The pH of a sample of rain is found to be 3.3. Calculate the percentage of HSO4- that is ionized in this sample, given that the acid dissociation constant for the second stage of ionization of H2SO4 is 1.2E-2.© BrainMass Inc. brainmass.com September 23, 2018, 7:06 am ad1c9bdddf - https://brainmass.com/chemistry/chemical-measures-of-environmental-indicators/ph-rainwater-diprotonic-acids-22977
The solution is attached below in two files. the files are identical in content, only differ in format. The first is in MS Word XP Format, while the other is in Adobe pdf format. Therefore you can choose the format that is most suitable to you.
Here are the steps to solve the problem:
1. Find the final [H] ions using the pH. denote this concentration x.
2. Assume ...
The solution (2 pages in length) shows how to seal with dissociation of acids that can contribute two protons, such as sulphuric acid. The solution shows how not to fall into the common trap of assuming full dissociation right in the first reaction.