ISO 31-8

Quantity			Unit		Remarks
Name	Symbol	Definition	Name	Symbol
relative atomic mass	Ar	Ratio of the average mass per atom of an element to 1/12 of the mass of an atom of the nuclide 12C	one	1	Formerly called atomic/molecular weight. Example: Ar(Cl) = 35.453. Both quantities depend on the nuclidic composition.
relative molecular mass	Mr	Ratio of the average mass per molecule or specified entity of a substance to 1/12 of the mass of an atom of the nuclide 12C
number of molecules or other elementary entities	N	Number of molecules or other elementary entities in a system	one	1
amount of substance	n, (ν)		mole	mol	The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kg of 12C. When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specific groups of such particles. The definition applies to unbound atoms of 12C, at rest and in their ground state.
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In the tables of quantities and their units, the ISO 31-8 standard shows symbols for substances as subscripts (e.g., c_B, w_B, p_B). It also notes that it is generally advisable to put symbols for substances and their states in parentheses on the same line, as in c(H₂SO₄).

This annex contains a list of elements by atomic number, giving the names and standard symbols of the chemical elements from atomic number 1 (hydrogen, H) to 109 (unnilennium, Une).

The list given in ISO 31-8:1992 was quoted from the 1998 IUPAC "Green Book" Quantities, Units and Symbols in Physical Chemistry and adds in some cases in parentheses the Latin name for information, where the standard symbol has no relation to the English name of the element. Since the 1992 edition of the standard was published, some elements with atomic number above 103 have been discovered and renamed.

Symbols for chemical elements shall be written in roman (upright) type. The symbol is not followed by a full-stop.

Examples:

H He C Ca

Attached subscripts or superscripts specifying a nucleotide or molecule have the following meanings and positions:

• The nucleon number (mass number) is shown in the left superscript position (e.g., ¹⁴N)
• The number of atoms of a nucleotide is shown in the right subscript position (e.g., ¹⁴N₂)
• The proton number (atomic number) may be indicated in the left subscript position (e.g., ₆₄Gd)
• If necessary, a state of ionization or an excited state may be indicated in the right superscript position (e.g., state of ionization Na⁺)

pH is defined operationally as follows. For a solution X, first measure the electromotive force E_X of the galvanic cell

reference electrode | concentrated solution of KCl | solution X | H₂ | Pt

and then also measure the electromotive force E_S of a galvanic cell that differs from the above one only by the replacement of the solution X of unknown pH, pH(X), by a solution S of a known standard pH, pH(S). Then obtain the pH of X as

pH(X) = pH(S) + (E_S − E_X) F / (RT ln 10)

where

F is the Faraday constant;

R is the molar gas constant;

T is the thermodynamic temperature.

Defined this way, pH is a quantity of dimension 1, that is it has no unit. Values pH(S) for a range of standard solutions S are listed in Definitions of pH scales, standard reference values, measurement of pH, and related terminology. Pure Appl. Chem. (1985), 57, pp 531–542, where further details can be found.

pH has no fundamental meaning; its official definition is a practical one. However, in the restricted range of dilute aqueous solutions having amount-of-substance concentrations less than 0.1 mol/L, and being neither strongly alkaline nor strongly acidic (2 < pH < 12), the definition is such that

pH = −log₁₀[c(H⁺) y₁ / (1 mol/L)] ± 0.02

where c(H⁺) denotes the amount-of-substance concentration of hydrogen ion H⁺ and y₁ denotes the activity coefficient of a typical uni-univalent electrolyte in the solution.