When and how a solution become an ideal solution?
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Ideal soln.
An ideal solution, in chemistry, is a mixture that follows Raoult’s law, which states the vapor pressure above a solution is directly proportional to the mole fraction of the solvent. A vapor pressure lowering is commonly observed in mixtures of solvents and non-volatile solutes, or substances dissolved in a solvent. An ideal solution of similar compounds can use differences in volatility to separate the compounds by fractional distillation.
Liquids are continually vaporizing and condensing. A liquid in an open container placed into a closed system will vaporize until the rates of condensation from gas to liquid and vaporization from liquid to gas are equal. The liquid is then in equilibrium with its vapor. Vapor pressure is the part of the total pressure due to the vaporized liquid. The vapor pressure of an ideal solution is a measure of the concentrations of the molecules in the solution.
Raoult’s law is followed by most dilute solutions. If the solute and solvent are dissimilar, significant variations from an ideal solution are observed as solute concentrations increase. When the solute is nonvolatile, the vapor pressure of the solvent is actually decreased as solute concentrations increase. This effect, called vapor-pressure lowering, does not occur in an ideal solution.
Raoult’s law
Definition: A solution that obeys Raoult’s law for all concentrations is an
ideal solution (the vapor does not have to behave as an ideal gas)
An ideal solution, in chemistry, is a mixture that follows Raoult’s law, which states the vapor pressure above a solution is directly proportional to the mole fraction of the solvent. A vapor pressure lowering is commonly observed in mixtures of solvents and non-volatile solutes, or substances dissolved in a solvent. An ideal solution of similar compounds can use differences in volatility to separate the compounds by fractional distillation.
Liquids are continually vaporizing and condensing. A liquid in an open container placed into a closed system will vaporize until the rates of condensation from gas to liquid and vaporization from liquid to gas are equal. The liquid is then in equilibrium with its vapor. Vapor pressure is the part of the total pressure due to the vaporized liquid. The vapor pressure of an ideal solution is a measure of the concentrations of the molecules in the solution.
Raoult’s law is followed by most dilute solutions. If the solute and solvent are dissimilar, significant variations from an ideal solution are observed as solute concentrations increase. When the solute is nonvolatile, the vapor pressure of the solvent is actually decreased as solute concentrations increase. This effect, called vapor-pressure lowering, does not occur in an ideal solution.
Raoult’s law
Definition: A solution that obeys Raoult’s law for all concentrations is an
ideal solution (the vapor does not have to behave as an ideal gas)
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