Problem: Find the pH and percent ionization of each HF solution. (Ka for HF is 6.8 x 10-4.)Find the percent dissociation of a 0.270 M HF solution.

🤓 Based on our data, we think this question is relevant for Professor Carbonaro's class at TOWSON.

FREE Expert Solution

Recall that the percent ionization is given by:


% ionization=[H+][HA]initial×100



The dissociation of HA is as follows:

HF(aq) + H2O(l)  H3O+(aq) + F(aq)Ka = 6.8 × 10–4


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Problem Details

Find the pH and percent ionization of each HF solution. (Ka for HF is 6.8 x 10-4.)

Find the percent dissociation of a 0.270 M HF solution.

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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 Carbonaro's class at TOWSON.