Problem: A 0.100 M solution of chloroacetic acid (ClCH2COOH) is 11.0% ionized. Using this information, calculate [ClCH2COO-], [H+], [ClCH2COOH], and Ka for chloroacetic acid.

FREE Expert Solution

We’re being asked to calculate the equilibrium constant of a weak acid if a 0.100 M solution of chloroacetic acid is 11.0% ionized.


Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). 


The dissociation of chloroacetic acid is as follows:

ClCH2COOH(aq) + H2O(l) H3O+(aq) + ClCH2COO(aq)


Recall that the percent ionization is given by:


% ionization=[H3O+][HA]initial×100


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Problem Details

A 0.100 M solution of chloroacetic acid (ClCH2COOH) is 11.0% ionized. Using this information, calculate [ClCH2COO-], [H+], [ClCH2COOH], and Ka for chloroacetic acid.

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