Sure, to solve this question, we need to follow several steps.
First, we start by calculating the pOH of the solution. This is because we know that at 25 degrees celsius, the pH and pOH of a solution add up to 14. Given that the pH is 8.7272, the pOH would be calculated as 14 - 8.7272 = 5.2728.
Next, we need to determine the concentration of the OH- ions in the solution. The pOH is the negative base-10 logarithm (log10) of the OH- ion concentration. Therefore, by taking the inverse of the log10, we can calculate the OH- ion concentration as 10 ^ -5.2728, which equals 5.335805618460332e-06 moles/L (or Molarity).
Having determined the concentration of the OH- ions in solution, we can calculate the number of moles of KF needed to produce this solution. Based on the problem statement, we know that in a solution of KF, the number of moles of KF is equal to the number of moles of OH-.
So, to produce a 1.00 L solution with the given pOH, we need the same mole number of KF. Since the volume is in liters, the mole amount of KF needed is the same as the molarity, which is 5.335805618460332e-06 mol/L.
Therefore, 5.335805618460332e-06 moles of KF would be needed to create a 1.00 L solution with a pH of 8.7272, given that the volume does not change as the solution is formed.
In conclusion, by knowing the pH of the solution and some basic chemistry principles, we were able to calculate the number of moles of KF needed to produce this solution.