🤓 Based on our data, we think this question is relevant for Professor Cheek's class at AUSTINCC.
We are being asked to calculate the Ka for a 0.15 M chloroacetic acid (ClCH2COOH).
Step 1. Equilibrium reaction: ClCH2COOH(aq) + H2O(l) ⇌ H3O+(aq) + ClCH2COO-(aq)
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.
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Based on our data, we think this problem is relevant for Professor Cheek's class at AUSTINCC.