what are colligative properties
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COLLIGATIVE PROPERTIES DEFINITION
Colligative properties are properties of solutions that depend on the number of particles in a volume of solvent (the concentration) and not on the mass or identity of the solute particles. Colligative properties are also affected by temperature. Calculation of the properties only works perfectly for ideal solutions. In practice, this means the equations for colligative properties should only be applied to dilute real solutions when a nonvolatile solute is dissolved in a volatile liquid solvent. For any given solute to solvent mass ratio, any colligative property is inversely proportional to the molar mass of the solute. The word "colligative" comes from the Latin word colligatus, which means "bound together", referring to how the properties of a solvent are bound to the concentration of solute in a solution.
HOW COLLIGATIVE PROPERTIES WORK
When a solute is added to a solvent to make a solution the dissolved particles displace some of the solvent in the liquid phase. This reduces the concentration of the solvent per unit of volume. In a dilute solution, it doesn't matter what the particles are, just how many of them are present. So, for example, dissolving CaCl2 completely would yield three particles (one calcium ion and two chloride ions), while dissolving NaCl would only produce two particles (a sodium ion and a chloride ion). The calcium chloride would have a greater effect on colligative properties than the table salt.
This is why calcium chloride is an effective de-icing agent at lower temperatures than ordinary salt!
WHAT ARE THE COLLIGATIVE PROPERTIES?
Examples of colligative properties include vapor pressure lowering, freezing point depression, osmotic pressure, and boiling point elevation. For example, adding a pinch of salt to a cup of water makes the water freeze at a lower temperature than it normally would, boiling at a higher temperature, have a lower vapor pressure, and changes its osmotic pressure.
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Colligative Properties of Solutions
Definition and Examples of Colligative Properties
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Boiling point elevation is a colligative property. Dorling Kindersley / Getty Images
by Anne Marie Helmenstine, Ph.D.
Updated July 01, 2017
CITE
COLLIGATIVE PROPERTIES DEFINITION
Colligative properties are properties of solutions that depend on the number of particles in a volume of solvent (the concentration) and not on the mass or identity of the solute particles. Colligative properties are also affected by temperature. Calculation of the properties only works perfectly for ideal solutions. In practice, this means the equations for colligative properties should only be applied to dilute real solutions when a nonvolatile solute is dissolved in a volatile liquid solvent.
For any given solute to solvent mass ratio, any colligative property is inversely proportional to the molar mass of the solute. The word "colligative" comes from the Latin word colligatus, which means "bound together", referring to how the properties of a solvent are bound to the concentration of solute in a solution.
HOW COLLIGATIVE PROPERTIES WORK
When a solute is added to a solvent to make a solution the dissolved particles displace some of the solvent in the liquid phase. This reduces the concentration of the solvent per unit of volume. In a dilute solution, it doesn't matter what the particles are, just how many of them are present. So, for example, dissolving CaCl2 completely would yield three particles (one calcium ion and two chloride ions), while dissolving NaCl would only produce two particles (a sodium ion and a chloride ion). The calcium chloride would have a greater effect on colligative properties than the table salt.
This is why calcium chloride is an effective de-icing agent at lower temperatures than ordinary salt!
WHAT ARE THE COLLIGATIVE PROPERTIES?
Examples of colligative properties include vapor pressure lowering, freezing point depression, osmotic pressure, and boiling point elevation. For example, adding a pinch of salt to a cup of water makes the water freeze at a lower temperature than it normally would, boiling at a higher temperature, have a lower vapor pressure, and changes its osmotic pressure.
FREEZING POINT DEPRESSION AND BOILING POINT ELEVATION EQUATIONS
Freezing Point Depression may be calculated from the equation:
ΔT = iKfm
where
ΔT = Change in temperature in °C
i = van 't Hoff factor
Kf = molal freezing point depression constant or cryoscopic constant in °C kg/mol
m = molality of the solute in mol solute/kg solvent
Boiling point elevation may be calculated from the equation:
ΔT = Kbm
where
Kb = ebullioscopic constant (0.52°C kg/mol for water)
m = molality of the solute in mol solute/kg solvent
Colligative properties are properties of solutions that depend on the number of particles in a volume of solvent (the concentration) and not on the mass or identity of the solute particles. Colligative properties are also affected by temperature. Calculation of the properties only works perfectly for ideal solutions. In practice, this means the equations for colligative properties should only be applied to dilute real solutions when a nonvolatile solute is dissolved in a volatile liquid solvent. For any given solute to solvent mass ratio, any colligative property is inversely proportional to the molar mass of the solute. The word "colligative" comes from the Latin word colligatus, which means "bound together", referring to how the properties of a solvent are bound to the concentration of solute in a solution.
