It is defined aste depression in freezing point of solution containing non-volatile solute.wen molality is equal to 1 and is caled molal depression constant
i.e. Tf=kf . m
The freezing point depression constant for water is 1.86 degrees Celsius per molal.
The freezing point depression of a solution is given by the equation ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the cryoscopic constant, and m is the molality of the solution. With the molality (m) of 3.23 molal and the cryoscopic constant for water (Kf) being approximately 1.86 ºC kg/mol, you can calculate the freezing point depression.
This is a colligative property which does not depend on the nature of solute is the molal boiling point elevation constant or ebullioscopic constant of the solvent.
The freezing-point depression constant (Kf) of benzoic acid is 6.22 °C/m, and for salicylic acid, it is 6.93 °C/m. These values indicate how much the freezing point of a solvent will decrease for each molal concentration of the solute.
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The freezing point depression constant for water is 1.86 degrees Celsius per molal.
The freezing point depression of a solution is given by the equation ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the cryoscopic constant, and m is the molality of the solution. With the molality (m) of 3.23 molal and the cryoscopic constant for water (Kf) being approximately 1.86 ºC kg/mol, you can calculate the freezing point depression.
This is a colligative property which does not depend on the nature of solute is the molal boiling point elevation constant or ebullioscopic constant of the solvent.
The molar freezing point constant (Kf) is a physical constant that represents the amount by which the freezing point of a solvent is lowered for each mole of solute dissolved in it. It is specific to each solvent and is used in calculating the freezing point depression in colligative properties.
To determine which solution has a lower freezing point, you need the concentrations of solute in each solution and their respective properties (molal freezing point depression constants). The solution with the higher concentration of solute and lower molal freezing point depression constant will have the lower freezing point.
The freezing-point depression constant (Kf) of benzoic acid is 6.22 °C/m, and for salicylic acid, it is 6.93 °C/m. These values indicate how much the freezing point of a solvent will decrease for each molal concentration of the solute.
"http://wiki.answers.com/Q/The_molal_freezing_point_constant_kf_is_a_property_of_the_solvent_not_the_solute_What_does_this_say_about_the_fact_that_freezing_point_depends_on_the_amount_of_solute_rather_than_solute%27s_nature"
The freezing point depression constant for water is 1.86 degrees Celsius per molal. This means that for every mole of solute added to water, the freezing point of water decreases by 1.86 degrees Celsius. The presence of solute particles disrupts the formation of ice crystals, lowering the freezing point of the solution compared to pure water.
The Kf (freezing point depression constant) of water is approximately 1.86 °C/m. This means that for every 1 molal solution of a solute in water, the freezing point of water is expected to decrease by 1.86°C.
Constant molal overflow is a term used in binary distillation. When a 2 component mixture is being separated in a distillation column,the assumption of constant molal overflow means assuming that both components have the same enthalpy. It assumes that one mole of component 1 when it condenses will vapourise 1 mole of component 2,also assumes no heat loss from the column. Can be wildly innacurate,particularly with separating organic solvents,and water. Water has a uniquely high enthalpy,often 5-6 times higer than the organic solvents.
-1.6°C and -3.0°C, depending on the molal freezing point depression constant for calcium chloride-water solution.
-5.58 C