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