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CHAPTER 15 ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ Acids and Bases ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ You should read this chapter if you need to review or learn about: ➜ Brønsted-Lowery acid-base theory Acid-base strength ➜ ➜ Kw ➜ ➜ ➜ ➜ pH calculations Acid-base equilibria ➜ Ka, Kb Acid-base properties of salts and oxides Lewis acids and bases 219 Copyright © 2007 by John Moore and Richard Langley. Click here for terms of use.
220 CHEMISTRY FOR THE UTTERLY CONFUSED Get Started Our goal in this chapter is to help you understand the equilibrium systems involving acids and bases. If you don’t recall the Arrhenius acid-base theory, refer to Chapter 4 on Aqueous Solutions. You will learn a couple of other acidbase theories, the concept of pH, and will apply those basic equilibrium techniques we covered in Chapter 14 to acid-base systems. In addition, you will need to be familiar with the log and 10 x functions of your calculator. And, as usual, in order to do well you must Practice, Practice, Practice. 15-1 Brønsted-Lowery Acids and Bases An acid in the Brønsted-Lowery theory is an H + donor and a base is an H + acceptor. In the Brønsted-Lowery acid-base theory, there is a competition for an H + . Consider the acid-base reaction between acetic acid, a weak acid, and ammonia, a weak base: CH 3COOH(aq) NH 3(aq) K CH 3COO (aq) NH 4 (aq) Acetic acid donates a proton to ammonia in the forward (left to right) reaction of the equilibrium to form the acetate and ammonium ions. However, in the reverse (right to left) reaction, the ammonium ion donates a proton to the acetate ion to form ammonia and acetic acid. The ammonium ion is acting as an acid and the acetate ion a base. Under the Brønsted-Lowery system, acetic acid (CH 3COOH) and the acetate ion (CH 3COO ) are conjugate acid-base pairs. Conjugate acidbase pairs differ by only a single H . Ammonia (NH 3) and the ammonium ion (NH 4 ) are also conjugate acid-base pairs. In this reaction, there is a competition for the H between acetate ion and ammonia. In order to predict on which side the equilibrium will lie, this general rule applies: the equilibrium will favor (shift towards) the side in which the weakest acid and base are present. 15-2 Strength of Acids and Bases In Chapter 4, we introduced the concept of acids and bases. Acids and bases may be strong or weak. Strong acids completely dissociate in water and weak acids only partially dissociate. For example, consider two acids HCl (strong) and CH 3COOH (weak). If we add each to water to form aqueous solutions, the following reactions take place: HCl(aq) H 2O(l) l H 3O (aq) Cl (aq) CH 3COOH(aq) H 2O(l) K H 3O (aq) CH 3COO (aq)
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Chemistry for the Utterly Confused
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We would like to dedicate this book
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Contents ix Chapter 5 Gases 79 Do I
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Contents xi Get Started 146 10-1 Mo
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Contents xiii 15-4 pH 222 15-5 Acid
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Contents xv Chapter 20 Nuclear Chem
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CHAPTER 1 ◆◆◆◆◆◆◆◆
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Chemistry: First Steps 3 compound b
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Chemistry: First Steps 5 exact norm
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Chemistry: First Steps 7 We now nee
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Chemistry: First Steps 9 mathematic
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Chemistry: First Steps 11 we do not
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Chemistry: First Steps 13 19. How m
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CHAPTER 2 ◆◆◆◆◆◆◆◆
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Atoms, Ions, and Molecules 17 Caref
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Atoms, Ions, and Molecules 19 table
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Atoms, Ions, and Molecules 21 If a
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Atoms, Ions, and Molecules 23 Once
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Atoms, Ions, and Molecules 25 and n
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Atoms, Ions, and Molecules 27 1. Th
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Atoms, Ions, and Molecules 29 20. N
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CHAPTER 3 ◆◆◆◆◆◆◆◆
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Mass, Moles, and Equations 33 Caref
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Mass, Moles, and Equations 35 Quick
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Mass, Moles, and Equations 41 Caref
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Mass, Moles, and Equations 43 the b
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Mass, Moles, and Equations 45 7. Th
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Mass, Moles, and Equations 47 17. a
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CHAPTER 4 ◆◆◆◆◆◆◆◆
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Aqueous Solutions 51 4-2 Solubility
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Aqueous Solutions 53 Don’t Forget
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Aqueous Solutions 55 Quick Tip Cert
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Aqueous Solutions 57 Quick Tip Quic
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Aqueous Solutions 63 Quick Tip Mg(N
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Aqueous Solutions 65 All the separa
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Aqueous Solutions 69 There will be
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Aqueous Solutions 75 The calculatio
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Aqueous Solutions 77 25. The titrat
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CHAPTER 5 ◆◆◆◆◆◆◆◆
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Gases 81 Quick Tip Don’t Forget!
