
BH3E)
50
HI
51
8)
52
Water has a boiling point of 100 °C, and alcohol has a boiling point of 78 °C, even though water is a smaller molecule. This large difference in boiling point is due to
A)
53
weak dispersion forces in the alcohol molecules. B)
54
ionic bonds between the water molecules. C)
55
covalent bonds in the ethanol molecules. D)
56
stronger hydrogen bonds between the water molecules. E)
57
stronger hydrogen bonds between the alcohol molecules.
58
9)
59
A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the A)
60
solute. B)
61
solvent. C)
62
solution. D)
63
solid. E)
64
ionic compound.
65
10)
66
Oil does not dissolve in water because A)
67
oil is polar. B)
68
oil is nonpolar. C)
69
water is nonpolar. D)
70
water is saturated. E)
71
oil is hydrated.
72
11)
73
When KCl dissolves in water A)
74
the Cl- ions are attracted to dissolved K+ ions. B)
75
the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C)
76
the K+ ions are attracted to Cl- ions on the KCl crystal. D)
77
the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E)
78
the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
79
80
12)
81
Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?
A)
82
mineral oil, soluble in water B)
83
CaCl2, soluble in hexane C)
84
HaHCO3, soluble in water D)
85
CCl4, soluble in water E)
86
octane, soluble in water
87
13)
88
In water, a substance that ionizes completely in solution is called a A)
89
weak electrolyte. B)
90
nonelectrolyte. C)
91
semiconductor. D)
92
nonconductor. E)
93
strong electrolyte.
94
14)
95
In water, a substance that partially ionizes in solution is called a A)
96
weak electrolyte. B)
97
nonelectrolyte. C)
98
semiconductor. D)
99
nonconductor. E)
100
strong electrolyte.
101
15)
102
An equivalent is A)
103
the amount of ion that has a 1+ charge. B)
104
the amount of ion that has a 1- charge. C)
105
the amount of ion that carries 1 mole of electrical charge. D)
106
1 mole of any ion. E)
107
1 mole of an ionic compound.
108
16)
109
How many equivalents are present in 5.0 g of Al3+? A)
110
15 Eq B)
111
0.56 Eq C)
112
0.19 Eq D)
113
0.37 Eq E)
114
3 Eq
115
17)
116
How many equivalents are present in 5.0 moles of Al3+? A)
117
15 Eq B)
118
1.3 Eq C)
119
5.0 Eq D)
120
0.67 Eq E)
121
3.0 Eq
122
123
18)
124
An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution?
A)
125
0.24 g B)
126
0.80 g C)
127
0.40 g D)
128
240 g E)
129
4.0 g
130
19)
131
When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is
A)
132
dilute. B)
133
polar. C)
134
nonpolar. D)
135
saturated. E)
136
unsaturated.
137
20)
138
The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O,
A)
139
all of the KI will dissolve. B)
140
the solution will freeze. C)
141
the solution will start boiling. D)
142
a saturated solution will form. E)
143
the solution will be unsaturated.
144
21)
145
An increase in the temperature of a solution usually A)
146
increases the boiling point. B)
147
increases the solubility of a gas in the solution. C)
148
increases the solubility of a solid solute in the solution. D)
149
decreases the solubility of a solid solute in the solution. E)
150
decreases the solubility of a liquid solute in the solution.
151
22)
152
Which one of the following compounds will NOT be soluble in water? A)
153
NaOH B)
154
PbS C)
155
K2SO4 D)
156
LiNO3E)
157
MgCl2
158
23)
159
Which one of the following compounds will NOT be soluble in water? A)
160
LiOH B)
161
K2S C)
162
BaSO4 D)
163
NaNO3 E)
164
MgCl2
165
24)
166
Which one of the following compounds will be soluble in water? A)
167
AgCl B)
168
Cu(OH)2 C)
169
LiCl D)
170
CaSO4 E)
171
PbCO3
172
25)
173
Which one of the following compounds will be soluble in water? A)
174
AgBr B)
175
Cu(OH)2C)
176
NaH4Cl D)
177
CaCO3 E)
178
PbS
179
26)
180
When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?
