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A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant?
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A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the di...
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A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the di...
Introduction
To calculate the dissociation constant of acetic acid, we need to know the degree of ionization of the acid in a given solution. In this case, we are given that a 0.01 M solution of acetic acid is 5% ionized at 25°C. The dissociation constant, also known as the acid dissociation constant (Ka), is a measure of the strength of an acid in solution.
Formula for Dissociation Constant
The dissociation constant (Ka) for a weak acid is given by the equation:
Ka = [A-][H+]/[HA]
Where:
[A-] is the concentration of the conjugate base
[H+] is the concentration of hydrogen ions
[HA] is the concentration of the acid
Calculating the Concentration of Acid and Conjugate Base
Since acetic acid is a weak acid, it does not completely dissociate in solution. Let's assume that x moles of acetic acid dissociate into x moles of acetate ions (A-) and x moles of hydrogen ions (H+). The initial concentration of acetic acid is 0.01 M, so the concentration of acetate ions and hydrogen ions will also be x M.
Therefore, the concentration of the acid (HA) will be (0.01 - x) M.
Calculating Degree of Ionization
The degree of ionization (α) is given by the equation:
α = (x/(0.01 - x)) * 100
Given that the degree of ionization is 5%, we can substitute α = 0.05 in the equation above and solve for x.
0.05 = (x/(0.01 - x)) * 100
0.05 * (0.01 - x) = x
0.0005 - 0.05x = x
0.0005 = 1.05x
x = 0.0005/1.05
x = 0.000476 M
Therefore, the concentration of acetate ions and hydrogen ions is 0.000476 M.
Calculating Dissociation Constant
Now that we know the concentration of acetate ions ([A-]) and hydrogen ions ([H+]), as well as the concentration of the acid ([HA]), we can calculate the dissociation constant (Ka).
Ka = [A-][H+]/[HA]
= (0.000476 * 0.000476)/(0.01 - 0.000476)
= 2.268 x 10^-6
Therefore, the dissociation constant (Ka) for acetic acid is 2.268 x 10^-6.
Conclusion
In summary, to calculate the dissociation constant of acetic acid, we used the degree of ionization and the formula for the dissociation constant. By solving the equation for the degree of ionization, we found the concentration of acetate ions and hydrogen ions. Using these concentrations, we then calculated the dissociation constant of acetic acid.
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A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant?
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A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant?.
A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0.01 M solution of acetic acid is 5% ionised at 25c calculate the dissociation constant?.
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