Problem: A certain weak acid, HA, has a Ka value of 8.4 x 10 -7. Calculate the percent ionization of HA in a 0.10 M solution.

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FREE Expert Solution

We’re being asked to calculate the percent ionization of a 0.10 M aqueous solution of HA.

Recall that the percent ionization is given by:

We know the initial concentration of HA, 0.10 M. We just need to find the concentration of H+ at equilibrium.

Since HA has a low Ka value, it’s a weak acid.

Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).

The dissociation of HA is as follows:

HA(aq) + H2O(l)  H3O+(aq) + A(aq); Ka = 8.4 × 10–7

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Problem Details

A certain weak acid, HA, has a Ka value of 8.4 x 10 -7. Calculate the percent ionization of HA in a 0.10 M solution.

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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Our tutors rated the difficulty of A certain weak acid, HA, has a Ka value of 8.4 x 10 -7. Calc... as medium difficulty.

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