Problem: A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid?

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FREE Expert Solution

We are being asked to calculate the Ka for a 0.15 M chloroacetic acid (ClCH2COOH).


Step 1. Equilibrium reaction:        ClCH2COOH(aq) + H2O(l) ā‡Œ  H3O+(aq) + ClCH2COO-(aq)


Ka=productsreactants=[H3O+][ClCH2COO-][ClCH2COOH]

Ka=(x)(x)0.15-xKa=x20.15-x

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Problem Details

A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this 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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Cheek's class at AUSTINCC.