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Find the percentage ionization of 0.2M acetic acid solution,whose dissociation constant is 1.8*10-5
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Find the percentage ionization of 0.2M acetic acid solution,whose diss...
Introduction:
The percentage ionization of a weak acid can be calculated using its dissociation constant and initial concentration. Acetic acid is a weak acid with a dissociation constant of 1.8x10^-5. In this case, we need to find the percentage ionization of a 0.2M acetic acid solution.
Formula:
The dissociation constant (Ka) of acetic acid can be expressed as:
Ka = [H+][CH3COO-]/[CH3COOH]
Steps to Calculate the Percentage Ionization:
Step 1: Calculate the concentration of H+:
Since acetic acid is a monoprotic acid, the concentration of H+ is the same as the concentration of acetic acid that ionizes.
[H+] = [CH3COOH] (initial concentration) = 0.2M
Step 2: Calculate the concentration of CH3COO-:
Using the equation for Ka, we can rearrange it to calculate the concentration of CH3COO-.
Ka = [H+][CH3COO-]/[CH3COOH]
1.8x10^-5 = [H+][CH3COO-]/0.2M
Assuming x is the concentration of CH3COO- that ionizes:
1.8x10^-5 = (0.2M - x)x/0.2M
Step 3: Solve for x:
Solving the equation from Step 2 will give us the concentration of CH3COO- that ionizes.
1.8x10^-5 = (0.2M - x)x/0.2M
1.8x10^-5 = (0.2 - x)x/0.2
Simplifying the equation and solving for x will give us the concentration of CH3COO-.
Step 4: Calculate the percentage ionization:
Now that we have the concentration of CH3COO- that ionizes, we can calculate the percentage ionization using the following formula:
Percentage Ionization = (x/[CH3COOH]) x 100
Substitute the values into the formula to find the percentage ionization.
Explanation:
The percentage ionization of a weak acid measures the extent to which it dissociates into ions in solution. In this case, we are calculating the percentage ionization of a 0.2M acetic acid solution, which has a dissociation constant (Ka) of 1.8x10^-5.
To calculate the percentage ionization, we first determine the concentration of H+. Since acetic acid is a monoprotic acid, the concentration of H+ is the same as the initial concentration of acetic acid, which is 0.2M.
Next, using the equation for Ka, we can calculate the concentration of CH3COO-. Assuming x is the concentration of CH3COO- that ionizes, we rearrange the equation to solve for x. By substituting the values, we can determine the concentration of CH3COO-.
Finally, we can calculate the percentage ionization by dividing the concentration of CH3COO- (x) by the initial concentration of acetic acid (0.2M), and then
The percentage ionization of a weak acid can be calculated using its dissociation constant and initial concentration. Acetic acid is a weak acid with a dissociation constant of 1.8x10^-5. In this case, we need to find the percentage ionization of a 0.2M acetic acid solution.
Formula:
The dissociation constant (Ka) of acetic acid can be expressed as:
Ka = [H+][CH3COO-]/[CH3COOH]
Steps to Calculate the Percentage Ionization:
Step 1: Calculate the concentration of H+:
Since acetic acid is a monoprotic acid, the concentration of H+ is the same as the concentration of acetic acid that ionizes.
[H+] = [CH3COOH] (initial concentration) = 0.2M
Step 2: Calculate the concentration of CH3COO-:
Using the equation for Ka, we can rearrange it to calculate the concentration of CH3COO-.
Ka = [H+][CH3COO-]/[CH3COOH]
1.8x10^-5 = [H+][CH3COO-]/0.2M
Assuming x is the concentration of CH3COO- that ionizes:
1.8x10^-5 = (0.2M - x)x/0.2M
Step 3: Solve for x:
Solving the equation from Step 2 will give us the concentration of CH3COO- that ionizes.
1.8x10^-5 = (0.2M - x)x/0.2M
1.8x10^-5 = (0.2 - x)x/0.2
Simplifying the equation and solving for x will give us the concentration of CH3COO-.
Step 4: Calculate the percentage ionization:
Now that we have the concentration of CH3COO- that ionizes, we can calculate the percentage ionization using the following formula:
Percentage Ionization = (x/[CH3COOH]) x 100
Substitute the values into the formula to find the percentage ionization.
Explanation:
The percentage ionization of a weak acid measures the extent to which it dissociates into ions in solution. In this case, we are calculating the percentage ionization of a 0.2M acetic acid solution, which has a dissociation constant (Ka) of 1.8x10^-5.
To calculate the percentage ionization, we first determine the concentration of H+. Since acetic acid is a monoprotic acid, the concentration of H+ is the same as the initial concentration of acetic acid, which is 0.2M.
Next, using the equation for Ka, we can calculate the concentration of CH3COO-. Assuming x is the concentration of CH3COO- that ionizes, we rearrange the equation to solve for x. By substituting the values, we can determine the concentration of CH3COO-.
Finally, we can calculate the percentage ionization by dividing the concentration of CH3COO- (x) by the initial concentration of acetic acid (0.2M), and then
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Find the percentage ionization of 0.2M acetic acid solution,whose diss...
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Find the percentage ionization of 0.2M acetic acid solution,whose dissociation constant is 1.8*10-5 for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Find the percentage ionization of 0.2M acetic acid solution,whose dissociation constant is 1.8*10-5 covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Find the percentage ionization of 0.2M acetic acid solution,whose dissociation constant is 1.8*10-5.
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