chemistry 142 chapter 15: acids and bases outline i.definitions ii.ion-product constant for water...
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Chemistry 142Chapter 15: Acids and Bases
OutlineI. DefinitionsII. Ion-product Constant for WaterIII. pH ScaleIV. Percent DissociationV. Polyprotic AcidsVI. Salts of Acid-Base ReactionsVII. Acid Strength
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Tro, Chemistry: A Molecular Approach
2
Structures of Acids
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Tro, Chemistry: A Molecular Approach
3
Arrhenius Theory
HCl ionizes in water,producing H+ and Cl– ions
NaOH dissociates in water,producing Na+ and OH– ions
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Brønsted-Lowry Model
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Lewis Acids and Bases
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Autoionization of Water
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Hydronium Ion in Water
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Chapter 15 – Acids and BasesExample – Ion Product
15.1 What are the equilibrium concentrations of hydronium and hydroxide ions at 25
˚C?
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pH Scale
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Tro, Chemistry: A Molecular Approach
11
Acids Conjugate Bases HClO4 ClO4
-1 H2SO4 HSO4
-1
HI I-1
HBr Br-1
HCl Cl-1
HNO3 NO3-1
H3O+1 H2O
HSO4-1 SO4
-2
H2SO3 HSO3-1
H3PO4 H2PO4-1
HNO2 NO2-1
HF F-1
HC2H3O2 C2H3O2-1
H2CO3 HCO3-1
H2S HS-1
NH4+1 NH3
HCN CN-1
HCO3-1 CO3
-2
HS-1 S-2
H2O OH-1
CH3-C(O)-CH3 CH3-C(O)-CH2-1
NH3 NH2-1
CH4 CH3-1
OH-1 O-2
Incr
easi
ng A
cidi
ty
Increasing Basicity
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Weak Bases
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.3 Calculate the pH and pOH of a 1.73 x 10-3 M barium hydroxide solution.
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.4 If 250.0 mL of 0.1520 M sulfuric acid is mixed with 150.0 mL of 0.2601 M
sodium hydroxide, what is the pH of the resulting solution?
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Chapter 15 – Acids and BasesExample – Percent Dissociation
15.2 For a 1.00 M hydrofluoric acid solution, the hydronium ion concentration was found to be 2.7 x 10-2 M. What is the percent dissociation of the solution?
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Acid Strength
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Tro, Chemistry: A Molecular Approach
20
Metal Cations as Weak AcidsAl(H2O)6
3+(aq) + H2O(l) Al(H2O)5(OH)2+ (aq) + H3O+(aq)
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Chapter 15 – Acids and BasesExample – Salts
15.5 Determine whether the following aqueous solutions of salts have a pH equal to, greater than, or less than 7. If pH > 7 or pH < 7, write a chemical equation to justify your answer.
ammonium bromidesodium carbonatepotassium fluoridepotassium bromidealuminum chloridecopper(II) nitrate
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.6 Calculate the pH of a 0.20 M lactic acid, CH3CH(OH)COOH, solution. Ka = 8.4 x 10-4
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.7 Calculate the pH and percent protonation of a 0.20 M aqueous solution of methylamine, CH3NH2. The Ka of methylamine is 2.78 x 10-11.
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.8 Calculate the pH of a 0.010 M sulfuric acid solution at 25 ˚C. Ka1 is strong and Ka2 is
1.2 x 10-2.
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.9 The pH of a 0.025 M aqueous solution of a base was 11.6. What is the pKb of the base?
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.1 Calculate the molarities of sulfurous acid, bisulfite ion, sulfite ion, hydronium ion and hydroxide ion in a 0.10 M sulfurous acid solution. Ka1 = 1.5 x 10-2 and Ka2 = 1.2 x 10-7 .
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.11 A 42.07 mL sample of 0.255 M sulfuric acid is mixed 68.01 mL of 0.555 M potassium hydroxide. Determine the concentration of all of the ions in solution, the pH, and pOH.
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Chapter 15 – Acids and BasesExample – pH, pOH, pKa
15.12Calculate the pH of a solution that contains 1.00 M hydrocyanic acid (Ka = 6.2 x 10-10) and 5.00 M nitrous acid (Ka = 4.0 x 10-4). In addition calculate the concentration of cyanide ions at equilibrium.
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Chapter 15 – Acids and BasesExample – Ka
15.13When 2.55 g of an unknown weak acid (HA) with a molar mass of 85.0 g/mol is dissolved in 250.0 g of water, the freezing point of the resulting solution is -0.257 °C. Calculate the acid equilibrium constant, Ka, for the unknown weak acid (Kf for water is 1.86 °C/m)