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  2. Van 't Hoff factor - Wikipedia

    en.wikipedia.org/wiki/Van_'t_Hoff_factor

    The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved and the concentration of a substance as calculated from its mass. For most non- electrolytes dissolved in water, the van 't Hoff factor is essentially 1.

  3. Van 't Hoff equation - Wikipedia

    en.wikipedia.org/wiki/Van_'t_Hoff_equation

    The Van 't Hoff equation relates the change in the equilibrium constant, K eq, of a chemical reaction to the change in temperature, T, given the standard enthalpy change, Δ r H ⊖, for the process. The subscript r {\displaystyle r} means "reaction" and the superscript ⊖ {\displaystyle \ominus } means "standard".

  4. Osmotic coefficient - Wikipedia

    en.wikipedia.org/wiki/Osmotic_coefficient

    where is the chemical potential of the pure solvent and is the chemical potential of the solvent in a solution, M A is its molar mass, x A its mole fraction, R the gas constant and T the temperature in Kelvin. [1] The latter osmotic coefficient is sometimes called the rational osmotic coefficient. The values for the two definitions are ...

  5. List of dimensionless quantities - Wikipedia

    en.wikipedia.org/wiki/List_of_dimensionless...

    The tables also include pure numbers, dimensionless ratios, or dimensionless physical constants; these topics are discussed in the article. ... van 't Hoff factor: i

  6. Colligative properties - Wikipedia

    en.wikipedia.org/wiki/Colligative_properties

    Here K f is the cryoscopic constant (equal to 1.86 °C kg/mol for the freezing point of water), i is the van 't Hoff factor, and m the molality (in mol/kg). This predicts the melting of ice by road salt. In the liquid solution, the solvent is diluted by the addition of a solute, so that fewer molecules are available to freeze.

  7. Ebullioscopic constant - Wikipedia

    en.wikipedia.org/wiki/Ebullioscopic_constant

    i is the van 't Hoff factor, the number of particles the solute splits into or forms when dissolved. b is the molality of the solution. A formula to compute the ebullioscopic constant is: [2] = R is the ideal gas constant. M is the molar mass of the solvent.

  8. Osmotic pressure - Wikipedia

    en.wikipedia.org/wiki/Osmotic_pressure

    where is osmotic pressure, i is the dimensionless van 't Hoff index, c is the molar concentration of solute, R is the ideal gas constant, and T is the absolute temperature (usually in kelvins). This formula applies when the solute concentration is sufficiently low that the solution can be treated as an ideal solution.

  9. Cryoscopic constant - Wikipedia

    en.wikipedia.org/wiki/Cryoscopic_constant

    i is the van ‘t Hoff factor, the number of particles the solute splits into or forms when dissolved; b is the molality of the solution. Through cryoscopy, a known constant can be used to calculate an unknown molar mass. The term "cryoscopy" means "freezing measurement" in Greek.