Chap 5 questions - 1. For the following reaction of...

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1. For the following reaction of hypochlorous acid (HOCl) with water, HOCl + H 2 O <==> H 3 O + + OCl - what would be the effect of adding sodium hypochlorite (NaOCl) to the reaction at equilibrium? a. The concentrations of both HOCl and H 3 O + would increase. b. The concentrations of both HOCl and H 3 O + would decrease. c. The concentration of HOCl would increase and the concentration of H 3 O + would decrease. d. The concentration of HOCl would decrease and the concentration of H 3 O + would increase. e. There would be no change because sodium hypochlorite is a salt without any acidic or basic properties. 2. Calculate the molar hydronium ion concentration in a solution containing 0.23 M hypochlorous acid (HOCl), a monoprotic weak acid used in bleach solutions. For HOCl, K a = 2.9 x 10 -8 . 3. Given three separate solutions containing equal concentrations of formic acid (K a = 1.7 x 10 -4 ), phenol (K a = 1.3 x 10 -10 ), and acetic acid (K a = 1.8 x 10 -5 ), select the response below that has the acids arranged in order of increasing percent dissociation at equilibrium. a. formic < phenol < acetic b. formic < acetic < phenol c. acetic < formic < phenol d. phenol < acetic < formic e. No response is correct. 4. From the following choices, select the one that would be the most basic (least acidic). a. 0.1 M hydrochloric acid (a strong acid) b. 0.1 M acetic acid (a weak acid) c. 0.1 M sodium acetate (the salt of a weak acid) d. 0.1 M ammonium chloride (the salt of a weak base) e. pure water 5. The reactions of perchloric acid (HClO 4 ) and acetic acid (HOAc) in water can be written as: 6. HClO 4 + H 2 O --> H 3 O + + ClO 4 - and 7. 8. HOAc + H 2 O <=> H 3 O + + OAc - From these reactions it can be concluded that: a. acetic acid is a stronger acid than perchloric acid. b. acetate ion is a weaker base than perchlorate ion. c. acetate ion is a stronger base than perchlorate ion. d. water is a very strong acid. e. none of the above is correct. 9. If 10 mL a 1.0 x 10 -4 M solution of a strong acid were added to 100 mL each of one solution containing 1.8 x 10 -5 M hydrochloric acid and a second solution containing 1.0 M acetic acid (K a = 1.8 x 10 -5 ) plus 1.0 M sodium acetate, it is expected that the:
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a. pH of both solutions would remain unchanged. b. change in pH would be very large in both solutions. c. change in pH would be the same in both solutions. d. change in pH would be larger in the solution containing acetic acid and sodium acetate. e. change in pH would be larger in the HCl solution. 10. Addition of a strong acid to a solution of acetic acid at equilibrium (HOAc + H 2 O <=> H 3 O + + OAc - ) would cause the: a. acetate ion concentration to decrease. b. acetate ion concentration to increase. c.
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This note was uploaded on 02/05/2012 for the course CHEM 116 taught by Professor Stevenson during the Fall '08 term at Purdue University-West Lafayette.

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Chap 5 questions - 1. For the following reaction of...

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