The quantity pH is defined in terms of the activity of hydrogen(1+) ions (hydrogen
ions) in solution:
where
is the activity of hydrogen ion (hydrogen 1+) in aqueous solution,
,
is the activity
coefficient of
(molality basis) at molality
,
and
is the standard molality.
Notes:
- pH cannot be measured independently because calculation of the activity involves the
activity coefficient of a single ion. Thus it can be regarded only as a notional definition.
- The establishment of primary pH standards requires the application of the concept of 'primary method of measurement', assuring full traceability of the results of all measurements and their uncertainties. Any limitation in the
theory of determination of experimental variables must be included in the estimated
uncertainty of the method.
- The primary method for measurement of pH involves the use of a cell without transference,
known as the Harned cell:
Pt(s) |
H2(g) |
Buffer S, Cl−(aq) |
AgCl(s) |
Ag(s)
The equation for this cell can be rearranged to give:
where
is the potential difference of the cell and
is the known standard potential of the
AgCl | Ag
electrode. Measurements of
as a function of
are made and the quantity
(called the acidity function) is found by extrapolation to
.
The value of
is calculated using the Bates–Guggenheim convention based on Debye–Hückel theory. Then
is calculated and identified as
,
where
signifies primary standard. The uncertainties in the two estimates are typically
in
and
in pH.
Materials for primary standard buffers must also meet the appropriate requirements for reference materials, including
chemical purity and stability, and applicability of the Bates–Guggenheim convention for the estimation of
This convention requires that the ionic strength be
.
Primary standard buffers should also lead to small liquid junction potentials when used in cells with liquid junctions. Secondary standards,
,
are also available, but carry a greater uncertainty in measured values.
- Practical pH measurements generally use cells with liquid junctions in which, consequently,
liquid junction potentials,
,
are present. Measurements of pH are not normally performed using the
Pt|H2
electrode, but rather the glass (or other
H+
- selective) electrode, whose response factor
(
)
usually deviates from the Nernst slope. The associated uncertainties are significantly
larger than those associated with fundamental measurements using the Harned cell.
Nonetheless, incorporation of the uncertainties for the primary method, and for all
subsequent measurements, permits the uncertainties for all procedures to be linked
to the primary standards by an unbroken chain of comparisons.
- Reference values for standards in
D2O
and aqueous-organic solvent mixtures exist.
Source:
PAC, 1997, 69, 1007
(Reference value standards and primary standards for pH measurements in D2O and aqueousorganic
solvent mixtures: New accessions and assessments (Technical Report))
on page 1007
PAC, 1996, 68, 957
(Glossary of terms in quantities and units in Clinical Chemistry (IUPAC-IFCC Recommendations
1996))
on page 986
See also:
PAC, 2002, 74, 2169
(Measurement of pH. Definition, standards, and procedures (IUPAC Recommendations 2002))
on page 2169
PAC, 1990, 62, 2167
(Glossary of atmospheric chemistry terms (Recommendations 1990))
on page 2205
PAC, 1984, 56, 567
(Physicochemical quantities and units in clinical chemistry with special emphasis
on activities and activity coefficients (Recommendations 1983))
on page 569
Cite as:
IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by
A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997).
XML on-line corrected version: http://goldbook.iupac.org (2006-) created by M. Nic,
J. Jirat, B. Kosata; updates compiled by A. Jenkins. ISBN 0-9678550-9-8.
https://doi.org/10.1351/goldbook.