A)
181
KCl(aq) + Pb(NO3)2 (aq) → KNO3 (aq) + PbCl2 (s) B)
182
KNO3 (aq) + PbCl2 (s) → KCl(aq) + Pb(NO3)2 (aq) C)
183
K+ (aq) + NO3-(aq) → KNO3 (aq) D)
184
2KCl (aq) + Pb(NO3)2 (aq) → 2 KNO3 (aq) + PbCl2 (s) E)
185
KCl(aq) + Pb(NO3)2 (aq) → KNO3 (aq) + PbCl(s)
186
27)
187
When solutions of NaCl and AgNO3 are mixed, A)
188
a precipitate of AgCl forms. B)
189
a precipitate of NaNO3 forms. C)
190
no precipitate forms. D)
191
precipitate of NaNO3 and AgCl form. E)
192
a precipitate of AgCl2 forms.
193
28)
194
The mass/mass percent concentration refers to A)
195
grams of solute in 1 kg of solvent. B)
196
grams of solute in 1 kg of solution. C)
197
grams of solute in 100 g of solvent. D)
198
grams of solute in 100 g of solution. E)
199
grams of solvent in 100 g of solution.
200
29)
201
The mass/volume percent concentration refers to A)
202
grams of solute in 1 L of solvent. B)
203
grams of solute in 1 L of solution. C)
204
grams of solute in 100 mL of solvent. D)
205
grams of solute in 100 mL of solution. E)
206
grams of solvent in 100 mL of solution.
207
30)
208
What is the concentration, in m/m%, of a solution prepared from 50.0 g NaCl and 150.0 g of water?
A)
209
0.250% B)
210
33.3% C)
211
40.0% D)
212
25.0% E)
213
3.00%
214
31)
215
Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?
A)
216
70. mL B)
217
0.15 mL C)
218
680 mL D)
219
470 mL E)
220
330 mL
221
32)
222
What is the concentration, in m/v%, of a solution prepared from 50. g NaCl and 2.5 L of water?
A)
223
5.0% B)
224
2.0% C)
225
0.020% D)
226
0.050% E)
227
20.%
228
33)
229
How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution?
A)
230
800. g B)
231
0.0050 g C)
232
8.0 g D)
233
2.0 g E)
234
200. g
235
34)
236
A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours?
A)
237
1700 mL B)
238
60 mL C)
239
6000 mL D)
240
17 mL E)
241
204 mL
242
35)
243
What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A)
244
18 mL B)
245
0.13 mL C)
246
13 mL D)
247
120 mL E)
248
8.0 x 102 mL
249
36)
250
How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH? A)
251
25 mL B)
252
75 mL C)
253
33 mL D)
254
19 mL E)
255
3.0 x 102 mL
256
37)
257
A(n) __________ is a type of colloid in which a liquid is dispersed in another liquid or a solid. A)
258
suspension B)
259
aerosol C)
260
foam D)
261
sol E)
262
emulsion
263
38)
264
A homogeneous mixture that does not settle out upon standing is A)
265
an element. B)
266
a colloid. C)
267
a suspension. D)
268
homogeneous. E)
269
hydrated.
270
39)
271
In the process known as osmosis, __________ moves through a semipermeable membrane into an area of __________ concentration.
A)
272
solute; lower solute B)
273
solute; higher solute C)
274
solvent; lower solute D)
275
solvent; lower solvent E)
276
solvent; higher solvent
277
For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
40)
278
Which starch solution will decrease in volume as osmosis occurs? A)
279
4% B)
280
10% C)
281
Neither exerts osmotic pressure. D)
282
They exert equal osmotic pressures. E)
283
They exert opposite osmotic pressures.
284
41)
285
The process that occurs in this system is A)
286
filtration. B)
287
hydration. C)
288
neutralization. D)
289
dialysis. E)
290
osmosis.
291
42)
292
Which of the following also occurs in this system? A)
293
Water flows equally in both directions. B)
294
There is a net flow of water from the 4% starch solution into the 10% starch solution. C)
295
There is a net flow of water from the 10% starch solution into the 4% starch solution. D)
296
Water does not cross the membrane at all. E)
297
Starch moves out of the 10% starch solution into the 4% starch solution.
298
43)
299
A solution with the same osmotic pressure as the blood is A)
300
isotonic to the blood. B)
301
hypotonic to the blood. C)
302
hypertonic to the blood. D)
303
nontonic to the blood. E)
304
molar to the blood.
