Can you measure the pH of non aqueous solutions?

Question

For example, acetic acid in a solvent.

Answer 1

pH is a measure of the acidity of a solution in terms of activity of hydrogen (H+). For dilute solutions, however, it is convenient to substitute the activity of the hydrogen ions with the molarity (mol/L) of the hydrogen ions (however, this is not necessarily accurate at higher concentrations [1][2]).

In aqueous systems, the hydrogen ion activity is dictated by the dissociation constant of water (Kw = 1.011 × 10−14 M2 at 25 °C) and interactions with other ions in solution. Due to this dissociation constant, a neutral solution (hydrogen ion activity equals hydroxide ion activity) has a pH of approximately 7. Aqueous solutions with pH values lower than 7 are considered acidic, while pH values higher than 7 are considered basic.

Answer 2

sure. a pH ingredient is additionally desperate for reliable compounds (by and massive organic and organic pastes *semi-solids) with out water present day in any respect. the only dificulty is that the standard 0-14 pH scale won't nessisarilly be usable because it quite is for aqueos recommendations... and a few of the common mesuring approaches would would desire to get replaced for extra technical approaches. to my information the backside pH & optimal pHs of gear go previous + and - 28 on the pH scale.

Answer 3

yes. a pH factor can also be determined for solid compounds (primarily organic pastes *semi-solids) with no water present at all.

The only dificulty is that the standard 0-14 pH scale may not nessisarilly be usable as that is for aqueos solutions... and some of the typical mesuring methods would have to be changed for more technical methods.

to my knowledge the lowest pH & highest pHs of substances go beyond + and - 28 on the pH scale.

Answer 4

Lancenigo di Villorba (TV), Italy

As you wrote, it is well-known that pH is conventional estimate for acidity's containt in aqueous solutions...pH is a mathematical expression of this containt (e.g. |molar concentration of H+ ions, |H+|).
See this reaction, the "water's auto-protolysis"
n H2O <---> ([n-1] H2O)H+ + OH-
which I wrote in this feature because it is known H+ is an ion who binds several water molecules. This reaction lies itself in a chemical equilibrium..it belong to "solvent's dissociation".
Analogous it is behaviour of acetic acid (if it is pure).
Now, reaction of "solvent's dissociation"
2 CH3COOH <---> CH3COOH2+ + CH3COO-
It is necessarily that you suppose molar concentration of protoned species might be molar concentration of hydrogen ions, since it is yet supposed that the latters exist not as free form but H+ are bound to some substance (e.g. Bronsted-Lewis bases).

WARNING! I wrote you about pure solvents as "protic species", that is compounds whom molecule show hydrogen atom bound to electronegative one (e.g. O or N, see Pauling's electronegativity). Sulphur dioxide (e.g. SO2) belong not to "protic compounds", nonetheless it is a useful solvent if it is pure liquid (under-pressure conditions). Its "solvent dissociation" is not leading to hydrogen ions
2 SO2 <---> SO++ + SO3--
as you see.
Moreover, few drops of water need to modify chemical equilibria and oxydril ions finally appear
SO3-- + 2 H2O <----> H2SO3 + 2 OH-
SO++ + 2 OH- <---> H2SO3
I shown oxydril ions but not hydrogen ones because water acts like a base versus sulphur's dioxide. Same reasoning values in case of acetic acid.

I hope this helps you.

Answer 5

No, to determine the pH value you have to determine the concentration of (H3O+) in the solution, and there is no (H3O+) ions in non aqueous soluttions.

Answer 6

Yes,If there will be H+ ion present in them.

It is simple, we have to find the concentration of the H+ ion and put it in the foumula
pH = - log (H+)

Answer 7

i would reduce it to a 50% hci saline solution measure the ph then just double it.