What is the pH of a solution that is 0.0 100 M in HClO and 0.0300 M in NaClO
Have you studied the Henderson-Hasselbalch equation? That is used for solutions that are buffed solutions.
pH = pKa + log(base)/(acid)
NaClO is the base; HClO is the acid.
To find the pH of a solution, you need to know the concentration of the hydrogen ions (H+) in the solution. In this case, the concentration of H+ comes from the dissociation of HClO.
The dissociation of HClO can be represented by the equation:
HClO ⇌ H+ + ClO-
Given that the solution is 0.0100 M in HClO, we can assume that the concentration of H+ is also 0.0100 M. This is because, in the dissociation of HClO, equal amounts of H+ and ClO- are produced.
Now, to calculate the pH, you can use the formula:
pH = -log[H+]
Substituting the concentration of H+ into the formula, we get:
pH = -log(0.0100)
Using a calculator, you can find that the pH is approximately 2.00 for this solution.
It's important to note that the presence of NaClO (sodium hypochlorite) does not affect the concentration of H+ ions and therefore, does not play a role in determining the pH of the solution.