Material true concentration or partial pressure {partial molar quantity} depends on other-substance concentrations or partial pressures, because having different substances contributes more disorder to system. Substances interact, because system has total pressure, temperature, and concentration.
Material true concentration or partial pressure {chemical potential, solution}| {free energy per mole} depends on partial molar quantity, because having different substances contributes more disorder to system. Substances interact, because system has total pressure, temperature, and concentration that distribute among substances. Substance partial molar Gibbs free energy is partial derivative of free energy with substance moles, if temperature, pressure, and other-substance amounts are constant.
Gas solubility in liquid is proportional to partial pressure of gas in contact with liquid {Henry's law} {Henry law}.
Gases in mixtures independently contribute pressure {partial pressure} to total gas pressure {law of partial pressures}.
Solute-vapor partial pressure above solution equals solute mole fraction times pure-solute vapor pressure {Raoult's law} {Raoult law}.
Pure substances have molar quantities, but mixtures have partial molar quantities, which depend on material moles divided by total moles, the mole fraction. Solution properties {colligative property}|, such as partial pressures, boiling point elevation, freezing point depression, osmotic pressure, solubility, volatility, and surface tension, can depend on solute mole fraction. Partial molar quantities are interdependent, because mole fraction total must be one.
Solutions have higher boiling point than pure solvent {boiling point elevation}|, because solute molecules are heavier than solvent molecules and have lower volatility. If liquid includes impurities that are less volatile than liquid, liquid boils only at higher temperature. Salt in water raises boiling temperature. Mixture boiling point is higher, because mixtures are more random, so difference between liquid and gas is less. Immiscible substances lower boiling point, because both vapor pressures add to increase pressure. In boiling-point elevation, temperature change dT equals constant k times molality M: dT = K*M. People know constants for solutes and solvents.
Solutions have lower freezing point than pure solvent {freezing point depression}|, because solute molecules are impurities in solvent crystals and so make crystals harder to form. In freezing-point depression, temperature change dT equals constant k times molality M: dT = K*M. People know constants for solutes and solvents.
5-Chemistry-Inorganic-Phase-Solution
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Date Modified: 2022.0225