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Buffers and Other Equilibria 249 The common-ion effect is an application of Le Châtelier’s principle to equilibrium systems of slightly soluble salts. A buffer is a solution that resists a change in pH if we add an acid or base. We can calculate the pH of a buffer using the Henderson-Hasselbalch equation. We use titrations to determine the concentration of an acid or base solution. We can represent solubility equilibria by the solubility product constant expression, K sp. We can use the concepts associated with weak acids and bases to calculate the pH at any point during a titration. 1. Write the Henderson-Hasselbalch equation for pH and for pOH. 2. Complete the following table for use with buffer solutions: [HA] [A ] HNO2 _____ _____ HCO3 _____ CH3NH3 NH3 _____ 2 HPO4 _____ 3. Write equilibrium constant expressions (K sp) for the addition of each of the following substances to water. a. AgBr b. Ag 2SO 4 c. AlF 3 d. CaCO 3 e. Ca 3(PO 4) 2 4. Write an equilibrium constant expression (K f) for the formation of the Ag(NH 3) 2 ion. 5. Calculate the molar solubility of calcium carbonate, CaCO 3 that will dissolve in each of the following. The K sp for calcium carbonate is 8.7 10 9 . a. in pure water b. in 6.5 10 2 M Ca 2 c. in 0.35 M CO 3 2 solution. 6. Determine the pH of each of the following buffer solutions. a. 0.15 M HC 2H 3O 2 and 0.15 M C 2H 3O 2 with pKa 4.76 b. 0.25 M NH 3 and 0.30 M NH 4 with pKb 4.76 c. 1.0 M HF and 0.75 M F with K a 6.8 10 4 d. 1.2 M C 5H 5N and 0.75 M HC 5H 5N with K b 1.5 10 9 e. 0.60 M HCO 3 and 0.80 M CO3 2 with pKa1 6.35 and pK a2 10.32 7. The pH of a 50.00-mL sample of 0.06000 M strontium hydroxide is measured as it is titrated with a 0.1200 M hydrochloric acid. Determine the pH of the solution after the following total volumes of hydrochloric acid have been added. a. 0.00 mL b. 25.00 mL c. 50.00 mL d. 75.00 mL 8. The pH of a 50.00-mL sample of 0.1100 M ammonia, NH 3, is measured as it is titrated with a 0.1100 M hydrochloric acid, HCl. Determine the pH of the solution after the following total volumes of hydrochloric acid have been added. a. 0.00 mL b. 25.00 mL c. 50.00 mL d. 75.00 mL (K b for NH 3 is 1.76 10 5 .)
250 CHEMISTRY FOR THE UTTERLY CONFUSED ANSWER KEY [A 1. pH pKa log pOH pKb log ] [HA] 2. [HA] [A ] HNO 2 NO 2 NH 4 NH 3 HCO 3 CO 3 2 H 2PO 4 HPO 4 2 CH 3NH 3 CH 3NH 2 3. a. K sp [Ag ] [Br ] b. K sp [Ag ] 2 [SO 4 2 ] c. Ksp [Al 3 ] [F ] 3 d. K sp [Ca 2 ] [CO 3 2 ] e. Ksp [Ca 2 ] 3 [PO 4 3 ] 2 4. K f [Ag ] [NH 3] 2 5. K sp [Ca 2 ] [CO 3 2 ] 8.7 10 9 [HA] [A ] a. 9.3 105 M b. 1.3 107 M c. 2.5 108 M 6. a. pH 4.76 b. pH 9.16 c. pH 3.04 d. pH 5.38 e. pH 10.44 (only pKa2 is necessary) 7. a. pH 13.079 b. pH 12.602 c. pH 7.000 d. pH 1.620 8. a. pH 11.14 b. pH 9.25 c. pH 5.25 d. pH 1.66
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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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CHAPTER 12 ◆◆◆◆◆◆◆◆
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Solutions 173 ways of expressing th
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Solutions 175 Don’t Forget! Don
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Solutions 177 12-3 Colligative Prop
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Solutions 179 Just as the freezing
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Solutions 181 Don’t Forget! Using
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Solutions 183 Quick Tip A molar mas
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Solutions 185 3. All methods of num
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CHAPTER 13 ◆◆◆◆◆◆◆◆
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Kinetics 189 4. Physical state of r
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Kinetics 191 Don’t Forget! consta
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Kinetics 193 Don’t Forget! the co
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Kinetics 195 Quick Tip Careful! Rem
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Kinetics 197 The decomposition of h
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Page 316 and 317: Nuclear Chemistry 293 The sum of th
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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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Untitled - Kelly Walsh High School

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