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Bromoacetic acid, with the chemical formula \(\mathrm{BrCH}_{2}\mathrm{COOH}\), is a weak organic acid. Its significance lies primarily in its structure because it contains a bromine atom near the acidic carboxyl group. This bromine atom increases the acid's ionization potential by weakening the \(\mathrm{O-H}\) bond in the carboxyl group, making it easier for the acid to donate a hydrogen ion \(\left(\mathrm{H}^{+}\right)\). This is an important aspect of understanding how bromoacetic acid behaves in solution.

When dissolved in water, bromoacetic acid partially dissociates, as depicted in the equation:

BrCH鈧侰OOH (aq) 鈬� H鈦� (aq) + BrCH鈧侰OO鈦� (aq).

This equilibrium represents the acid in its ionized and non-ionized forms, which helps determine concentrations at equilibrium states in solutions.

The percent ionization of an acid is a key concept in understanding acid strength and behavior in solution. It tells us what percentage of the original acid molecules have ionized into ions in a solution. For bromoacetic acid in our exercise, the percent ionization is 13.2%.

This means that out of all the bromoacetic acid molecules originally in the solution, 13.2% have dissociated to form hydrogen ions \(\left(\mathrm{H}^{+}\right)\) and conjugate base ions \(\left(\mathrm{BrCH}_{2}\mathrm{COO}^{-}\right)\).

To calculate the percent ionization, you can use the formula:

\[\text{Percent Ionization} = \left(\frac{\left[\mathrm{H}^{+}\right]_{eq}}{\left[\mathrm{HA}\right]_{\text{initial}}}\right) \times 100\]%

Knowing the percent ionization helps in determining both the degree to which a weak acid dissociates in water and the concentrations of ions at equilibrium.

Equilibrium concentrations are pivotal in chemistry, especially in acid-base reactions, to understand the outcome of the reaction's progress. For bromoacetic acid, equilibrium concentrations are calculated based on initial concentrations and changes due to ionization.

Initially, the concentration of bromoacetic acid was 0.100 M, with no \(\left[\mathrm{H}^{+}\right]\) or \(\left[\mathrm{BrCH}_{2}\mathrm{COO}^{-}\right]\). As ionization occurs, these concentrations change.

Given a 13.2% ionization rate, the change in concentration for each ion and the molecule is calculated as follows:

- Change in \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{BrCH}_{2}\mathrm{COO}^{-}\right]\) = 13.2% of 0.100 M = 0.0132 M
- Change in \(\left[\mathrm{BrCH}_{2}\mathrm{COOH}\right]\) is negative due to consumption and equals -0.0132 M.

So, the equilibrium concentrations are:

• [H鈦篯 = 0.0132 M
• [BrCH鈧侰OO鈦籡 = 0.0132 M
• [BrCH鈧侰OOH] = 0.0868 M

These values indicate the balance achieved in the reaction, reflecting both ionized and non-ionized forms of bromoacetic acid.