Key Question #15 - left. 76A) a) When a small amount of...

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Lesson 16 Key Questions 77) a) An oxidizing agent accepts electrons and, consequently become reduced. b) 572 c) A reducing agent gives-up electrons and become oxidized. d) 72) a) Cl - d) HSO 4 - b) CH 3 - e) NH 2 - c) HSO 3 2- f) ClO 4 - 72) a) Lewis acid: [Fe 4 3+ ] - Lewis base: [H 2 0] 6 b) Lewis acid: [BF 3 + ] - Lewis base: [NH 3 - ] c) Lewis acid: [BF 3 + ] - Lewis base: [F - ] d) Lewis acid: [H + ] - Lewis base: [Cl - ] 73) c) releases hydrogen ions in an aqueous solution. 74) d) 10 -5 75) HF + H 2 O H 3 O + + F - HF = 1 + 19 = 20 g/mol (2g) / (20 g/mol) = 0.1 mol of HF H 3 O + = 1 x 10 -2.2 = 0.0063 mol/L F - = 0.0063 mol/L
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K a = [H 3 O + ][F - ] / [HF] = (0.0063)(0.0063) / (0.1) = 3.97 x 10 -4 76) a) The bases competing for protons are: B - and X - . b) The stronger base is: B - . c) The weaker acid is: HB. d) The k value would be large. e) By adding the soluble salt NaB it would shift the equilibrium to the
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Unformatted text preview: left. 76A) a) When a small amount of acid is added, the reaction will shift towards the left (the formation of reactants is favoured). When the acid dissociates the H 3 O + generated will be neutralized by the buffer. In general buffers resist change. The hydrogen ion will be used to create more H 2 PO 4-. This will cause the pH to say relatively the same because the concentration of H + is very negligible because it is so small. b) When a small amount of base is added, the reaction will shift towards the right (the formation of products will be favoured). When the base becomes dissociated, the hydroxide ions (OH-) will be used up in the reaction to create more HPO 4 2-, therefore the blood is neutralized and the pH remains the same....
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Key Question #15 - left. 76A) a) When a small amount of...

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