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The problem in the image asks to calculate the percent dissociation of 4-chlorobutanoic acid (C₄H₆ClCO₂H) in a 2.2 M aqueous solution. To find the percent dissociation, you will need to use the formula:

\[
\text{Percent Dissociation} = \frac{[\text{H}^+]}{[\text{HA}]_0} \times 100
\]

Where:
- \([\text{H}^+]\) is the concentration of hydrogen ions (or hydronium ions) at equilibrium,
- \([\text{HA}]_0\) is the initial concentration of the weak acid (2.2 M in this case).

Steps to solve:
1. **Use the acid dissociation constant (\(K_a\))**: You need the \(K_a\) value for 4-chlorobutanoic acid, which can be found in the ALEKS Data resource. The formula for the dissociation constant is:
   \[
   K_a = \frac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}
   \]
   where \([\text{A}^-]\) is the concentration of the conjugate base, and \([\text{HA}]\) is the concentration of undissociated acid at equilibrium.

2. **Set up an ICE (Initial, Change, Equilibrium) table**: This table will help you express the concentrations at equilibrium in terms of \(x\), the amount of dissociation.
   
3. **Solve for \(x\)**: Once you have the equilibrium expression in terms of \(x\) and \(K_a\), solve for \(x\), which gives the concentration of \([\text{H}^+]\).

4. **Calculate percent dissociation**: Finally, use the formula for percent dissociation, where \(x\) represents the \([\text{H}^+]\).

Do you have the \(K_a\) value from the ALEKS resource, or would you like help with further steps?

### Would you like a detailed explanation on:
1. How to find \(K_a\) values from tables?
2. How to set up and solve an ICE table?
3. How to use equilibrium expressions in weak acid calculations?
4. How to apply approximations for weak acid dissociation?
5. The significance of percent dissociation in acid-base chemistry?

### Tip:
In weak acid problems, if the acid dissociation is very small, you can often approximate the initial concentration of the acid to stay nearly unchanged at equilibrium, simplifying calculations.

Calculate the percent dissociation of 4-chlorobutanoic acid (C₄H₆ClCO₂H) in a 2.2 M aqueous solution. Round your answer to 2 significant digits.

Learn how to calculate the percent dissociation of 4-chlorobutanoic acid (C₄H₆ClCO₂H) in a 2.2 M solution. This problem involves key chemistry concepts like weak acid equilibria and percent dissociation, suitable for high school or college-level students.

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