We’re being asked to calculate the pH of a mixture of weak acids containing 5.5×10−2 M in acetic acid and 5.5×10−2 M in hydrocyanic acid.
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of each weak acid is as follows:
**chemical formula of each weak acid can be found in textbooks/online
To solve for the pH of the mixture, we need to do these steps:
Step 1. Determine the weak acid with a higher acid dissociation constant, Ka
Step 2. Construct an ICE table for each weak acid to solve for the concentration of H3O+ from each weak acid
Step 3. Solve for the pH of the mixture
Recall that pH is given by:
Find the pH of each of the following solutions of mixtures of acids.
5.5×10−2 M in acetic acid and 5.5×10−2 M in hydrocyanic acid
Frequently Asked Questions
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.