In chemistry, the<unk> ole <unk>   is a non-SI unit of measurement that defines the number of moles of a chemical compound that contribute to a solution's<unk> otic pressure.<unk>  is a measure of the<unk> oles of solute per liter of solution, while the<unk>  is a measure of the<unk> oles of solute per kilogram of solvent.  Molarity and<unk>  are not commonly used in<unk> ometry because they are temperature dependent; that is, water changes its volume with temperature. However, if the concentration is very low,<unk>  and<unk>  are considered equivalent. In calculations for these two measurements, salts are presumed to dissociate into their component ions. For example, a mole of glucose in solution is one<unk> ole, whereas a mole of sodium chloride in solution is two<unk> oles (one mole of sodium and one mole of chloride). Both sodium and chloride ions affect the<unk> otic pressure of the solution.
The equation to determine the<unk>  of a solution is given by
O
s
m
=
ϕ
 
n
C
{\displaystyle<unk> =\phi \ nC}
where
Φ is the<unk> otic coefficient, which accounts for the degree of non-ideality of the solution. In the simplest case it is the degree of dissociation of the solute. Then, Φ is between 0 and 1 where 1 indicates 100% dissociation. However, Φ can also be larger than 1 (e.g. for sucrose). For salts, electrostatic effects cause Φ to be smaller than 1 even if 100% dissociation occurs (see Debye-Hückel equation).
n is the number of particles (ions) into which a molecule dissociates. For example: Glucose equals 1 and NaCl equals 2.
C is the molal concentration of the solution
The units are<unk> /kg<unk>  can be measured using an<unk> ometer which measures colligative properties, such as Freezing-point depression, Vapor pressure, or Boiling-point elevation.
Osmolarity
Aqueous humour
Ionic liquid
Anion gap
Albumin
Density
Fluency
Uric acid