would the pKa = pH in this case? because the ml and concentrations are equal in each scenario? If you plug it in the formula, I think your logs would equal 0 because it would be log(1) = 0. My asnwer is not coming out right though.
No. See my response below.
I think I told you the answer for the acetic acid/salt buffered solution was 4.23.
To determine whether pKa = pH in a specific case, you need to consider the context and the molecular species involved. The relationship between pKa and pH depends on the ionization state of an acid or base in a given solution.
In general, when the pH of a solution is equal to the pKa of an acid or base, it means that exactly half of the acid/base molecules have ionized and half are in their non-ionized form. At this point, the concentrations of the ionized and non-ionized forms are equal.
However, if you have ml and concentrations that are equal across different scenarios, it does not necessarily mean that pKa will always equal pH. The pKa is determined by the inherent properties of the acid or base, while the pH depends on the concentration of hydrogen ions in solution.
To correctly evaluate the situation, you cannot rely solely on the formula log(1) = 0. The formula you are referring to might be the Henderson-Hasselbalch equation, which relates the pH and pKa of a weak acid or base in a solution:
pH = pKa + log([A-]/[HA])
In this equation, [A-] represents the concentration of the ionized form and [HA] represents the concentration of the non-ionized form of the acid or base. The use of this equation requires knowing the values of both [A-] and [HA].
To determine whether pKa = pH, you need to know the specific acid or base you are dealing with, as well as the concentrations of the ionized and non-ionized forms. If those values are not provided, it is not possible to determine if pKa = pH solely based on equal ml and concentrations.