Review_Exam4(2)

Review_Exam4(2) - 10/22/10 Chapter 15: Acids and Bases...

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Unformatted text preview: 10/22/10 Chapter 15: Acids and Bases Acid/bases definitions, the ion product of water, the pH scale (Sec. 15.1 15.3) 10/22/10 B. Brnsted Acids and Bases (Sec. 15.1) acid base base acid Brnsted acid is a substance that donates protons (the molecule must have a removable proton) Brnsted base is a substance that accepts protons (the molecule must have a pair of non-bonding electrons) 10/22/10 Clicker Questions Join Channel 43 Step-1: Press Go Step-2: Press 43 Step-3: Press Go 10/22/10 Which of one the following statements is TRUE ? A r r h e n i u s a c i d i s a p r o t . . A r r h e n i u s b a s e i s a p r o t . . B r n s t e d a c i d i s a p r o t . . B r n s t e d b a s e i s a p r o t . . 0% 0% 0% 0% 1. Arrhenius acid is a proton (H+) acceptor. 2. Arrhenius base is a proton (H+) acceptor. 3. Brnsted acid is a proton (H+) donor. 4. Brnsted base is a proton (H+) donor. 10/22/10 Which of the following is the hydroxide ion? 0% 0% 0% 0% 0% 1. H3O+ 2. OH- 3. H2O 4. H3O- 5. H2O+ 10/22/10 B. Brnsted Acids and Bases (Sec. 15.1) acid 1 base 2 base 1 acid 2 Conjugate acid-base pairs: Conjugate acid-base pairs: acid 1 base 1 acid 2 base 2 H2O is amphiprotic , i.e. could be either an acid or a base (other examples: HCO3-, HSO4-) 10/22/10 The conjugate acid of HSO4- is __________. 0% 0% 0% 0% 0% 1. SO42- 2. H2SO4 3. HSO4+ 4. H+ 5. HSO3+ 10/22/10 The conjugate base of HSO4- is __________. 0% 0% 0% 0% 0% 1. SO42- 2. H2SO4 3. HSO4+ 4. H+ 5. HSO3+ 10/22/10 B. Acid-Base Properties of Water (Sec. 15.2) Autoionization of water: O H H + O H H O H H H O H- + [ ] + acid 1 base 1 base 2 acid 2 At 250 C: Kw (= K'c[H2O]) =[H3O+][OH- ] = [H+][OH- ] = 1.0 x 10-14 Note: the reaction constant Kw has a subscript w for water and is called the ion-product constant K'c = [H3O+][OH- ] / [H2O] = [H+][OH- ] / [H2O] [H2O] =const 10/22/10 C. The pH (and pOH) Scale A Measures of Acidity (Sec. 15.3) pH = -log [H+] pH = -log [H3O+] or The pH scale: The pOH scale: pOH = -log [OH-] At 250 C: pH + pOH = pKw =14.00 The connection between the pH and pOH scales: [H+] = [OH-] [H+] > [OH-] [H+] < [OH-] neutral acidic basic [H+] = 1 x 10- 7 [H+] > 1 x 10- 7 [H+] < 1 x 10- 7 pH = 7 pH < 7 pH > 7 pH [H+ ] At 250 C the solution is: 10/22/10 What is the concentration of [H3O+] in a 9 M 7 M 7 M 5 M 2 M 3 M 0% 0% 0% 0% 0% 0% 1. 2.3 x 10-9 M 2. 1.0 x 10-17 M 3. 4.9 x 10-7 M 4. 3.45 M 5. 0.00012 M 6. 10.23 x 103 M 10/22/10 What is the pH of an aqueous solution 0% 0% 0% 0% 0% 1. 8.40 2. 7.00 3. 9.00 4. 3.98 5. 5.60 10/22/10 What is the pOH of an aqueous solution 0% 0% 0% 0% 0% 1. 4.29 2. 1.94 3. 7.00 4. 14.0 5. 9.71 10/22/10...
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Review_Exam4(2) - 10/22/10 Chapter 15: Acids and Bases...

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