We’re being asked to calculate the equilibrium concentration of chloroacetic acid (ClCH2COOH) if the percent dissociation of 0.100 M ClCH2COOH is 11.0%.
Recall that the percent dissociation is given by:
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of ClCH2COOH is as follows:
ClCH2COOH(aq) + H2O(l) ⇌ H3O+(aq) + ClCH2COO–(aq)
A 0.100 M solution of chloroacetic acid (ClCH2 COOH) is 11.0% ionized.
Using this information, calculate [ClCH2 COOH] 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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