Explanation Given The concentration of phenylacetic acid solution is 0.085 M . The pH of the solution is 2.68 . Phenylacetic acid ( C 6 H 5 CH 2 COOH ) is a weak acid so it will ionize partially and release H + ions in the aqueous solution. The chemical reaction of phenylacetic acid in aqueous solution with H + ion as a product is, C 6 H 5 CH 2 COOH ( a q ) ⇌ H + ( a q ) + C 6 H 5 CH 2 COO − ( a q ) pH is the negative logarithm in the base 10 of [ H + ] . The concentration of H + ion is calculated by the formula, pH = − log [ H + ] [ H + ] = 10 − pH Where, [ H + ] is the concentration of H + ions. Substitute the value of pH in the above formula. [ H + ] = 10 − 2 .68 = 2.08 × 10 − 3 M K a is the dissociation constant of acids. Weak acids ionize partially in aqueous solution. So, the dissociation constant of acids is used for determining the extent to which a weak acid ionizes. The initial concentration of phenylacetic acid is 0.085 M and the concentration of H + ion after dissociation is 2.08 × 10 − 3 M . The ICE table for the dissociation reaction of lactic acid is, C 6 H 5 CH 2 COOH ( a q ) ⇌ H + ( a q ) + C 6 H 5 CH 2 COO − ( a q ) Initial: 0.085 M 0 0 Change: − 2.08 × 10 − 3 M 2.08 × 10 − 3 M 2

Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP

14th Edition

ISBN: 9780134661483

Author: Edward L Waterman

Publisher: PEARSON

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Chapter 16, Problem 52E

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To determine: The dissociation constant (Ka) for phenylacetic acid.

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Chapter 16, Problem 51E

Chapter 16, Problem 53E

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9 7 8 C 9 8 200 190 B 5 A -197.72 9 8 7 15 4 3 0: ང་ 200 190 180 147.52 134.98 170 160 150 140 130 120 110 100 90 90 OH 10 4 3 1 2 -143.04 140. 180 170 160 150 140 130 120 110 100 90 CI 3 5 1 2 141.89 140.07 200 190 180 170 160 150 140 130 120 110 100 ៖- 90 129. 126.25 80 70 60 -60 50 40 10 125.19 -129.21 80 70 3.0 20 20 -8 60 50 10 ppm -20 40 128.31 80 80 70 60 50 40 40 -70.27 3.0 20 10 ppm 00˚0-- 77.17 30 20 20 -45.36 10 ppm -0.00 26.48 22.32 ―30.10 ―-0.00

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C 5 4 3 CI 2 the Righ B A 5 4 3 The Lich. OH 10 4 5 3 1 LOOP- -147.52 T 77.17 -45.36 200 190 180 170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 ppm B -126.25 77.03 200 190 180 170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 ppm 200 190 180 170 160 150 140 130 120 110 100 90 80 TO LL <-50.00 70 60 50 40 30 20 10 ppm 45.06 30.18 -26.45 22.36 --0.00 45.07 7.5 1.93 2.05 -30.24 -22.36 C A 7 8 5 ° 4 3 7.5 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 1.0 ppm 9 8 5 4 3 ཡི་ OH 10 2 7.5 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 5 4 3 2 that th 7 I 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 115 2.21 4.00 1.0 ppm 6.96 2.76 5.01 1.0 ppm 6.30 1.00

Chapter 16 Solutions

Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP

Ch. 16.2 - Practice Exercise 1 Consider the following...Ch. 16.2 - Prob. 16.1.2PE Ch. 16.2 - Prob. 16.2.1PE Ch. 16.2 - Practice Exercise 2 When lithium oxide (Li2O) is...Ch. 16.2 - Based on information in Figure 16.4, place the...Ch. 16.2 - Practice Exercise 2 For each reaction, use Figure...Ch. 16.3 - Practice Exercise 1 In a certain acidic solution...Ch. 16.3 - Practice Exercise 2 Indicate whether solutions...Ch. 16.3 - Prob. 16.5.1PE Ch. 16.3 - Prob. 16.5.2PE

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The dissociation constant ( K a ) for phenylacetic acid.

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To determine: The dissociation constant (Ka) for phenylacetic acid.

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Chapter 16 Solutions