(a) Rearrange the Arrhenius equation k = a(-#) = A so that T is the subject (function) of the formula. (b) Formic acid is a weak acid with a dissociation constant K, of 1.8 x 10-4. The K. relates the concentration of the H+ ions denoted [H+] and the amount of acid dissolved denoted N by the equation: [H*]? Ка N - [H+] %3D Given that there is 0.1 moles of formic acid dissolved, calculate the pH of the solution.
(a) Rearrange the Arrhenius equation k = a(-#) = A so that T is the subject (function) of the formula. (b) Formic acid is a weak acid with a dissociation constant K, of 1.8 x 10-4. The K. relates the concentration of the H+ ions denoted [H+] and the amount of acid dissolved denoted N by the equation: [H*]? Ка N - [H+] %3D Given that there is 0.1 moles of formic acid dissolved, calculate the pH of the solution.
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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Answer the all sub parts A&B with step. Thank u and no reject. I'm Needed a solution in 60-120 minutes max thank u
![(2.5) [CHEMISTRY]
(a) Rearrange the Arrhenius equation
k = A-R)
so that T is the subject (function) of the formula.
(b) Formic acid is a weak acid with a dissociation constant Ka of 1.8 x 10-4.
The Ka relates the concentration of the Ht ions denoted [H+] and the amount of
acid dissolved denoted N by the equation:
[H*]?
Ka =
N - [H+]
Given that there is 0.1 moles of formic acid dissolved, calculate the pH of the solution.
(Hint: an applied quadratic function)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd7ebf975-dacd-4b34-a639-91267d2eadb1%2F94a581bf-af92-4bef-a222-5b2c97ac7912%2Fm9ja08o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(2.5) [CHEMISTRY]
(a) Rearrange the Arrhenius equation
k = A-R)
so that T is the subject (function) of the formula.
(b) Formic acid is a weak acid with a dissociation constant Ka of 1.8 x 10-4.
The Ka relates the concentration of the Ht ions denoted [H+] and the amount of
acid dissolved denoted N by the equation:
[H*]?
Ka =
N - [H+]
Given that there is 0.1 moles of formic acid dissolved, calculate the pH of the solution.
(Hint: an applied quadratic function)
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