HOW COLLIGATIVE PROPERTIES WORK
When a solute is added to a solvent to make a solution the dissolved particles displace some of the solvent in the liquid phase. This reduces the concentration of the solvent per unit of volume. In a dilute solution, it doesn't matter what the particles are, just how many of them are present. So, for example, dissolving CaCl2 completely would yield three particles (one calcium ion and two chloride ions), while dissolving NaCl would only produce two particles (a sodium ion and a chloride ion). The calcium chloride would have a greater effect on colligative properties than the table salt.
This is why calcium chloride is an effective de-icing agent at lower temperatures than ordinary salt!
WHAT ARE THE COLLIGATIVE PROPERTIES?
Examples of colligative properties include vapor pressure lowering, freezing point depression, osmotic pressure, and boiling point elevation. For example, adding a pinch of salt to a cup of water makes the water freeze at a lower temperature than it normally would, boiling at a higher temperature, have a lower vapor pressure, and changes its osmotic pressure.
Science, Tech, Math › Science
Colligative Properties of Solutions
Definition and Examples of Colligative Properties
Share
Boiling point elevation is a colligative property. Dorling Kindersley / Getty Images
by Anne Marie Helmenstine, Ph.D.
Updated July 01, 2017
CITE
COLLIGATIVE PROPERTIES DEFINITION
Colligative properties are properties of solutions that depend on the number of particles in a volume of solvent (the concentration) and not on the mass or identity of the solute particles. Colligative properties are also affected by temperature. Calculation of the properties only works perfectly for ideal solutions. In practice, this means the equations for colligative properties should only be applied to dilute real solutions when a nonvolatile solute is dissolved in a volatile liquid solvent.
For any given solute to solvent mass ratio, any colligative property is inversely proportional to the molar mass of the solute. The word "colligative" comes from the Latin word colligatus, which means "bound together", referring to how the properties of a solvent are bound to the concentration of solute in a solution.
HOW COLLIGATIVE PROPERTIES WORK
When a solute is added to a solvent to make a solution the dissolved particles displace some of the solvent in the liquid phase. This reduces the concentration of the solvent per unit of volume. In a dilute solution, it doesn't matter what the particles are, just how many of them are present. So, for example, dissolving CaCl2 completely would yield three particles (one calcium ion and two chloride ions), while dissolving NaCl would only produce two particles (a sodium ion and a chloride ion). The calcium chloride would have a greater effect on colligative properties than the table salt.
This is why calcium chloride is an effective de-icing agent at lower temperatures than ordinary salt!
WHAT ARE THE COLLIGATIVE PROPERTIES?
Examples of colligative properties include vapor pressure lowering, freezing point depression, osmotic pressure, and boiling point elevation. For example, adding a pinch of salt to a cup of water makes the water freeze at a lower temperature than it normally would, boiling at a higher temperature, have a lower vapor pressure, and changes its osmotic pressure.
FREEZING POINT DEPRESSION AND BOILING POINT ELEVATION EQUATIONS
Freezing Point Depression may be calculated from the equation:
ΔT = iKfm
where
ΔT = Change in temperature in °C
i = van 't Hoff factor
Kf = molal freezing point depression constant or cryoscopic constant in °C kg/mol
m = molality of the solute in mol solute/kg solvent
Boiling point elevation may be calculated from the equation:
ΔT = Kbm
where
Kb = ebullioscopic constant (0.52°C kg/mol for water)
m = molality of the solute in mol solute/kg solvent
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What are colligative properties
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Colligative properties are those properties of dilute solutions of non volatile solutes whose value depend upon the number of solute particles irrespective of their nature relative to the total numbef of particles present in the solution
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