# Problem: When a 0.0538 M solution of an unknown weak acid, HA, is made, only 3.57% acid ionized. What is the Ka of the unknown acid?

94% (57 ratings)
###### FREE Expert Solution

We’re being asked to calculate the equilibrium constant of HA if a 0.0538 M solution is 3.57% ionized.

Recall that the percent ionization 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 HNO2 is as follows:

HA(aq) + H2O(l)  H3O+(aq) + A(aq)

94% (57 ratings) ###### Problem Details

When a 0.0538 M solution of an unknown weak acid, HA, is made, only 3.57% acid ionized. What is the Ka of the unknown acid?

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 is the difficulty of this problem?

Our tutors rated the difficulty ofWhen a 0.0538 M solution of an unknown weak acid, HA, is mad...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Jules took 4 minutes and 38 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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