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18. If the acetic acid dissociation constant is Ka-1.8 X 10 and its concentration before dissolution is( 0.34M), the concentration of [H ] in an acid solution is equal to the following equation CH3COOH CH;COO +H* A) 3.52X103 B) 2.47X103 C) 3.52X105 D) 2.47X105

18. If the acetic acid dissociation constant is Ka-1.8 X 10 and its concentration before dissolution is( 0.34M), the concentration of [H ] in an acid solution is equal to the following equation CH3COOH CH;COO +H* A) 3.52X103 B) 2.47X103 C) 3.52X105 D) 2.47X105

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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18. If the acetic acid dissociation constant is Ka= 1.8 X 105 and its concentration before dissolution is( 0.34M), the concentration of [H ] in an acid solution is equal to the following equation CH3COOH CH;COO +H* A) 3.52X103 B) 2.47X103 C) 3.52X105 D) 2.47X105 19. If K-0.45 at a (150°C) for the equilibrium reaction: %3D N2 (g)+ O2 (g) 2NO The Ke of the reaction is : A) 0.45 B) 0.54 C) 0.69 D) 0.96. 20. If K= (0.92) at a (150°C) for the equilibrium reaction: CO(g)+ 3H>(g) + CH:(g) + H2O(g) The K. of the reaction is : A) 1106.86 B) 2.32 x104 C) 4.20 x105 D) 3.29 x 10-5 .
Transcribed Image Text:18. If the acetic acid dissociation constant is Ka= 1.8 X 105 and its concentration before dissolution is( 0.34M), the concentration of [H ] in an acid solution is equal to the following equation CH3COOH CH;COO +H* A) 3.52X103 B) 2.47X103 C) 3.52X105 D) 2.47X105 19. If K-0.45 at a (150°C) for the equilibrium reaction: %3D N2 (g)+ O2 (g) 2NO The Ke of the reaction is : A) 0.45 B) 0.54 C) 0.69 D) 0.96. 20. If K= (0.92) at a (150°C) for the equilibrium reaction: CO(g)+ 3H>(g) + CH:(g) + H2O(g) The K. of the reaction is : A) 1106.86 B) 2.32 x104 C) 4.20 x105 D) 3.29 x 10-5 .
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