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3) Based on the value for [H3O*], calculate the pH of this 0.160 M HPro solution. 4) Calculate the value for [OH¯] of this 0.160 M HPro solution.

3) Based on the value for [H3O*], calculate the pH of this 0.160 M HPro solution. 4) Calculate the value for [OH¯] of this 0.160 M HPro solution.

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please solve question 3 and 4 only (they are very closely interconnected). Thank you!

Propanoic acid is a weak monoprotic acid with the formula HC3H5O2. It partially dissociates in water to release hydronium ions (H3O*) and propanoate ions (C;H5O2-). We can abbreviate propanoic acid as “HPro" and the propanoate ion as Prol-. The acid-dissociation equilibrium for propanoic acid is described below. HPro (aq) + H2O () = H3O*(aq) + Pro- (aq) At 25°C, Ka, is 1.3 × 10-5 1) Write the mass-action expression for this reaction. (As a pure liquid, H2O is not included). The K value for this reaction is equal to Ka. 2) Use an "ICE" (or "IAE" table to determine the concentrations of HPro, H3O†, and Prol- in an aqueous solution of 0.160 M HPro. 3) Based on the value for [H3O*], calculate the pH of this 0.160 M HPro solution. 4) Calculate the value for [OH¯] of this 0.160 M HPro solution. 5) The percent dissociation of a weak acid depends on the initial concentration of HA ([HA]o). It is found using this value and the equilibrium concentration of {H*] ([H*]e). ([H*]e` |(100%) THAJO. [HA], % dissociation Calculate the percent dissociation of 0.160 M HPro.
Transcribed Image Text:Propanoic acid is a weak monoprotic acid with the formula HC3H5O2. It partially dissociates in water to release hydronium ions (H3O*) and propanoate ions (C;H5O2-). We can abbreviate propanoic acid as “HPro" and the propanoate ion as Prol-. The acid-dissociation equilibrium for propanoic acid is described below. HPro (aq) + H2O () = H3O*(aq) + Pro- (aq) At 25°C, Ka, is 1.3 × 10-5 1) Write the mass-action expression for this reaction. (As a pure liquid, H2O is not included). The K value for this reaction is equal to Ka. 2) Use an "ICE" (or "IAE" table to determine the concentrations of HPro, H3O†, and Prol- in an aqueous solution of 0.160 M HPro. 3) Based on the value for [H3O*], calculate the pH of this 0.160 M HPro solution. 4) Calculate the value for [OH¯] of this 0.160 M HPro solution. 5) The percent dissociation of a weak acid depends on the initial concentration of HA ([HA]o). It is found using this value and the equilibrium concentration of {H*] ([H*]e). ([H*]e` |(100%) THAJO. [HA], % dissociation Calculate the percent dissociation of 0.160 M HPro.
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