305
44)
306
A solution that has an osmotic pressure less than that of red blood cells is called A)
307
saturated. B)
308
hypertonic. C)
309
isotonic. D)
310
hypotonic. E)
311
unsaturated.
312
45)
313
A red blood cell will undergo crenation in A)
314
water. B)
315
0.5% NaCl. C)
316
3% glucose. D)
317
5% glucose. E)
318
7% NaCl.
319
46)
320
Which solution is isotonic to a red blood cell? A)
321
water B)
322
0.5% NaCl C)
323
2% glucose D)
324
0.9% NaCl E)
325
10% glucose
326
47)
327
A red blood cell will undergo hemolysis in A)
328
water. B)
329
0.9% NaCl. C)
330
5% glucose. D)
331
5% NaCl. E)
332
10% glucose.
333
334
48)
335
The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called
A)
336
osmotic pressure. B)
337
dialysis. C)
338
solvation. D)
339
dilution. E)
340
hydration.
341
49)
342
An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid) is placed in a dialyzing bag and immersed in distilled water. Which of the following correctly describes the location of the indicated substance after dialysis?
A)
343
albumin, inside B)
344
starch outside C)
345
albumin inside and outside D)
346
water inside only E)
347
starch inside and outside
348
50)
349
What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution? A)
350
34 M B)
351
2.0 M C)
352
0.50 M D)
353
0.029 M E)
354
1.0 M
355
51)
356
What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution?
A)
357
3.25 M B)
358
6.50 M C)
359
0.0130 M D)
360
13.0 M E)
361
2.60 M
362
52)
363
When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.)
A)
364
12%. B)
365
4.0%. C)
366
36%. D)
367
6.0%. E)
368
8.0%.
369
53)
370
The molarity (M) of a solution refers to A)
371
moles of solute/L of solution. B)
372
moles of solute/L of solvent. C)
373
moles of solute/100 mL of solution. D)
374
grams of solute/100 mL of solution. E)
375
grams of solute/L of solution.
376
54)
377
What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution? A)
378
2.5 M B)
379
1.0 M C)
380
5.0 M D)
381
10. M E)
382
2.0 M
383
55)
384
What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?
A)
385
0.500 M B)
386
1.00 M C)
387
1.50 M D)
388
2.00 M E)
389
4.00 M
390
56)
391
How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution? A)
392
750 moles B)
393
1.3 moles C)
394
83 moles D)
395
0.75 mole E)
396
3.0 moles
397
57)
398
What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH? A)
399
3.0 L B)
400
0.50 L C)
401
2.0 L D)
402
4.5 L E)
403
0.22 L
404
58)
405
During the process of diluting a solution to a lower concentration, A)
406
the amount of solute does not change. B)
407
the amount of solvent does not change. C)
408
there is more solute in the concentrated solution. D)
409
the volume of the solution does not change. E)
410
water is removed from the concentrated solution.
411
59)
412
According to Henry's law, the solubility of a gas in a liquid A)
413
decreases as the gas pressure above the liquid increases. B)
414
increases as the gas pressure above the liquid increases. C)
415
remains the same as the temperature increases. D)
416
depends on the liquid polarity. E)
417
depends on the liquid density.
418
419
60)
420
What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?
A)
421
0.267 M B)
422
0.150 M C)
423
0.200 M D)
424
6.67 M E)
425
0.100 M
426
61)
427
What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution? A)
428
0.0040 mL B)
429
63 mL C)
430
0.10 mL D)
431
125 mL E)
432
250 mL
433
62)
434
What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A)
435
0.075 L B)
436
0.25 L C)
437
0.75 L D)
438
0.083 L E)
439
750 L
440
63)
441
What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution?
A)
442
0.0400 mL B)
443
25.0 mL C)
444
2.00 mL D)
445
1.00 x mL E)
446
5.00 x mL
447
64)
448
What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL?
A)
449
2% B)
450
1% C)
451
6% D)
452
12% E)
453
18%
454
65)
455
Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l)What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)?
