Search results
Results From The WOW.Com Content Network
In the International System of Units (SI), the coherent unit for molar concentration is mol/m 3. However, most chemical literature traditionally uses mol/dm 3, which is the same as mol/L. This traditional unit is often called a molar and denoted by the letter M, for example: 1 mol/m 3 = 10 −3 mol/dm 3 = 10 −3 mol/L = 10 −3 M = 1 mM = 1 ...
20 mM: neutrinos during a supernova, 1 AU from the core (10 58 over 10 s) [18] 44.6 mM: pure ideal gas at 0 °C and 101.325 kPa [19] 10 −1: dM: 140 mM: sodium ions in blood plasma [10] 480 mM: sodium ions in seawater [20] 10 0: M: 1 M: standard state concentration for defining thermodynamic activity [21] 10 1: daM 17.5 M pure (glacial) acetic ...
The SI unit of molar absorption coefficient is the square metre per mole (m 2 /mol), but in practice, quantities are usually expressed in terms of M −1 ⋅cm −1 or L⋅mol −1 ⋅cm −1 (the latter two units are both equal to 0.1 m 2 /mol). In older literature, the cm 2 /mol is sometimes used; 1 M −1 ⋅cm −1 equals 1000 cm 2 /mol.
Normality is defined as the molar concentration divided by an equivalence factor . Since the definition of the equivalence factor depends on context (which reaction is being studied), the International Union of Pure and Applied Chemistry and National Institute of Standards and Technology discourage the use of normality.
mole per cubic metre: mol/m 3: molarity, amount of substance concentration: m −3 ⋅mol cubic metre per mole: m 3 /mol molar volume: m 3 ⋅mol −1: joule per kelvin mole: J/(K⋅mol) molar heat capacity, molar entropy m 2 ⋅kg⋅s −2 ⋅K −1 ⋅mol −1: joule per mole: J/mol molar energy: m 2 ⋅kg⋅s −2 ⋅mol −1: siemens square ...
Metric units are units based on the metre, gram or second and decimal (power of ten) multiples or sub-multiples of these. According to Schadow and McDonald, [ 1 ] metric units, in general, are those units "defined 'in the spirit' of the metric system, that emerged in late 18th century France and was rapidly adopted by scientists and engineers.
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.
Molecular weight (M.W.) (for molecular compounds) and formula weight (F.W.) (for non-molecular compounds), are older terms for what is now more correctly called the relative molar mass (M r). [8] This is a dimensionless quantity (i.e., a pure number, without units) equal to the molar mass divided by the molar mass constant. [notes 1]