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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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