HBrO3 has a Ka of 3.6 x 10^-6. What is the pH of a 2.0M solution?
This is worked the same way as the propanoic acid problem below; however, I really don't believe the Ka value. I thought HBrO3 was a strong acid (ionized 100%). The literature says that is so.
ooh okay, thank you DrBob222!
To find the pH of a solution, we need to know the concentration of the hydrogen ions (H+). In this case, the given information is the Ka value, which represents the acid dissociation constant of HBrO3.
The Ka expression for a weak acid, such as HBrO3, is:
Ka = [H+][BrO3-] / [HBrO3]
Since we have the Ka value but not the concentration of H+, we need to use some algebra to rearrange the equation and solve for [H+].
[H+] = (Ka * [HBrO3]) / [BrO3-]
Now, substitute the given values into the equation:
[H+] = (3.6 x 10^-6 * 2.0) / 2.0
[H+] = 3.6 x 10^-6 M
Now that we have the concentration of H+, we can find the pH. The pH is calculated using the equation:
pH = -log[H+]
Substituting the value of [H+] we found:
pH = -log(3.6 x 10^-6)
Using a calculator, we can find that the pH of the 2.0M HBrO3 solution is approximately 5.44.