Problem: A 0.100 M solution of chloroacetic acid (ClCH2 COOH) is 11.0% ionized.Using this information, calculate 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.


Recall that the percent ionization is given by:


% ionization=[H3O+][HA]initial×100


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)


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Problem Details

A 0.100 M solution of chloroacetic acid (ClCH2 COOH) is 11.0% ionized.

Using this information, calculate Ka for chloroacetic acid.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

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