What is the PH of 0.0100M H2SO4?
I know that is a diprotic acid and you do ICE and compare with each Ka value but I am not sure if I am setting it up the right way or doing the correct thing.
It is true that H2SO4 is a diprotic acid but one is completely ionized while the second one has a k (k2 = about 10^-2). Why don't you show us how you have it set up?
To determine the pH of a solution, you need to know its concentration of hydrogen ions (H+). In the case of sulfuric acid (H2SO4), you can use the concentration of the acid to calculate the concentration of hydrogen ions.
Step 1: Understand the dissociation of sulfuric acid (H2SO4).
When sulfuric acid dissociates in water, it donates two protons (H+) to the solution, resulting in the formation of bisulfate (HSO4-) ions. So, one molecule of H2SO4 produces two hydrogen ions.
Step 2: Calculate the concentration of hydrogen ions.
If the concentration of H2SO4 is 0.0100 M, then the concentration of hydrogen ions will be twice that value, since each molecule of H2SO4 produces two hydrogen ions.
Concentration of H+ ions = 2 * 0.0100 M = 0.0200 M.
Step 3: Calculate the pH.
The pH is a logarithmic scale that measures the concentration of hydrogen ions in a solution. The formula to calculate pH is:
pH = -log[H+]
Using the concentration of hydrogen ions calculated earlier (0.0200 M), you can plug it into the formula to calculate the pH:
pH = -log(0.0200) ≈ 1.70
Therefore, the pH of a 0.0100 M H2SO4 solution is approximately 1.70.