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Gases 83 Quick Tip Let’s see how
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Gases 85 Don’t Forget! Quick Tip
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Gases 87 Second, the KMT relates th
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Gases 89 The larger the gas particl
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Gases 91 Note that the mandatory co
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Gases 93 If it was not clear before
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Gases 95 ANSWER KEY 1. PTotal PA
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CHAPTER 6 ◆◆◆◆◆◆◆◆
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Thermochemistry 99 Quick Tip Don’
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Thermochemistry 101 Don’t Forget!
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Thermochemistry 103 C2H2(g) (5/2) O
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Thermochemistry 105 Quick Tip Some
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CHAPTER 7 ◆◆◆◆◆◆◆◆
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Quantum Theory and Electrons 109 Al
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Quantum Theory and Electrons 111 Th
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Quantum Theory and Electrons 113 Do
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Quantum Theory and Electrons 115 Do
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Quantum Theory and Electrons 117 AN
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CHAPTER 8 ◆◆◆◆◆◆◆◆
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Periodic Trends 121 8-2 Ionization
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Periodic Trends 123 The general tre
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Periodic Trends 125 in its ground s
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CHAPTER 9 ◆◆◆◆◆◆◆◆
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Chemical Bonding 129 Quick Tip In S
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Chemical Bonding 131 9-3 Ionic Bond
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Chemical Bonding 133 Quick Tip Neve
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Chemical Bonding 135 Don’t Forget
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Chemical Bonding 137 9-6 Bond Energ
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Chemical Bonding 139 Quick Tip invo
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Chemical Bonding 141 Quick Tip Elem
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Chemical Bonding 143 11. a 12. b 13
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CHAPTER 10 ◆◆◆◆◆◆◆◆
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Molecular Geometry and Hybridizatio
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CHAPTER 11 ◆◆◆◆◆◆◆◆
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Intermolecular Forces, Solids and L
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Page 192 and 193: Intermolecular Forces, Solids and L
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Page 196 and 197: Solutions 173 ways of expressing th
Page 198 and 199: Solutions 175 Don’t Forget! Don
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Page 202 and 203: Solutions 179 Just as the freezing
Page 204 and 205: Solutions 181 Don’t Forget! Using
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Page 208 and 209: Solutions 185 3. All methods of num
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Page 212 and 213: Kinetics 189 4. Physical state of r
Page 214 and 215: Kinetics 191 Don’t Forget! consta
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Page 218 and 219: Kinetics 195 Quick Tip Careful! Rem
Page 220 and 221: Kinetics 197 The decomposition of h
Page 222 and 223: Kinetics 199 reaction is first orde
Page 224 and 225: Kinetics 201 energy of a reaction.
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Page 228 and 229: Chemical Equilibria 205 Quick Tip D
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Page 238 and 239: Chemical Equilibria 215 Quick Tip I
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Page 244 and 245: Acids and Bases 221 Don’t Forget!
Page 246 and 247: Acids and Bases 223 The pH of pure
Page 248 and 249: Acids and Bases 225 Quick Tip Quick
Page 250 and 251: Acids and Bases 227 15-7 Lewis Acid
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Page 276 and 277: Entropy and Free Energy 253 17-2 En
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Page 286 and 287: Entropy and Free Energy 263 ANSWER
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Page 290 and 291: Electrochemistry 267 Quick Tip Some
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Electrochemistry 269 Don’t Forget
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Electrochemistry 271 We can use thi
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Electrochemistry 273 do is reverse
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Electrochemistry 275 Don’t Forget
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Electrochemistry 277 Be Careful! Th
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Electrochemistry 279 ANSWER KEY 1.
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CHAPTER 19 ◆◆◆◆◆◆◆◆
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Chemistry of the Elements 283 19-2
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Chemistry of the Elements 285 Be Ca
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Chemistry of the Elements 287 Don
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Chemistry of the Elements 289 6. Wh
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CHAPTER 20 ◆◆◆◆◆◆◆◆
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Nuclear Chemistry 293 The sum of th
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Nuclear Chemistry 295 Don’t Forge
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Nuclear Chemistry 297 that is not a
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Nuclear Chemistry 299 Don’t Forge
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Nuclear Chemistry 301 t 1/2 (ln 2)
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Nuclear Chemistry 303 1. A typical
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CHAPTER 21 ◆◆◆◆◆◆◆◆
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Organic, Biochemistry, and Polymers
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Index 327 chemical formulas, 19-21
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Index 329 Gibbs free energy (G), 25
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Index 331 octet rule, 128, 135, 140
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Index 333 viscosity, 161 voltaic ce
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