Problem: Find the pH of each of the following solutions of mixtures of acids.0.155 M in HNO2 and 9.0×10−2 M in HNO3

FREE Expert Solution

We’re being asked to calculate the pH of a mixture of acids containing 0.155 M in HNO2 and 9.0×10−2 M in HNO3.


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


The dissociation of the acids are as follows:


  • HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq)
  • HNO3(aq) + H2O(l)  H3O+(aq)NO3-(aq)

**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 concentration of H3Ofrom strong acid.
Step 2. Construct an ICE table for each weak acid to solve for the concentration of H3Ofrom the weak acid.
Step 3. Solve for the pH of the mixture.


Recall that pH is given by:


pH=-log[H3O+]

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Problem Details

Find the pH of each of the following solutions of mixtures of acids.

0.155 M in HNO2 and 9.0×10−2 M in HNO3

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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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