A)
456
34.2 L B)
457
17.1 mL C)
458
34.2 mL D)
459
10.7 mL E)
460
53.4 mL
461
8.2
462
Bimodal Questions1)
463
Acetic acid can be classified as a __________. A)
464
gas B)
465
solid C)
466
weak electrolyte D)
467
strong electrolyte E)
468
ionic compound
469
2)
470
NaCl can be classified as a __________. A)
471
gas B)
472
liquid C)
473
weak electrolyte D)
474
strong electrolyte E)
475
nonelectrolyte
476
3)
477
Methanol, CH3OH, can be classified as a __________. A)
478
gas B)
479
solid C)
480
weak electrolyte D)
481
strong electrolyte E)
482
nonelectrolyte
483
4)
484
Using a kidney machine to remove waste products from the blood is known as __________. A)
485
osmosis B)
486
osmolysis C)
487
autolysis D)
488
hemolysis E)
489
hemodialysis
490
5)
491
A mixture in which one component settles is called a(n) __________. A)
492
solution B)
493
colloid C)
494
suspension D)
495
electrolyte E)
496
nonelectrolyte
497
6)
498
The molarity of a solution of 5.0 g of KCl in 100. mL of solution is __________. A)
499
0.038 M B)
500
0.067 M C)
501
0.67 M D)
502
0.13 M E)
503
1.3 M
504
505
7)
506
If 100. mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is __________. A)
507
25 M B)
508
1.0 M C)
509
5.0 M D)
510
2.0 M E)
511
1.3 M Answer :
512
B
8.3
513
Short Answer Questions1)
514
Is barium sulfate, BaSO4, soluble or insoluble in water? Answer :
515
insoluble
2)
516
In the following equation, __________ will precipitate out of water solution.
NaCl + AgNO3 → AgCl + NaNO3
517
3)
518
In the following equation, __________ will precipitate from solution.
BaCl2 + H2SO4 → BaSO4 + 2HCl
519
4)
520
The number of moles of a compound dissolved in one liter of a solution is called the __________.
521
5)
522
A substance that carries an electric current when dissolved in water is called a(n) __________.
523
6)
524
A substance that produces only a small number of ions in solution is known as a __________ electrolyte.
525
7)
526
A solution of sodium carbonate, Na2CO3, that has a molarity of 0.0100 M contains __________ equivalents of carbonate per liter of the solution.
527
8)
528
A solution of sodium carbonate, Na2CO3, that has a molarity of 0.0100 M contains __________ equivalents of sodium ions per liter of the solution.
529
9)
530
Substances whose particles in solution scatter light and pass through filters but cannot pass through semipermeable membranes are called __________.
531
532
8.4
533
Matching QuestionsIdentify the term defined in each description.
1)
534
a solution that contains the highest amount of solute that dissolves at a given temperature
535
A)
536
hydration B)
537
saturated
C)
538
unsaturated 2)
539
the major attraction between water molecules
540
D)
541
hydrogen bonding
3)
542
the association of several water molecules with ions produced in a solution
543
E)
544
hypertonic F)
545
hypotonic
4)
546
a solution in which more solute can be dissolved
5)
547
a solution that has a higher osmotic pressure than the red blood cells of the body
548
549
550
551
552
553
554
555
556
Match the type of mixture with the appropriate characteristics.
6)
557
a mixture of sodium chloride in water
558
A)
559
colloid B)
560
suspension 7)
561
a mixture whose particles settle on standing
562
C)
563
solution
8)
564
a homogeneous mixture in which suspended particles cannot pass through a semipermeable membrane
9)
565
a mixture whose particles cannot be separated by filters or semipermeable membranes
10)
566
a mixture whose particles can be separated by filters
567
568
569
570
571
572
573
574
575
576
Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells.
11)
577
water
578
A)
579
hypotonic
12)
580
0.5% NaCl
581
B)
582
isotonic
13)
583
7% glucose
584
C)
585
hypertonic
14)
586
5% glucose
15)
587
0.9% NaCl
588
589
590
591
592
593
594
595
596
Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both.
16)
597
NaCl, a strong electrolyte
598
A)
599
both
17)
600
HI, a weak electrolyte
601
B)
602
ions
18)
603
CH3CH3OH, a nonelectrolyte
604
C)
605
molecules
19)
606
KNO3, a strong electrolyte
20)
607
glucose, a nonelectrolyte
21)
608
H2CO3, a weak electrolyte
609
610
611
612
613
614
615
616
617
618
619
620
