We’re being asked **to calculate the equilibrium concentration of chloroacetic acid (ClCH _{2}COOH) ** if the

Recall that the ** percent dissociation **is given by:

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{dissociation}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{H}}^{\mathbf{+}}\mathbf{\right]}}{\mathbf{[}{\mathbf{ClCH}}_{\mathbf{2}}\mathbf{COOH}{\mathbf{]}}_{\mathbf{initial}}}{\mathbf{\times}}{\mathbf{100}}}$

Remember that ** weak acids** partially dissociate in water and that

The dissociation of ClCH_{2}COOH is as follows:

**ClCH _{2}COOH**

A 0.100 M solution of chloroacetic acid (ClCH_{2} COOH) is 11.0% ionized.

Using this information, calculate [ClCH_{2} COOH] for chloroacetic acid.

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