Although the wikipedia page on Hydronium indicates a pKa of −1.74, I noticed in the discussion of this page that the subject seems debated (cf. http://en.wikipedia.org/wiki/Talk:Hydronium#pKa.3F) since alternative (apparently more rigorous) reasoning leads to pKa=0 for HX3OX+.
Also, many demonstrations lead to pKa and pKb of 15.74 for HX2O and thus, using Kw=[HX+][OHX−]=10−14, give pKa and pKb of −1.74 for HX+ and OHX− respectively. But those demonstrations seem to make use of the concentration [HX2O]=55.56 mol/L instead of the activity aHX2O=1 (for a solvent) in the equilibrium constant of the reactions.
So it seems to me that the pKa of HX3OX+ must be equal to 0.
Is this question still debated?
PS1:
To add details about the question, the debate in the references mentioned in the discussion on the wikipedia page as well as in the link provided by Nicolau Saker Neto bellow seems to boil down to the coexistence of two different definitions for the equilibrium constant:
- one based on the activities of the compounds
- the other derived from the 'mass action law' and which thereby uses the molar fractions of the compounds
Reading through the Callen (Thermodynamics and an Introduction to Thermostatistics) gives me the impression that the derivation from the mass action law of an equilibrium constant involving molar fractions is based on the assumption of an ideal fluid. However, it is precisely the departure from ideality that seems to justify the use of activities instead of molar fractions. Is that correct?
PS2:
Another point, which I have not looked in details yet, seems to be a debate about the possibility to apply the definition for Ka to the water molecules HX2O considering that they are not a highly diluted solute since they constitute the solvent. Is this a valid issue and should then the acidity of HX3OX+/HX2O be determined in another solvent than HX2O to be compared with the other acids?
Answer
The controversy surrounding the pKa of hydronium mostly arises from the definition of Ka or lack thereof.
There is no IUPAC definition of pKa or Ka.
The closest IUPAC defined term is the standard equilibrium constant, which can be denoted as K∘ or just K.
Physical chemistry texts such as Levine and respected works such Bates's "Determination of pH — Theory and Practice" define K∘a of an acid in water as:
a(AX−)a(HX3OX+)a(HA)a(HX2O)
Where a is activity.
Substituting that the acid is HX3OX+:
a(HX2O)a(HX3OX+)a(HX3OX+)a(HX2O)=1
and of course −log(1)=0.
The number −1.74 that some quote for the hydronium pKa comes from:
- omitting the activity of water from the denominator of the K∘a definition (equation (1)); and
- taking the concentration of water (about 55.5 M) as the Ka of HX3OX+.
With that, one obtains the pKa as −log(55.5)=−1.74. For example, Levine even has the −1.74 value in a figure comparing the pKa's of various acids, but has a footnote explaining that the value for HX3OX+ is based upon the alternative pKa definition.
However, revisiting the analysis that K∘a=1 is probably the most authoritative paper on this issue:
New point of view on the meaning and on the values of Ka(H3O+, H2O) and Kb(H2O, OH-) pairs in water, which insists that
HX2O+HX3OX+−⇀↽−HX3OX++HX2O
"does not correspond to an actual chemical process" and therefore "it is not legitimate" to extend the concept of K∘a to HX3OX+ in water.
The article goes on to say that only by studying the Ka of HX3OX+ in another solvent such as ethanol can HX3OX+ be compared to other acids.
The pKa of HX3OX+ in ethanol is 0.3 and pKa values are 1.0±0.3 units lower in water than in ethanol, so the article suggests a pKa of −0.7 for HX3OX+ in water, for the purpose of comparison to other acids.