Propanoic acid is a weak monoprotic acid with the formula HC3H5O2. It partially dissociates in water to release hydronium ions (H3O*) and propanoate ions (C3H5O2'¯). 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 (1) = H30*(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` [HA]o, Calculate the percent dissociation of 0.160 M HPro. % dissociation (100%) %3D
Propanoic acid is a weak monoprotic acid with the formula HC3H5O2. It partially dissociates in water to release hydronium ions (H3O*) and propanoate ions (C3H5O2'¯). 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 (1) = H30*(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` [HA]o, Calculate the percent dissociation of 0.160 M HPro. % dissociation (100%) %3D
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
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 5 only. If it cannot be done without the values from the earlier parts, please substitute the values with another variable (such as X, Y, Z), make them explicit in the working out, and solve it through. It would help me a lot even if I only saw the working out for this question. 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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F476b5cb0-a3fb-4b49-8c26-098fb10da8e5%2F2cc62f1d-4a2d-40bc-be73-e65b3ce5bbe7%2Fzfol26n_processed.png&w=3840&q=75)
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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